Answer:
An experiment is completed where coal is burned in order to heat water and determine the specific heat capacity of coal. q = mcAT a. Water has a specific heat capacity of 4.184 J/g °C. The experiment heated 200 grams of water from 30°C to 100°C. How much energy is absorbed by the water? b. Assume the experiment is a closed system. The experiment used 170 grams of coal and the temperature change is 30°C to 252°C. What is the specific heat of coal?
The ionic compound
MX (s) is formed from the metal
M(s) and the diatomic gas
X₂ (9) at standard conditions. Calculate the lattice energy given the following data:
Sublimation
energy
for
M(8)
Bond
energy
for
X₂(g)
lonization
energy
of
M(g)
Electron
affinity
of
X(g)
Enthalpy
of
198 kJ/mol
of
MX()
142 kJ/mol
525 kJ/mol
-372 kJ/mol
formation-639 kJ/mol
Answer:
mark me brilliant
Explanation:
The lattice energy (ΔHlatt) can be calculated using the following equation:
ΔHlatt = ΔHf - ΔHsub - 1/2 ΔHbond - ΔHIE - ΔHEA
where ΔHf is the enthalpy of formation of the ionic compound, ΔHsub is the sublimation energy of the metal, ΔHbond is the bond energy of the diatomic gas, ΔHIE is the ionization energy of the metal, and ΔHEA is the electron affinity of the gas.
Substituting the given values:
ΔHlatt = (-639 kJ/mol) - (198 kJ/mol) - 1/2(142 kJ/mol) - (525 kJ/mol) - (-372 kJ/mol)
ΔHlatt = -639 kJ/mol - 198 kJ/mol - 71 kJ/mol - 525 kJ/mol + 372 kJ/mol
ΔHlatt = -1061 kJ/mol
Therefore, the lattice energy of the ionic compound MX is -1061 kJ/mol. Note that the negative sign indicates that the process of forming the solid ionic compound from the separate ions is exothermic (releases heat).
If I have 7.70 moles of gas at a pressure of
0.0900 atm and at a temperature of
56.0°C, what is the volume of the container
that the gas is in?
Answer: 2310
Explanation:
PV=nRT therefore V=nRT/
n= 7.70 moles
P= 0.0900atm
T= 56.O°C or 329.15K
R= 0.08206
V= ((7.70)(0.08206)(329.15))/0.0900
V= 2310
Help me I don’t understand this Label the chart. Write “Endothermic” or “Exothermic” Reactions look at the chart below please
Answer:
A is ENDO
B is EXCO
Explanation:
An exothermic process releases heat, causing the temperature of the immediate surroundings to rise. An endothermic process absorbs heat and cools the surroundings.”
K2S is an ionic compound. We need to know the number of particles it breaks into when it dissolves, the Van't Hoff Factor. How many particles does K2S break into in water? Van't Hoff Factor =
van 't Hoff factor for ionic compound [tex]K_{2}[/tex]S is 3.
Define van 't Hoff factor
The van 't Hoff factor is the difference between the concentration of a material determined by its mass and the concentration of particles actually formed when the substance is dissolved. The van 't Hoff factor is virtually 1 for the majority of non-electrolytes dissolved in water.
The van 't Hoff factor for the majority of ionic compounds dissolved in water is equal to the number of discrete ions in the substance's formula unit. Only perfect solutions can claim this as ion pairing occasionally happens in solutions. Only a small portion of the ions are ever coupled and count as a single particle at any given time. In all electrolyte solutions, ion pairing takes place to some extent.
[tex]K_{2}[/tex]S ⇒ 2K+ + S2-
[tex]K_{2}[/tex]S dissolves into 3 particles .
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The Vant Hoff factor as [tex]K_{2}S[/tex] break into in water is 3
What does vant Hoff factor mean?
The ratio of a substance's mass concentration to the concentration of the particles that are produced when it dissolves is known as the Van't Hoff factor. The Van't Hoff factor describes how much a substance associates or dissociates in a solution.
The ratio of the final moles following dissociation or association to the beginning moles before to dissociation or association of an electrolyte in a solution is known as the Van't Hoff factor. The solute's property governs the number of particles, which is independent of the solution's concentration.
[tex]K_{2}S[/tex] ⇒ 2K+ + -[tex]S_{2}[/tex]
[tex]K_{2}S[/tex] dissolves into 3 particles .
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is legislation regardingwaste water necessary? yes or no
Animal fats and vegetable oils are triacylglycerols, or triesters, formed from the reaction
of glycerol (1, 2, 3-propanetriol) with three long-chain fatty acids. One of the methods
used to characterize a fat or an oil is a determination of its saponification number. When
treated with boiling aqueous KOH, an ester is saponified into the parent alcohol and fatty
acids (as carboxylate ions). The saponification number is the number of milligrams of
KOH required to saponify 1.000 g of the fat or oil. In a typical analysis, a 2.085-g sample
of butter is added to 25.00 mL of 0.5131 M KOH. After saponification is complete, the
excess KOH is back titrated with 10.26 mL of 0.5000 M HCl. What is the saponification
number for this sample of butter?
Saponification number = (V × M × F × 56.1) / W
Where:
V = volume of HCl used in the back titration
M = molarity of HCl
F = factor of KOH (which is 1 for pure KOH)
W = weight of the butter sample used in grams
First, we need to calculate the amount of KOH used in the saponification reaction:
0.5131 M KOH = 0.5131 moles KOH / liter
25.00 mL KOH = 0.02500 L KOH
moles KOH used = 0.5131 moles/L × 0.02500 L = 0.0128 moles KOH
Since the saponification reaction is a 1:1 reaction between KOH and the triacylglycerol in the butter sample, the amount of butter used is also 0.0128 moles.
Next, we need to calculate the amount of HCl that reacted with the excess KOH:
0.5000 M HCl = 0.5000 moles HCl / liter
10.26 mL HCl = 0.01026 L HCl
moles HCl used = 0.5000 moles/L × 0.01026 L = 0.00513 moles HCl
Since the reaction between HCl and KOH is also a 1:1 reaction, the moles of KOH that were not used in the saponification reaction is equal to the moles of HCl used in the back titration:
moles KOH not used = moles HCl used = 0.00513 moles HCl
To find the saponification number,
Saponification number = (V × M × F × 56.1) / W
Saponification number = (0.01026 L × 0.5000 moles/L × 1 × 56.1) / 2.085 g
Saponification number = 6.50
Therefore, the saponification number for this sample of butter is 6.50.
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PLEASE HELP IM CONFUSEDD
An atom of xenon has a radius Ixc 108. pm and an average speed in the gas phase at 25°C of 137.m/s. Suppose the speed of a xenon atom at 25°C has been measured to within 0.010%. Calculate the smallest possible length of box inside of which the atom could be known to be located with certainty. Write your answer as a multiple of rye and round it to 2 significant figures. For example, if the smallest box the atom could be in turns out to be 42.0 times the radius of an atom of xenon, you would enter "42.ry" as your answer.
The smallest box that could contain the atom with certainty is 0.85 times the radius of a xenon atom, or 0.85ry, rounded to two significant figures.
How to calculate smallest possible length?The uncertainty principle in quantum mechanics states that it is impossible to simultaneously know the exact position and momentum of a particle. However, it can be calculated with the minimum uncertainty in position based on the uncertainty in velocity.
The uncertainty in velocity is given by:
Δv = (0.010/100) × 137 m/s = 0.0137 m/s
The uncertainty in position is given by:
Δx >= h/(4πmΔv)
where h is Planck's constant, m is the mass of a xenon atom, and Δv is the uncertainty in velocity.
Substituting the values:
Δx >= (6.626 x 10⁻³⁴ J s) / (4π × 131.29 x 10⁻²⁷ kg × 0.0137 m/s)
Δx >= 9.17 x 10⁻¹¹ m
The minimum uncertainty in position is 9.17 x 10⁻¹¹ m. To express this in terms of the radius of a xenon atom (Ixc 108 pm = 1.08 x 10⁻¹⁰ m), divide by the radius:
Δx/rx >= 9.17 x 10⁻¹¹ m / 1.08 x 10⁻¹⁰ m = 0.85
Rounding to 2 significant figures, the smallest possible length of the box inside of which the atom could be located with certainty is 0.85 times the radius of a xenon atom, or 0.85ry.
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Which is an unavoidable error in this experiment?
Responses
A The tube in the machine is on it's seventh run and may contain the remains of old experiments.The tube in the machine is on it's seventh run and may contain the remains of old experiments.
B Injection of the sample into the machine requires a certain minimum time.Injection of the sample into the machine requires a certain minimum time.
C Darryl washed the sample with the wrong solvent.Darryl washed the sample with the wrong solvent.
D Darryl set the temperature on the machine to 350°C instead of 400°CDarryl set the temperature on the machine to 350°C instead of 400°C
A 12.76 g mixture of sugar ( C12H22O11 ) and table salt ( NaCl ) is dissolved in 237 g of water. The freezing point of the solution was measured as −2.37 ∘C . Calculate the mass percent of sugar in the mixture. A list of Kf values can be found in the colligative constants table.
The mass percentage of the sugar (C₁₂H₂₂O₁₁) in the mixture, given that the mixture has a mass of 12.76 g, is 85.42%
How do i determine the mass percentage of the sugar (C₁₂H₂₂O₁₁)?We'll begin by obtaining the molar mass of sugar (C₁₂H₂₂O₁₁) and NaCl. Details below:
For C₁₂H₂₂O₁₁
Molar mass of C = 12 g/molMolar mass of H = 1 g/molMolar mass of O = 16 g/molMolar mass of C₁₂H₂₂O₁₁ = ?Molar mass of C₁₂H₂₂O₁₁ = (12 × 12) + (1 × 22) + (16 × 11)
Molar mass of C₁₂H₂₂O₁₁ = 342 g/mol
For NaCl
Molar mass of Na = 23 g/molMolar mass of Cl = 35.5 g/molMolar mass of NaCl =?Molar mass of NaCl = 23 + 35.5
Molar mass of NaCl = 58.5 g/mol
Next, we shall obtain the mass of the sugar (C₁₂H₂₂O₁₁) in the mixture. Details below:
Molar mass of C₁₂H₂₂O₁₁ = 342 g/molMolar mass of NaCl = 58.5 g/molMass of mixture = 12.76 gMass of C₁₂H₂₂O₁₁ =?Mass of C₁₂H₂₂O₁₁ = [molar mass of C₁₂H₂₂O₁₁ / molar mass of (C₁₂H₂₂O₁₁ + NaCl)] × mass of mixture
Mass of C₁₂H₂₂O₁₁ = [342 / (342 + 58.5)] × 12.76
Mass of C₁₂H₂₂O₁₁ = 10.90 g
Finally, we shall determine the mass percentage of the sugar (C₁₂H₂₂O₁₁). This is illustrated as follow:
Mass of C₁₂H₂₂O₁₁ = 10.90 gMass of mixture = 12.76 gMass percentage of sugar (C₁₂H₂₂O₁₁) =?Mass percentage of sugar (C₁₂H₂₂O₁₁) = (mass of of KClO₃ / mass of mixture) × 100
Mass percentage of sugar (C₁₂H₂₂O₁₁) = (10.90 / 12.76) × 100
Mass percentage of sugar (C₁₂H₂₂O₁₁) = 85.42%
Thus, the mass percentage of the sugar (C₁₂H₂₂O₁₁) is 85.42%
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Given the equation, 2 C₂H6(s) + 702(g) → 6 H₂O(l) + 4 CO₂(g),
how many liters of carbon dioxide gas will be created with 4.6 L of
oxygen gas?
A. 128.8 L
B. 8.1 L
C. 2.6 L
D. 1.4 L
E. 6.2 L
2 L
The solution is D. 1.4 L The formula is 2 C2H6(s), 702(g), 6 H2O(l), and 4 CO2(g). According to this equation, four molecules of carbon dioxide and seven molecules of oxygen are created for every two molecules of C2H6.
We can thus determine how many litres of carbon dioxide gas will be produced if we have 4.6 litres of oxygen gas. By dividing 4.6 litres of oxygen gas by 7, we get 0.657 litres of oxygen gas per molecule, which we may use for this purpose.
This is 2.628 litres of carbon dioxide gas when multiplied by four molecules of carbon dioxide. Finally, we arrive at 1.4 litres of carbon dioxide gas after rounding this to the nearest litre. The solution is D as a result.
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71.587 grams of KCl are dissolved in 1.947 L of water. What is the molarity of this solution?
Answer:
To calculate the molarity of a solution, we need to use the formula
which is:
Molarity = moles of solute / liters of solution
First, we need to calculate the moles of KCl in the solution:
m = 71.587 g (mass of KCl)
M = 74.55 g/mol (molar mass of KCl)
moles of KCl = m / M = 71.587 g / 74.55 g/mol = 0.9607 mol
Next, we have to calculate the liters of solution:
V = 1.947 L
since we found solute and solution then we can put it into the formula
Molarity = moles of solute / liters of solution
Molarity = 0.9607 mol / 1.947 L = 0.4939 M
Therefore, the molarity of the KCl solution is 0.4939 M.
how many moles of SnF2 are produced from the reaction of 30g of HF
0.375 moles of SnF_2 are produced from the reaction of 30g of HF.
What are some instances of chemical reactions?When a substance undergoes a chemical transformation, its chemical identity changes. Rust is one illustration of this. An iron nail rusts, turning brown-red, when it comes into touch with water and is then exposed to air. The chemical makeup of the original material is altered throughout this process.
To determine the moles of SnF2:
[tex]SnO_2(s) + 4HF(aq) = > SnF_2(s) + 2H_2O(l)[/tex]
From the balanced equation,
Now, we have to calculate the number of moles of HF from the given mass of 30g:
30g HF x (1 mol HF/20.01 g HF) = 1.50 mol HF
So, we have 1.50 mol of HF.
Applying the stoichiometry from the balanced chemical equation,
1.50 mol HF x (1 mol SnF2/4 mol HF) = 0.375 mol SnF2
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Please help me I have to find the unknown by this given info
The condensed structural formula of the organic compound cannot be determined from the given information. However, the compound is basic and is a reducing agent.
What is a condensed structural formula?Condensed structural formulas are the formula of organic compounds that conserves space and are easier and faster to write out, displaying the atoms' positions similar to a structural formula but on a single line.
When demonstrating how a group of atoms in a molecule are linked to a single atom, condensed structural formulae are also helpful.
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I WILL GIVE 35 POINTS TO THOSE WHO ANSWER THIS QUESTION RIGHT NOOOO SCAMS PLEASE
The mass (in grams) of Cu(OH)₂ that can be made when you mix 374.48 mL of 1.451 M NaOH with excess CuCl₂ is 52.98 grams
How do i determine the mass of Cu(OH)₂ formed?First, we shall determine the mole present in 374.48 mL of 1.451 M NaOH Details below:
Volume = 374.48 mL = 374.48 / 1000 = 0.37448 LMolarity = 1.451 MMole of NaOH =?Molarity = Mole / Volume
Cross multiply
Mole of NaOH = molarity × volume
Mole of NaOH = 1.451 × 0.37448
Mole of NaOH = 0.543 mole
Next, we shall determine the mole of Cu(OH)₂ obtained from the reaction. Details below:
CuCl₂ + 2NaOH -> Cu(OH)₂ + 2NaCl
From the balanced equation above,
1 moles of NaOh reacted to produce 1 mole of Cu(OH)₂
Therefore,
0.543 mole of NaOH will also react to produce 0.543 mole of Cu(OH)₂
Finally, we shall determine the mass of Cu(OH)₂ obtained from the reaction. Details below:
Molar mass of Cu(OH)₂ = 97.56 g/mol
Mole of Cu(OH)₂ = 0.543
Mass of Cu(OH)₂ = ?
Mole = mass / molar mass
0.543 = Mass of Cu(OH)₂ / 142
Cross multiply
Mass of Cu(OH)₂ = 0.543 × 97.56
Mass of Cu(OH)₂ = 52.98 grams
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1 Given that the density of CO₂ at the temperatures we used is 1.25 g/L, calculate the theoretical
and actual yield (based on the amount of sodium acetate produced!) for CO2, in liters, for the
experiment.
нсо
2 How many grams of sodium hydrogen carbonate would be necessary to produce 425 mL of CO₂?.
Use the density of CO2 from
1.596 grams of sodium hydrogen carbonate would be necessary to produce 425 mL of [tex]CO_{2}[/tex] at STP.
To calculate the amount of sodium hydrogen carbonate needed to produce 425 mL of [tex]CO_{2}[/tex], you can use the following steps:
Convert the volume of [tex]CO_{2}[/tex] to moles using the molar volume at STP:
425 mL ÷ 1000 mL/L = 0.425 L [tex]CO_{2}[/tex]
0.425 L [tex]CO_{2}[/tex] ÷ 22.4 L/mol = 0.019 moles [tex]CO_{2}[/tex]
Use the balanced chemical equation to determine the stoichiometry between sodium acetate and carbon di oxide:
[tex]NaC_{2} H_{3} O_{2}[/tex] [tex]+ H_{2} O + CO_{2}[/tex] → [tex]Na HC_{3} O_{2}[/tex][tex]+ CH_{3} COOH[/tex]
For every 1 mole of sodium acetate, 1 mole of CO2 is produced. Therefore,
0.019 moles CO2 = 0.019 moles [tex]NaC_{2} H_{3} O_{2}[/tex]
Calculate the mass of sodium hydrogen carbonate needed using its molar mass:
0.019 moles [tex]NaC_{2} H_{3} O_{2}[/tex] × 84.01 g/mol = 1.596 g [tex]Na HC_{3} O_{2}[/tex]
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Submit your answers to the following questions:
What is the difference between a physical change and a chemical change?
What kind of change occurred in each test? Explain why in your own words.
its due April 30 so please answer this question before that time also giving ten points
Online Experiment: Chemical Change
You will see several procedures. Make observations and determine whether a chemical or physical change occurred with each procedure. [The experiment’s materials are displayed: small utility candle and holder, matches, digital metric balance, two small sheets of paper, watch glass or crucible, three test tubes, test tube holder, tray, one 100 mL beaker, water, table salt, baking soda, vinegar]
Here, measure the mass of a candle and its holder. [Electronic balance massing a candle in a candle holder.] Be sure to record this mass. [219 grams] Then, light the candle and allow it to burn for five minutes or so. [Burning candle] Make observations of the burning candle and record. [Five minutes later]
Blow out the candle and let the wax cool. [Candle is blown out] Once the wax is cool, measure the new mass of the candle and holder. [The mass of the candle and candle holder is taken with the electronic balance.] Be sure to record this mass. [218 grams]
Next we are going to work with the pieces of paper. Tear the first piece of paper into small pieces. [A piece of paper is ripped into small pieces.] Record your observations.
Then wet the second piece of paper and record your observations. [Water is poured on top of the second piece of paper.]
Finally, put a few of the small pieces of paper on the watch glass. [Some of the small pieces of paper are placed on a watch glass.] Carefully light them with a match. [The small pieces of paper are set on fire with a match.] Record your observations.
This time you will add salt to a test tube and then add water and shake until the salt is no longer visible. [Salt and water are added to a test tube and then shaken.] Record your observations. [The water in the test tube appears clear.]
Now you will dissolve some baking soda in water in a test tube. [Water and baking soda are dissolved in a test tube and shaken.] Add some vinegar to another test tube. [Vinegar is poured into a test tube.] Carefully pour the contents of both test tubes into the beaker. [Both test tubes are poured into a beaker and then there is vigorous bubbling.] Make observations and record.
Physical changes involve changes in the physical properties of a substance, while chemical changes involve changes in the chemical properties and identity of a substance.
A physical change is a change in the physical properties of a substance without changing its chemical identity. Physical changes can be observed without altering the substance’s composition or identity. For example, changes in state of matter, such as melting, freezing, and boiling. On the other hand, Chemical changes involve changes in chemical identity of substance, resulting in the formation of one or more new substances with different chemical properties. In chemical change, the original substance is transformed into a different substance with different chemical properties. Examples of chemical changes include combustion, oxidation, decomposition.
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--The complete Question is, What is the difference between a physical change and a chemical change?--
When some water condensed onto a glass, it released 9.15 Cal (kcal) of energy. How many joules of energy is this?
On converting Calories to joules, 9.15 Cal is 38.28 joules of energy.
We will see how to convert calories to joules of energy. We have obtained the following data from the given question. We are given that energy is released in calories which is 9.15 calories and we have to find energy in joules by converting the energy from calories to joules.
We have got a conversion scale to convert calories to joules. We know that
1 Calorie = 4.184 Joules
Using the above scale, we can convert 9.15 calories to joules as given below:
1 Calorie = 4.184 Joules
Therefore,
9.15 Calories = (9.15 Calories × 4.184 Joules) / 1 Calorie
9.15 Calories = 38.28 Joules
Therefore, we can conclude from the above calculation that the energy in joules is 38.28 Joules.
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Answer:
38,200J
Explanation:
9.15 x 4.18 x 1000= 38,247 → 38,200J
a student reacts 1.2 g of carbon with 16.2g of zinc oxide. the resulting products are 4.4g of carbon dioxide and 113g of zinc. Determine the balanced equation for this reaction? can i have some help with this
The balanced equation for the reaction is written as:
C + 2ZnO -> CO₂ + 2Zn
How do i write the balanced equation for the reaction?Chemical equation equation basically has two sides. These are the reactants and products
Reactants -> Products
The balancing of chemical equation is done by ensuring that the number of atoms of the reactants is equal to the number of atoms of the products.
Now, we shall write the balance the equation as follow:
Carbon => CZinc oxide => ZnOcarbon dioxide => CO₂Zinc => ZnC + ZnO -> CO₂ + Zn
There are 2 atoms of O on the right side and 1 atom on the left side. It can be balanced by writing 2 before ZnO as shown below:
C + 2ZnO -> CO₂ + Zn
There are 2 atoms of Zn on the left side and 1 atom on the right side. It can be balanced by writing 2 before Zn as shown below:
C + 2ZnO -> CO₂ + 2Zn
Thus, the equation is balanced!
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write the acidic equilibrium equation for CCl2HCOOH
The acidic equilibrium equation for CCl₂HCOOH, which is also known as dichloroacetic acid, can be written as; CCl₂HCOOH ⇌ CCl₂HCOO⁻ + H⁺
In this equation, CCl₂HCOOH represents dichloroacetic acid in its uncharged, acidic form. When dichloroacetic acid dissolves in water or an aqueous solution, it can dissociate into its corresponding ions, CCl₂HCOO⁻ (dichloroacetate ion) and H⁺ (hydrogen ion).
The arrow (⇌) indicates that the reaction can proceed in both directions, with dichloroacetic acid donating a hydrogen ion to form the dichloroacetate ion, and the dichloroacetate ion accepting a hydrogen ion to reform dichloroacetic acid. This is an example of a weak acid dissociating in water to form its conjugate base and hydrogen ions, establishing an acidic equilibrium.
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What is the mass of milk fat in 1.0 L of lowfat milk? Whole milk is 2.0% w/v milk fat.
The mass of milk fat in 1.0 L of low fat milk is 10 g.
What is Low fat milk?
Low-fat milk is a type of milk that has had most of its fat content removed. It typically contains 1% or 2% milkfat, which is significantly less than whole milk, which contains about 3.5% milkfat. Low-fat milk is often recommended as a healthier alternative to whole milk because it contains fewer calories and less saturated fat. However, it still contains important nutrients such as calcium, vitamin D, and protein, which are essential for maintaining good health. Low-fat milk can be used in cooking and baking, and is commonly consumed on its own or used in coffee and tea.
Low fat milk typically contains 1% milk fat, which is half the milk fat content of whole milk. Therefore, the mass of milk fat in 1.0 L of low fat milk can be calculated using the following steps:
Calculate the mass of milk fat in 1.0 L of whole milk:
Whole milk is 2.0% w/v milk fat, which means that there are 2.0 g of milk fat in 100 mL of whole milk.
Therefore, there are 20 g of milk fat in 1.0 L (1000 mL) of whole milk.
Calculate the mass of milk fat in 1.0 L of low fat milk:
Low fat milk contains half the milk fat of whole milk, so there are 10 g of milk fat in 1.0 L of low fat milk.
Therefore, the mass of milk fat in 1.0 L of low fat milk is 10 g.
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Which of the following best describes the third law of thermodynamics?
A) U(univ) = U(sys) + U(surr)
B) S* = 0 for perfect Li(s) at 0 K
C) S (univ) > 0 (spontaneous process)
D) SH(rev)/T at constant T
E) G=H-TS
A student adds 88.4 g of sucrose(molar mass=342.3 g/mol to 1.50 L of 20 degrees C water she stirs until all the crystals dissolve what is the solutions molarity
A calorimeter contains 145 g of water at 24.5 °C. A 23.2 g sample of MgBr₂ is added to the water in the calorimeter. After the solid has dissolved, the temperature of the water is 63.0 °C. Calculate the enthalpy of solution, in kJ/mol, for dissolving magnesium bromide in water. Assume that all heat is transferred to the water, and that the specific heat of the solution is the same as that of pure water.
First, we need to calculate the heat absorbed by the water:
q = m × c × ΔT
where q is the heat absorbed, m is the mass of water, c is the specific heat of water, and ΔT is the change in temperature.
q = 145 g × 4.184 J/g°C × (63.0°C - 24.5°C)
q = 16394.12 J
Next, we need to calculate the amount of substance of MgBr₂ that was added to the water:
n = m/MW
where n is the amount of substance, m is the mass of MgBr₂, and MW is the molecular weight of MgBr₂.
MW(MgBr₂) = 184.11 g/mol
n = 23.2 g ÷ 184.11 g/mol
n = 0.1259 mol
Finally, we can calculate the enthalpy of solution, ΔH, using the following formula:
ΔH = q ÷ n
where ΔH is the enthalpy of solution.
ΔH = 16394.12 J ÷ 0.1259 mol
ΔH = 130233.72 J/mol
Converting to kilojoules per mole (kJ/mol):
ΔH = 130.23 kJ/mol
Therefore, the enthalpy of solution for dissolving magnesium bromide in water is 130.23 kJ/mol.
The enthalpy of solution of magnesium bromide in water is calculated using the formula for heat transfer and taking into account the mass of the solvent, the specific heat of the solvent, and the change in temperature. The result is 186 kJ/mol.
Explanation:To calculate the enthalpy of solution of magnesium bromide (MgBr₂), we need to use the formula for heat transfer: Q = m * c * ΔT, where m is the mass of the solvent (water), c is the specific heat of the solvent, and ΔT is the change in temperature.
In our case, the mass of water is 145g, the specific heat of water (c) is 4.18 J/g°C, and the change in temperature (ΔT) is 63.0 °C - 24.5 °C = 38.5 °C.
Using the formula Q = m * c * ΔT, we can calculate the heat transferred to the water: Q = 145g * 4.18 J/g°C * 38.5 °C = 23432 J or 23.432 kJ. This is the heat absorbed by the water.
The enthalpy of the solution is defined as the amount of heat absorbed (or released) when one mole of a substance is dissolved in water. So, to find the enthalpy of solution, we first need to convert the grams of MgBr₂ to moles. The molar mass of MgBr₂ is 184.11 g/mol, so 23.2 g of MgBr₂ is 23.2 g / 184.11 g/mol = 0.126 mol.
Now we can calculate the enthalpy change by dividing the heat absorbed by the moles of the solute: ΔH = Q / n = 23.432 kJ / 0.126 mol = 186 kJ/mol. Therefore, the enthalpy of solution for magnesium bromide in water is 186 kJ/mol.
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I have 0.345 L of a 1.5 M NaCl solution. If i boil the water until the volume of the solution id 0.250 L, What will the molarity of the solution be?
A. 2.07 M
B. 0.21 M
C. 1.09 M
D. 0.11 M
At room temperature, Si is a solid, CCl4 is a liquid, and Ar is a gas. List these substances in order of increasing intermolecular energy of attraction
Answer:
Most energy Si> CCl4 > Ar least energy
Explanation:
The strength of a bond is proportional to its bond/attraction energy. This means the molecule with the strongest bonds will have the strongest energy.
We know that Si has the strongest bonds because each atom in the compound is bonded tightly enough that it is solid. Recall that a solid has molecules closer and and more tightly bonded than in a liquid or gas, when the molecules move freer.
With this in mind, we know that Ar has the weakest attraction strength, and thus weakest energy of attraction, because it is a gas and that atoms move freely and interact minimally. There is not enough attraction for the molecules to form bonds nor to effect one another beyond accidental collisions.
propose a scheme for the synthesis of 2-benzylbutanoic acid using acetoacetic ester
The final product, 2-benzylbutanoic acid, can be obtained after purification through techniques such as recrystallization or chromatography.
2-benzylbutanoic acid can be synthesized via the following scheme using acetoacetic ester:
Step 1: Condensation of acetoacetic ester with benzyl bromide in the presence of a base, such as potassium carbonate, to form 2-benzyl-3-ketobutyric ester.
Step 2: Hydrolysis of 2-benzyl-3-ketobutyric ester with aqueous acid, such as hydrochloric acid, to form 2-benzyl-3-ketobutyric acid.
Step 3: Reduction of 2-benzyl-3-ketobutyric acid with a reducing agent, such as sodium borohydride, to form 2-benzylbutanoic acid.
Overall Scheme:
Acetoacetic ester --(condensation with benzyl bromide, [tex]K2CO3)[/tex]--> 2-benzyl-3-ketobutyric ester --(hydrolysis with HCl)--> 2-benzyl-3-ketobutyric acid --(reduction with[tex]NaBH4)[/tex]--> 2-benzylbutanoic acid
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provide the mechanism of hydrolysis of 2-methylpropionic acid nitrile in acidic conditions
The hydrolysis of 2-methylpropionic acid nitrile in acidic conditions proceeds through an acid-catalyzed mechanism.
The mechanism can be described as follows:
Protonation of the nitrile group by the acid catalyst to form a protonated nitrile intermediate.Nucleophilic attack of water on the protonated nitrile intermediate to form a protonated amide intermediate.Deprotonation of the protonated amide intermediate by the acid catalyst to form the corresponding carboxylic acid.Protonation of the water molecule by the acid catalyst to generate a hydronium ion, which can then protonate another molecule of the nitrile substrate and continue the reaction.The hydrolysis of 2-methylpropionic acid nitrile in acidic conditions results in the conversion of the nitrile group to a carboxylic acid group through the addition of a water molecule and subsequent proton transfer steps. This reaction is commonly used in the synthesis of carboxylic acids from nitriles, and is an important process in organic chemistry.
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if the reaction used up 2.35 moles of H2 , how many moles of NH3 were produced? use this eqationN2 + 3 H2 → 2 NH3
Answer:
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Explanation:
According to the balanced chemical equation, for every 3 moles of H2 consumed, 2 moles of NH3 are produced.
Therefore, to find the number of moles of NH3 produced, we need to determine the ratio of H2 to NH3 based on the balanced equation:
3 moles H2 : 2 moles NH3
If 3 moles of H2 produces 2 moles of NH3, then 2.35 moles of H2 would produce:
(2 moles NH3 / 3 moles H2) x 2.35 moles H2 = 1.57 moles NH3
So, 1.57 moles of NH3 would be produced if 2.35 moles of H2 were consumed in this reaction.
What mass in grams of tin would be required to completely react with 1.45 L of 0.750 M HBr in the following chemical reaction?
Sn(s) + 4 HBr(aq) -› SnBr, (aq) + 2 H, (g)
