When given 20.76 moles of H2 and plenty of O2, you can make 20.76 moles of H2O.
To determine how many moles of H2O can be produced from 20.76 moles of H2 and plenty of O2, we'll use the balanced chemical equation provided: 2H2 + 1O2 --> 2H2O.
Step 1: Identify the limiting reactant. In this case, we have plenty of O2, so H2 is the limiting reactant.
Step 2: Determine the mole ratio between the limiting reactant (H2) and the product (H2O). According to the balanced equation, the mole ratio is 2H2 to 2H2O, or 1:1.
Step 3: Calculate the moles of H2O produced. Since the mole ratio is 1:1, the number of moles of H2O produced will be the same as the number of moles of H2 available. Thus, you can produce 20.76 moles of H2O.
In summary, when given 20.76 moles of H2 and plenty of O2, you can make 20.76 moles of H2O.
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Use this equation to answer the following two questions.
2 Mg + O2 → 2Mgo
5) If you have 7. 8 moles of magnesium and 4. 7 moles of oxygen, which one 2 points
will be the EXCESS reactant if they are allowed to react until ithe reaction
stops?
magnesium
oxygen
O magnesium oxide
The excess reactant will be oxygen.
To determine the excess reactant, we need to compare the amount of moles of each reactant to the stoichiometry of the balanced equation. The stoichiometric ratio between magnesium and oxygen is 2:1, which means that for every 2 moles of magnesium, 1 mole of oxygen is required for complete reaction.
In this case, we have 7.8 moles of magnesium and 4.7 moles of oxygen. Based on the stoichiometric ratio, we can see that 7.8 moles of magnesium require 3.9 moles of oxygen (2 moles of oxygen for every 1 mole of magnesium). Since we only have 4.7 moles of oxygen, it is the limiting reactant, and magnesium will be in excess.
Therefore, after the reaction is complete, all of the magnesium will be consumed, and some oxygen will be left over. The product of the reaction will be 7.8 moles of magnesium oxide.
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(marking brainliest!) given the following bond energies:
h-h = 436 kj/mol
i-i = 151 kj/mol
h-i = 297 kj/mol
calculate the enthalpy change for the following reaction:
h-h + i-i ---> 2h-i
-choices are attached!
Bond energy refers to the amount of energy required to break a bond between two atoms. This energy is required because bonds are formed when electrons are shared between atoms, and breaking a bond requires energy to be put into the system to overcome the electrostatic forces holding the atoms together.
In the case of the reaction given, h-h + i-i ---> 2h-i, we are asked to determine the energy change associated with breaking the H-H and I-I bonds and forming two new H-I bonds. To do this, we can use the bond energies of the individual bonds involved.
According to a standard table of bond energies, the H-H bond has a bond energy of 432 kJ/mol, while the I-I bond has a bond energy of 149 kJ/mol. The H-I bond has a bond energy of 436 kJ/mol. Using these values, we can calculate the energy change for the reaction as follows:
(2 x H-I bond energy) - (H-H bond energy + I-I bond energy)
= (2 x 436 kJ/mol) - (432 kJ/mol + 149 kJ/mol)
= 293 kJ/mol
So the energy change for the reaction is 293 kJ/mol. This means that the reaction is exothermic, as energy is released when the bonds are formed. This energy can be used to do work or heat up the surroundings.
Finally, you mentioned the term "marking brainliest". I assume you are referring to the "Brainliest Answer" feature on certain online platforms, where the person who asks a question can choose which answer they found most helpful or accurate. If this is the case, I hope my answer has been helpful and informative!
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A piece of unknown metal with a mass of 23.8 g is heated to 100.0°C and is dropped into 50.0 g of water at 24.0°C. The final temperature is 32.5°C. What is the specific heat of the metal?
The metal has a specific heat of 0.385 J/g°C.
To solve for the specific heat of the metal, we need to use the equation:
Q = mCΔT
where Q is the heat transferred, m is the mass of the substance, C is the specific heat, and ΔT is the change in temperature.
In this case, the heat transferred from the metal to the water can be calculated as:
Q = mcΔT
where c is the specific heat of water (4.184 J/g°C) and ΔT is the change in temperature of the water (from 24.0°C to 32.5°C).
Q = (50.0 g)(4.184 J/g°C)(32.5°C - 24.0°C)
Q = 1743.8 J
The heat transferred from the metal to the water is equal to the heat absorbed by the metal:
Q = mCΔT
where m is the mass of the metal and ΔT is the change in temperature of the metal (from 100.0°C to 32.5°C).
1743.8 J = (23.8 g)C(100.0°C - 32.5°C)
C = 0.385 J/g°C
Therefore, the specific heat of the metal is 0.385 J/g°C.
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If a gas occupies 30 L at STP, what would be the volume if the temperature was raised to 323. 15K ?
At STP, typically defined as a temperature of 0°C (273.15K) and a pressure of 1 atm, the volume of a gas is equal to 30 L.
When the temperature of the gas is increased, the kinetic energy of the gas particles increases, causing them to move more quickly and expand. This expansion of the gas increases its volume.
Using the ideal gas law, the new volume of the gas can be calculated by multiplying the original volume by the ratio of the new temperature (323.15K) to the original temperature (273.15K) and raising that to the power of 1/273.15.
In this case, the new volume of the gas is 33.53 L. In conclusion, when the temperature of a gas is raised, its volume increases.
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Calculate the pH of 0. 10 M solution of hypochlorous acid, HOCl, Ka = 2. 9 x 10-8
The pH of a 0.10 M solution of hypochlorous acid with a Ka value of 2.9 x 10-8 is approximately 4.77.
Hypochlorous acid, also known as HOCl, is a weak acid that can dissociate in water to form hydrogen ions (H+) and hypochlorite ions (OCl-). The dissociation constant of HOCl, also known as Ka, is a measure of the strength of the acid. In this case, the Ka value of HOCl is 2.9 x 10-8.
To calculate the pH of a 0.10 M solution of HOCl, we need to use the Ka value and the expression for the equilibrium constant:
Ka = [H+][OCl-]/[HOCl]
We can assume that the concentration of HOCl at equilibrium is equal to the initial concentration, since it is a weak acid and only partially dissociates. We also know that the concentration of H+ is equal to the concentration of the acid that dissociated, so we can substitute these values into the expression:
Ka = [H+]^2/[HOCl]
[H+]^2 = Ka x [HOCl]
[H+]^2 = 2.9 x 10-8 x 0.10
[H+] = 1.7 x 10-5 M
Now that we have calculated the concentration of H+, we can use the pH equation to find the pH:
pH = -log[H+]
pH = -log(1.7 x 10-5)
pH = 4.77
Therefore, the pH of a 0.10 M solution of hypochlorous acid with a Ka value of 2.9 x 10-8 is approximately 4.77.
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This is the chemical formula for cassiterite (tin ore):
sno2
a geochemist has determined by measurements that there are 3.316 moles of tin in a sample of cassiterite. how many moles of oxygen are in the sample?
be sure your answer has the correct number of significant digits.
The chemical formula for cassiterite is SnO2, which means that there are two moles of oxygen for every one mole of tin in the compound.
Given that there are 3.316 moles of tin in the sample, we can use the mole ratio to determine the number of moles of oxygen:
1 mole Sn : 2 moles O
3.316 moles Sn : x moles O
x = (3.316 moles Sn) x (2 moles O / 1 mole Sn) = 6.632 moles O
Therefore, there are 6.632 moles of oxygen in the sample of cassiterite.
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What mass in grams of hydrogen gas is produced if 20.0 mol of zn are added to excess hydrochloric acid according to the equation
zn(s) +2hcl(aq) --> zncl₂(aq) + h₂(g)?
40.32 grams of hydrogen gas will be produced.
According to the balanced chemical equation:
1 mol of Zn reacts with 2 mol of HCl to produce 1 mol of H2
So if 20.0 mol of Zn is added to excess HCl, all the Zn will react to produce:
20.0 mol Zn × 1 mol H2 / 1 mol Zn = 20.0 mol H2
To calculate the mass of H2 produced, we need to use its molar mass, which is 2.016 g/mol:
Mass of H2 = number of moles of H2 × molar mass of H2
Mass of H2 = 20.0 mol × 2.016 g/mol
Mass of H2 = 40.32 g
Therefore, 40.32 grams of hydrogen gas will be produced.
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A helium filled balloon has a volume of 50. 0L at 25⁰ C and 1. 00 atm. What volume will it have at 0. 855 atm and 10. 0⁰ C?
A helium filled balloon has a volume of 50. 0L at 25⁰C and 1. 00 atm. 43.6 L will it have at 0. 855 atm and 10. 0⁰C.
To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas. The formula is:
[tex]\frac{{P_1V_1}}{{T_1}} = \frac{{P_2V_2}}{{T_2}}[/tex]
Where P1, V1, and T1 are the initial conditions, and P2, V2, and T2 are the final conditions. Plugging in the given values, we get:
[tex]\left(\frac{{1.00 , \text{atm} \cdot 50.0 , \text{L}}}{{298 , \text{K}}}\right) = \left(\frac{{0.855 , \text{atm} \cdot V2}}{{283 , \text{K}}}\right)[/tex]
Solving for V2, we get:
[tex]V2 = \frac{{1.00 , \text{atm} \cdot 50.0 , \text{L}}}{{298 , \text{K}}} \times \frac{{283 , \text{K}}}{{0.855 , \text{atm}}} = 43.6 , \text{L}[/tex]
Therefore, the helium-filled balloon will have a volume of 43.6 L at 0.855 atm and 10.0⁰C.
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a student is asked to transfer 0.03 ml of a concentrated solution in order to accurately dilute the solution to 0.020 m. which measuring tool would you choose to obtain the needed volume of the original concentrated solution?
To accurately measure a very small volume of liquid like 0.03 ml, a micropipette would be the most appropriate measuring tool to use.
What is micropipette?A micropipette is a laboratory instrument commonly used in biology, chemistry, and other related fields to accurately and precisely measure and transfer small volumes of liquids. It typically operates through a piston-driven air displacement system, allowing for very precise measurements in the microliter (μL) or even nanoliter (nL) range.
Micropipettes are commonly used in applications such as DNA sequencing, PCR, and protein assays, where precise and accurate liquid handling is essential for accurate results.
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.if you dilute 0.20 l of a 3.5 m solution of lici to 0.90 l, determine the new concentration of the
solution.
The new concentration of the solution can be calculated using the dilution formula, which states that the initial concentration multiplied by the initial volume (V1) is equal to the new concentration multiplied by the new volume (V2).
In this case, the equation would be: (3.5M)(0.20L) = (xM)(0.90L). Solving for x, we get the new concentration of the solution as 3.17M.
In other words, when a 3.5M solution of lici is diluted from 0.20L to 0.90L, the new concentration of the solution is 3.17M. This is because when the volume of a solution is increased, the concentration of the solution decreases proportionately.
Thus, when the volume of the solution is increased by a factor of four and a half, the concentration of the solution is reduced by the same factor.
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a generic salt, ab3, has a molar mass of 305 g/mol and a solubility of 4.30 g/l at 25 °c. ab3(s)↽−−⇀a3 (aq) 3b−(aq) what is the ksp of this salt at 25 °c?
The dissociation reaction for the salt AB3 is:
AB3(s) ↔ A3+(aq) + 3B-(aq)
Let's assume the solubility of AB3 in water at 25 °C is x mol/L. Then, the equilibrium concentrations of A3+ and B- can be expressed as x and 3x, respectively.
The Ksp expression for AB3 is:
Ksp = [A3+][B-]^3 = x(3x)^3 = 27x^4
The molar mass of AB3 is 305 g/mol, so the number of moles in 4.30 g (the solubility) is:
n = 4.30 g / 305 g/mol = 0.0141 mol/L
Therefore, the solubility of AB3 at 25 °C is:
x = 0.0141 mol/L
Substituting this into the Ksp expression:
Ksp = 27x^4 = 27(0.0141)^4 = 5.6 x 10^-9
Therefore, the Ksp of AB3 at 25 °C is 5.6 x 10^-9.
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8250 J of heat is applied to a piece of aluminum, causing a 40. 0 °C increase in its temperature. The specific heat of aluminum is 0. 9025 J/g ·°C. What is the mass of the aluminum?
We can use the formula for calculating heat:
Q = m × c × ΔT
where Q is the amount of heat transferred, m is the mass of the substance, c is its specific heat, and ΔT is the change in temperature.
Plugging in the given values, we get:
8250 J = m × 0.9025 J/g ·°C × 40.0 °C
Simplifying, we get:
8250 J = m × 36.1 J/g
Solving for m, we get:
m = 8250 J ÷ 36.1 J/g
m ≈ 228.26 g
Therefore, the mass of the aluminum is approximately 228.26 g.
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Calculate the mass of ethanol produced if 500.0 grams of glucose reacts completely
Answer:
The chemical equation for the conversion of glucose to ethanol during fermentation is:
C6H12O6 → 2C2H5OH + 2CO2
From the equation, we can see that for every mole of glucose (C6H12O6) that reacts, two moles of ethanol (C2H5OH) are produced. The molar mass of glucose is 180.16 g/mol, while the molar mass of ethanol is 46.07 g/mol.
Therefore, to calculate the mass of ethanol produced from 500.0 grams of glucose, we need to convert the mass of glucose to moles, then use the mole ratio from the balanced chemical equation to calculate the moles of ethanol produced, and finally convert the moles of ethanol to mass.
Step 1: Convert the mass of glucose to moles
Number of moles of glucose = mass of glucose ÷ molar mass of glucose
Number of moles of glucose = 500.0 g ÷ 180.16 g/mol
Number of moles of glucose = 2.776 mol
Step 2: Use the mole ratio to calculate the moles of ethanol produced
From the balanced equation, 1 mol of glucose produces 2 mol of ethanol
Therefore, 2.776 mol of glucose will produce:
2.776 mol glucose × (2 mol ethanol / 1 mol glucose) = 5.552 mol ethanol
Step 3: Convert moles of ethanol to mass
Mass of ethanol = number of moles of ethanol × molar mass of ethanol
Mass of ethanol = 5.552 mol × 46.07 g/mol
Mass of ethanol = 255.2 g
Therefore, 500.0 grams of glucose will produce 255.2 grams of ethanol during fermentation.
I hope this helps you! :)))
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which of these atoms has the most stable nuclei? Ra
Po
Rn
Au
Answer:
Rn has the most stable nucleus
Rn (Radon) has the most stable nuclei due to its closer proximity to the magic number 126.
Option (3) is correct.
The stability of a nucleus depends on the arrangement of protons and neutrons within it. Certain numbers of protons and neutrons result in more stable nuclei. These numbers are known as magic numbers, and they correspond to complete nuclear shells.
Among the given atoms:
Ra (Radium) has 88 protons and a varying number of neutrons.
Po (Polonium) has 84 protons and a varying number of neutrons.
Rn (Radon) has 86 protons and a varying number of neutrons.
Au (Gold) has 79 protons and a varying number of neutrons.
Radon (Rn) has the most stable nuclei because it is closer to the magic number 126 for neutrons. Elements with magic numbers of protons or neutrons tend to have more stable configurations, making Rn the most stable among the options provided.
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What could be a third quantum number of a 2p3 electron in phosphorus,
152252p 3s23p3?
A. M = -1
B. M = 3
c. M = 2
D. M = -2
The third quantum number of a 2p³ electron in phosphorus is M = -1. Option A is the answer.
The electronic configuration of phosphorus is 1s²2s²2p⁶3s²3p³. The 2p subshell has three orbitals, which can hold up to six electrons. The three orbitals are labeled as 2p_x, 2p_y, and 2p_z, where each orbital can hold a maximum of two electrons with opposite spins.
The three quantum numbers that define the state of an electron in an atom are n, l, and m. Here, n represents the principal quantum number, l represents the azimuthal quantum number, and m represents the magnetic quantum number.
The values of l for the 2p subshell are 1, and the possible values of m for l = 1 are -1, 0, and 1. The electron in question is in the 2p subshell, so its value of l is 1. Since the possible values of m for this electron are -1, 0, and 1, we can rule out options B, C, and D. Therefore, the correct answer is A, M = -1. Hence, option A is the answer.
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The heating was stopped before all of the liquid can evaporate how will this affect the results of the experiment
The heating process is often used in experiments to evaporate liquid and concentrate the sample. If the heating was stopped before all of the liquid could evaporate, this would have a significant impact on the results of the experiment.
Firstly, the concentration of the sample would be lower than expected. This could affect the accuracy and precision of any measurements or analyses performed on the sample.
For example, if the sample was being analyzed for the presence of a certain compound, the lower concentration may make it more difficult to detect or quantify the compound accurately.
Additionally, the incomplete evaporation of the liquid could lead to contamination of the sample. If the liquid is not fully evaporated, there may be impurities or other compounds present in the final sample that were not accounted for in the experimental design. This could affect the validity of the results and the interpretation of the data.
In summary, the premature stopping of heating in an experiment could lead to lower sample concentration and potential contamination, both of which could have significant implications for the results and conclusions drawn from the experiment.
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PLEASEEE HELP MEEEE!!! How many grams of iron (III) oxide will be produced if 4300 kJ of heat energy is released?
4 Fe+ 3 O2 → 2 Fe2O3
ΔH = -1652 kJ
Answer: 652.8 g of iron (III) oxide produced.
Explanation:
To calculate the amount of iron (III) oxide produced, we use the enthalpy change of the reaction to determine the amount of energy released and convert it to moles of Fe2O3 produced. Then, we multiply by the molar mass of Fe2O3 to obtain the mass of Fe2O3 produced. Using these calculations, we get 652.8 g of iron (III) oxide produced.
580.84 grams of iron (III) oxide will be produced when 4300 kJ of heat energy is released.
Given:
Enthalpy change (∆H) value: ∆H = -1652 kJ
Amount of heat energy released: 4300 kJ
From the balanced equation:
4Fe + 3O₂ → 2 Fe₂O₃
The molar ratio between Fe₂O₃ and ∆H is 2:1652 kJ.
To find the molar amount of Fe₂O₃ produced, the following calculation:
[tex]4300 \times \frac{2}{1652}[/tex] = 5.20 mol Fe₂O₃
To convert this into grams, it is required to multiply the molar amount by the molar mass of Fe₂O₃:
5.20 × 2 × 55.85 = 580.84 g
Therefore, 580.84 grams of iron (III) oxide will be produced when 4300 kJ of heat energy is released.
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A sample of 140 g of an unstable isotope goes through 4 half-lives. how much of the parent isotope will be left at that time?
After four half-lives, 12.5 grams of the parent isotope will be left in a sample that originally contained 140 grams of an unstable isotope.
The amount of the parent isotope remaining after a certain number of half-lives can be calculated using the formula:
Remaining amount = Initial amount x (1/2)^(number of half-lives)
For this problem, the initial amount of the unstable isotope is 140 g, and it goes through 4 half-lives.
One half-life is the time it takes for half of the original sample to decay, and the number of half-lives is equal to the total time elapsed divided by the length of one half-life.
If we know the half-life of the isotope, we can find the total time elapsed. Let's assume the half-life of the isotope is 10 days.
After 10 days, half of the initial sample will remain:
Remaining amount = 140 g x (1/2)¹ = 70 g
After another 10 days (20 days total), half of the remaining sample will decay:
Remaining amount = 70 g x (1/2)¹ = 35 g
After another 10 days (30 days total), half of the remaining sample will decay again:
Remaining amount = 35 g x (1/2)¹ = 17.5 g
After another 10 days (40 days total), half of the remaining sample will decay once more:
Remaining amount = 17.5 g x (1/2)¹ = 8.75 g
Therefore, after 4 half-lives (40 days), there will be approximately 8.75 g of the parent isotope remaining.
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There is a transfer of chemical energy from producers to consumers. What is this chemical energy?.
The chemical energy referred to in the transfer from producers to consumers is the energy stored in the organic molecules synthesized by the producers during photosynthesis.
Producers, such as plants and algae, use energy from sunlight to convert carbon dioxide and water into glucose and other organic molecules through the process of photosynthesis. The energy from the sunlight is converted into chemical energy and stored in the organic molecules.
Consumers, such as herbivores and carnivores, obtain this stored chemical energy by consuming the organic molecules synthesized by the producers. The organic molecules are broken down during cellular respiration to release the stored chemical energy, which is used by the consumer to power its cellular processes.
Thus, the transfer of chemical energy from producers to consumers is a fundamental process in the food chain, and it is essential for the maintenance of life on earth.
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Calculate the standard molar entropy change for the combustion of methane gas using s° values from standard thermodynamic tables. Assume that liquid water is one of the products.
The standard molar entropy change for the combustion of methane gas is 9.9 J/(mol·K).
The balanced equation for the combustion of methane is:
[tex]CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)[/tex]
The standard molar entropy change can be calculated using the formula:
ΔS° = ΣS°(products) - ΣS°(reactants)
The standard molar entropy values for the species involved in the reaction are:
ΔS°(CH4) = 186.3 J/(mol·K)
ΔS°(O2) = 205.0 J/(mol·K)
ΔS°(CO2) = 213.6 J/(mol·K)
ΔS°(H2O(l)) = 69.9 J/(mol·K)
Using these values, we can calculate the standard molar entropy change:
ΔS° = [ΔS°(CO2) + ΔS°(2H2O(l))] - [ΔS°(CH4) + ΔS°(2O2(g))]
ΔS° = [(213.6 J/(mol·K)) + (2 × 69.9 J/(mol·K))] - [(186.3 J/(mol·K)) + (2 × 205.0 J/(mol·K))]
ΔS° = 9.9 J/(mol·K)
Therefore, the standard molar entropy change for the combustion of methane gas is 9.9 J/(mol·K).
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14. Lab Analysis: You forgot to label your chemicals and do not know whether your unknown solution is strontium nitrate or magnesium nitrate. You use the solutions potassium carbonate and potassium sulfate in order to determine your mistake. unknown + potassium carbonate & unknown + potassium sulfate . Write the complete balanced molecular equation(s) below of the reaction(s) that occurred, including the states of matter. HINT: Try writing ALL possible reactions that could have been created, and then decide which reactions actually occurred.
Unknown + Potassium Carbonate → Potassium Nitrate + Unknown Carbonate
[tex]Sr(NO_3)_2[/tex] + [tex]K_2CO_3[/tex] → [tex]2KNO_3[/tex] + [tex]SrCO_3[/tex] (if the unknown is strontium nitrate)
[tex]Mg(NO_3)_2[/tex]+ [tex]K_2CO_3[/tex] → [tex]2KNO_3[/tex] + [tex]MgCO_3[/tex] (if the unknown is magnesium nitrate)
Here are the balanced molecular equations for the reactions that could have occurred between the unknown solution (either strontium nitrate or magnesium nitrate) and potassium carbonate and potassium sulfate: Unknown + potassium carbonate → potassium nitrate + magnesium or strontium carbonate (depending on the unknown)
Unknown + potassium sulfate → potassium nitrate + magnesium or strontium sulfate (depending on the unknown)
Unknown + Potassium Sulfate → Potassium Nitrate + Unknown Sulfate
[tex]Sr(NO_3)_2[/tex] + [tex]K_2SO_4[/tex] → [tex]2KNO_3[/tex] + [tex]SrSO_4[/tex] (if the unknown is strontium nitrate)
[tex]Mg(NO_3)_2[/tex] + [tex]K_2SO_4[/tex] → [tex]2KNO_3[/tex] + [tex]MgSO_4[/tex] (if the unknown is magnesium nitrate)
To determine which reaction occurred, you would need to observe which products were formed. If [tex]SrCO_3[/tex] or [tex]SrSO_4[/tex] were formed, then the unknown was strontium nitrate.
If [tex]MgCO_3[/tex] or [tex]MgSO_4[/tex] were formed, then the unknown was magnesium nitrate.
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What was the mass of zinc used in the first reaction of the experiment? note: depending on the actual amount of substances dispensed in the lab, there is a range of possible answers. Pick the value that is closest to yours
When zinc reacts with hydrochloric acid, the response bubbles vigorously as hydrogen fueloline is produced.
The manufacturing of a fueloline is likewise an illustration that a chemical response is occurring. When dilute hydrochloric acid is introduced to granulated zinc positioned in a take a look at tube, zinc metallic is transformed to zinc chloride and hydrogen fueloline is developed withinside the response. In the response we will see that a zinc chloride salt is fashioned and hydrogen fueloline is developed. The developed hydrogen fueloline is colourless and odourless. When Zinc granules reacts with Hydrochloric acid ,it'll produces hydrogen fueloline and zinc chloride.
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How many moles of gas occupy 128L at a pressure of 4. 2 atm and a temperature of 382K
To solve this problem, we need to use the ideal gas law which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. Rearranging this equation, we can solve for n by dividing both sides by RT.
n = PV/RT
Now, we can plug in the given values:
n = (4.2 atm)(128 L)/(0.0821 L*atm/mol*K)(382 K)
n = 16.4 moles
Therefore, 16.4 moles of gas occupy 128L at a pressure of 4.2 atm and a temperature of 382K.
It's important to note that the ideal gas law is only applicable to ideal gases, which follow certain assumptions such as having no intermolecular forces and having particles with negligible volume. Real gases can deviate from these assumptions, especially at high pressures and low temperatures. However, for most practical purposes, the ideal gas law provides a good approximation of gas behavior.
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2NaNO3 + PbO → Pb(NO3)2 + Na₂O
What is the mole ratio between
sodium nitrate and sodium oxide?
[?] mol NaNO3
mol Na₂O
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The mole ratio of [tex]NaNO_3[/tex] to [tex]Na_2O[/tex] is 2:1 in the balanced equation
The reasonable compound condition[tex]2NaNO_3 + PbO → Pb(NO_3)_2 + Na_2O[/tex] shows that two moles of sodium nitrate[tex](NaNO_3)[/tex] respond with one mole of lead oxide [tex](PbO)[/tex]to create one mole of sodium oxide [tex]Na_2O[/tex] and one mole of lead nitrate[tex](Pb(NO_3)_2)[/tex] .
In this way, the mole proportion of [tex]NaNO_3[/tex] to [tex]Na_2O[/tex]is 2:1. This intends that for each two moles of [tex]NaNO_3[/tex] utilized, one mole of[tex]Na_2O[/tex] is delivered.
This mole proportion is significant in deciding how much [tex]Na_2O[/tex]delivered when a known measure of [tex]NaNO_3[/tex] is utilized. For instance, assuming we have 2 moles of [tex]NaNO_3[/tex], we can establish that we will deliver 1 mole of [tex]Na_2O[/tex]. Assuming that we have 4 moles of[tex]NaNO_3[/tex] , we will create 2 moles of [tex]Na_2O[/tex].
Knowing the mole proportion likewise permits us to compute the hypothetical yield of [tex]Na_2O[/tex] in light of how much [tex]NaNO_3[/tex] utilized. In any case, practically speaking, the genuine yield might contrast because of exploratory mistake or different elements.
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Answer:
Explanation:
it's 2:1 the top person is right and how i know that is because when i was in school i have my notes so the top of me is right!!! :)
Translate the following balanced chemical equation into words.
Ba3N2(aq) + 6H2O(l) → 3Ba(OH)2(s) + 2NH3(g)
A. Barium nitride reacts with water to yield barium hydroxide and nitrogen trihydride.
B. Barium nitrogen reacts with water to yield barium hydroxide and nitrogen hydrogen.
C. Barium nitrate reacts with water to yield barium oxide and nitrogen hydride.
D. Boron nitride reacts with water to yield boron hydroxide and nitrogen trihydride
Translating the given balanced chemical equation into words : B)Barium nitride reacts with water to yield barium hydroxide and nitrogen hydrogen.
What is Barium nitride ?Barium nitride (Ba₃N₂) is an ionic compound composed of three barium cations (Ba²⁺) and two nitride anions (N³⁻). It is a gray or black crystalline solid that is highly reactive and is used in the production of other chemicals, such as barium azide (Ba(N₃)₂) and barium cyanide (Ba(CN)₂).
Barium nitride can also be used as a reducing agent in the synthesis of metals and alloys. When it reacts with water, it produces barium hydroxide (Ba(OH)₂) and ammonia gas (NH₃).
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Several students performed this experiment without paying adequate attention to the details of the procedure. Briefly explain what effect each of the following procedural changes would have ont the size of the volume-to-temperature ratio calculated by the students. A) One student failed to replenish the boiling water in the boiling-water bath as the flask was being heated. At the end of the 6 min of heating, the boiling water in the bath was only in contact with the lower portion of the flask. B) Following the proper heating of the flask in the boiling water, a student removed the flask from the boiling-water bath but only partially immersed the flask in the ice-water bath during the cooling period. C) A student neglected to close the pinch clamp before removing the flask from the boiling-water bath and immersing it in the ice-water bath. D) One student neglected to measure the volume of the flask before leaving the laboratory. Because the procedure called for a 125-mL Erlenmeyer flask, the student used 125 mL as the volume of the flask
The volume-to-temperature ratio calculated by the students would be affected differently by each procedural change.
A) Failing to replenish boiling water would result in the flask being heated at a lower temperature than intended, leading to a smaller volume-to-temperature ratio.
B) Partially immersing the flask in the ice-water bath would lead to slower cooling and a higher temperature at the end of the cooling period, resulting in a larger volume-to-temperature ratio.
C) Neglecting to close the pinch clamp would allow air to enter the flask during cooling, leading to a lower pressure and a larger volume-to-temperature ratio.
D) Using 125 mL as the volume of the flask would result in an inaccurate volume-to-temperature ratio, as the actual volume of the flask may be different. It is important to measure the volume of the flask accurately to obtain reliable results.
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How many valence electrons does carbon have available for bonding to other atoms?
a. 2
b. 4
c. 6
d. 8
Answer:
4 valence electrons.
Explanation:
Carbon has 4 valence electrons because it is in the 14th group on the Periodic Table.
A buffer solution contains 0.299 m nh4cl and
0.327 m nh3 (ammonia). determine the ph
change when 0.081 mol hi is added to 1.00 l of
the buffer.
ph after addition - ph before addition = ph change
The pH of the buffer solution will decrease by 0.28 units when 0.081 mol of HI is added
To solve this problem, we need to use the Henderson-Hasselbalch equation:
pH = pKa + log([A-]/[HA])
where pKa is the dissociation constant of the acid (NH4+) and A- is the conjugate base (NH3).
First, we need to find the pKa of NH4+ by using the equation:
pKa = -log(Ka)
where Ka is the acid dissociation constant. The Ka for NH4+ is 5.6 x 10^-10, so:
pKa = -log(5.6 x 10^-10) = 9.25
Next, we need to calculate the concentrations of NH4+ and NH3 in the buffer solution after the addition of HI. We can use the equation:
Cfinal = Cinitial + moles added / volume
The volume of the buffer is 1.00 L, and we are adding 0.081 mol of HI, which will react with NH3 according to the equation:
HI + NH3 -> NH4+ + I-
Since the reaction is 1:1, we will end up with 0.081 mol of NH4+ and 0.081 mol of I-. Therefore:
[C(NH4+)]final = [C(NH4+)]initial + 0.081 mol / 1.00 L = 0.380 M
[C(NH3)]final = [C(NH3)]initial - 0.081 mol / 1.00 L = 0.246 M
Now we can calculate the pH of the buffer before and after the addition of HI. Using the Henderson-Hasselbalch equation:
pHbefore = 9.25 + log([NH3] / [NH4+])
= 9.25 + log(0.327 / 0.299)
= 9.25 + 0.074
= 9.32
pHafter = 9.25 + log([NH3]final / [NH4+]final)
= 9.25 + log(0.246 / 0.380)
= 9.25 - 0.210
= 9.04
Finally, we can calculate the pH change:
pHchange = pHafter - pHbefore
= 9.04 - 9.32
= -0.28
Therefore, the pH of the buffer solution will decrease by 0.28 units when 0.081 mol of HI is added.
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Algae produce oxygen. Tiny animals that live in the water eat the algae. Small fish eat the tiny animals, absorb oxygen with their gills, and give off carbon dioxide as waste. Plants use the carbon dioxide to grow.
Which of the following would happen if the algae disappeared?
Plants would lose some of the carbon dioxide they need to grow.
The tiny animals would not have enough food.
Fish would not have enough oxygen.
If the algae disappeared, the tiny animals would not have enough food.
Which of the following would happen if the algae disappeared?Small fish that eat the tiny animals would also run out of food, which might lead to a drop in their number. As a result, less oxygen would be accessible for other organisms and the amount of oxygen the fish produce would decrease.
However, since the plants may still obtain their carbon dioxide from other sources, the loss of the algae would not have a direct impact on them.
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the commonly used rules of thumb used by chemists to make buffers are: a) the two components in the buffer should have about the same concentrations. b) a combination of a weak acid with its salt should be used for a buffer with a ph below 7, while a weak base/salt mixture should be used for a buffer with a ph above 7. c) for acidic buffers, the pka of the weak acid should be close to the ph of the desired buffer. in basic buffers however, the pka of the conjugate acid should be close to the desired ph.
The commonly used rules of thumb used by chemists to make buffers are:
The two components in the buffer should have about the same concentrations.A combination of a weak acid with its salt should be used for a buffer with a pH below 7, while a weak base/salt mixture should be used for a buffer with a pH above 7.For acidic buffers, the pKa of the weak acid should be close to the pH of the desired buffer. In basic buffers, however, the pKa of the conjugate acid should be close to the desired pH.Buffers are solutions that resist changes in pH when small amounts of acid or base are added to them. They are commonly used in many chemical and biological applications. The rules of thumb mentioned above provide guidelines for making effective buffers. Rule a) ensures that there is an adequate amount of buffering capacity in the solution. Rule b) is based on the fact that weak acids have a pH-dependent dissociation constant, and therefore, the pH of a buffer made from a weak acid will be close to the pKa of the weak acid.
Similarly, the pH of a buffer made from a weak base will be close to the pKa of the conjugate acid. Rule c) ensures that the buffering capacity of the solution is optimized by selecting the appropriate pKa value. Overall, these rules of thumb help chemists to design effective buffers that can maintain a stable pH over a range of conditions.
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