Answer:
2.The reaction is third order overall
Explanation:
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Gaseous methane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 9.6 g of methane is mixed with 64.9 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to significant digits.
Answer:
21.6 g
Explanation:
The reaction that takes place is:
CH₄ + 2O₂ → CO₂ + 2H₂OFirst we convert the given masses of both reactants into moles, using their respective molar masses:
9.6 g CH₄ ÷ 16 g/mol = 0.6 mol CH₄64.9 g O₂ ÷ 32 g/mol = 2.03 mol O₂0.6 moles of CH₄ would react completely with (2 * 0.6) 1.2 moles of O₂. As there are more O₂ moles than required, O₂ is the reactant in excess and CH₄ is the limiting reactant.
Now we calculate how many moles of water are produced, using the number of moles of the limiting reactant:
0.6 mol CH₄ * [tex]\frac{2molH_2O}{1molCH_4}[/tex] = 1.2 mol H₂OFinally we convert 1.2 moles of water into grams, using its molar mass:
1.2 mol * 18 g/mol = 21.6 gAcetic acid and water react to from hydronium cation and acetate anion, like this: HCH3CO2 (aq) + H2O (I) → H3O+(aq) + Ch3CO2-(aq)Imagine 226. mmol of CH3CO2- are added to a flask containing a mixture of HCH3CO2, H2O, H3O + and CH3CO2- at equilibrium, and then answer the following questions. 1. What is the rate of the forward reaction before any HCH3CO2 has been removed from the flask? a. Zero.b. Greater than zero, but less than the rate of the reverse reaction. c. Greater than zero, and equal to the rate of the reverse reaction. d. Greater than zero, and greater than the rate of the reverse reaction. 2. What is the rate of the forward reaction just after the HCH3CO2 has been removed from the flask?a. Zero.b. Greater than zero, but less than the rate of the reverse reaction. c. Greater than zero, and equal to the rate of the reverse reaction. d. Greater than zero, and greater than the rate of the reverse reaction.3. What is the rate of the forward reaction when the system has again reached equilibrium?a. Zero.b. Greater than zero, but less than the rate of the reverse reaction. c. Greater than zero, and equal to the rate of the reverse reaction. d. Greater than zero, and greater than the rate of the reverse reaction.
Answer:
1) Greater than zero, and equal to the rate of the reverse reaction
2) Greater than zero, but less than the rate of the reverse reaction
3) Greater than zero, and equal to the rate of the reverse reaction
Explanation:
A reaction system is said to be in equilibrium when the rate of forward reaction is equal to the rate of reverse reaction.
Before we remove HCH3CO2 from the system, the system was in equilibrium. Recall that when a system is in equilibrium, the rate of forward reaction is equal to the rate of reverse reaction. The rate of reaction is greater than zero because products are being formed as the reactants interact with each other.
When HCH3CO2 is removed from the system, the equilibrium position shifts towards the left hand side hence the rate of reverse reaction is greater than the rate of forward reaction.
When the system attains equilibrium again, the rates of forward and reverse reaction become equal.
A Bronsted-Lowry acid is defined as a substance that ________. A Bronsted-Lowry acid is defined as a substance that ________. increases Ka when placed in H2O increases [OH-] when placed in H2O acts as a proton donor acts as a proton acceptor decreases [H ] when placed in H2O
Answer: A Bronsted-Lowry acid is defined as a substance that acts as a proton donor.
Explanation:
A substance that is able to donate a proton or hydrogen ion to another substance is a Bronsted-Lowry acid.
For example, HCl is a Bronsted-Lowry acid as it dissociates to give a hydrogen ion.
[tex]HCl \rightleftharpoons H^{+} + Cl^{-}[/tex]
Thus, we can conclude that a Bronsted-Lowry acid is defined as a substance that acts as a proton donor.
give one important characteristic of the particles of matter very sort answer give
Answer:
The important characteristics of the particles of matter are – They are very, very small. They have spaces between them. They are constantly moving.
Answer:
They are very very small
In the titration of NaOH with vinegar, a student overshot the endpoint (i.e. added too much NaOH solution). How will this affect the calculate percent acetic acid in the vinegar
Answer:
Overshooting the endpoint leads to a percent acetic acid in vinegar higher than the correct value.
Explanation:
When too much NaOH solution is added, the resulting number of equivalent hydronium (OH⁻) will be higher than what it is in reality. This would directly lead to the number of acetic acid moles in the vinegar being found higher than normal.
In other words, overshooting the endpoint leads to a percent acetic acid in vinegar higher than the correct value.What is the law of multiple proportions?
A. The proportion of elements to compounds is constant.
B. All elements are found in equal proportions in nature.
C. Different compounds may contain the same elements but may have different ratios of those elements.
D. All compounds contain the same elements in the same proportions.
Answer:
I think
(d) All compounds contain the same elements in the same properties
determine the number of moles of Cl in 1.9 mol of CaCl2
Explanation:
In the formula of [tex]CaCl_2[/tex] we can see that there are 2mol Cl in 1 molecule of CaCl2. So, now we can do some math to find out how many mol of Cl there are in 1.9mol CaCl2!
[tex]1.9molCaCl_2*\frac{2molCl}{1molCaCl_2}[/tex]
So, there are 3.8mol Cl
Which procedure could a student use to examine an intensive property of a rectangular block of wood
Find the mass.
Record the length. Measure the volume. Determine the density.
Answer:
density
Explanation:
The procedure that the student could use to examine an intensive property of a rectangular block of wood is to determine its density. Density is intensive because it is the ration between the mass and the volume.
Answer: find the mass option A
Explanation:
To identify a halide, you can react a solution with chlorine water in the presence of mineral oil.
If the unknown halide is a
Choose...weaker/stronger
reducing agent than chlorine, the halide will be oxidized to
Choose...its elemental form/ its ionic form/ a solid
which would change the color of the
Choose...mineral oil/ aqueous
layer.
Answer:
- Stronger reducing agent than Chlorine
- Oxidized to it's elemental form
- Change the colour of the aqueous layer.
Explanation:
Halides are electronegative elements in group seven of the Periodic table which have gained electrons to complete their electronic configuration.
They include F-, CL-, Br- and I-.
As you descend the group electro negativity decreases as the number of outermost shells increases. Hence F- is the most electronegative while I- is the least electronegative.
In terms of oxidising and reducing abilities amongst the halogens, since an oxidizing agent readily accepts electrons and is thereby reduced, oxidizing power decreases down the group.
For example, Fluorine being the strongest oxidising agent in the group readily accepts electrons from other members of the group and is reduced to the fluoride ion
F + e = F -
Therefore in terms of oxidizing abilities,
F > Cl > Br > I
Conversely, , as the oxidising power decreases down the group, the reducing powers increases
Therefore, in terms of reducing powers,
I > Br > Cl > F
In the test for halide ions using aqueous chlorine, since chlorine is a stronger oxidizing agent/weaker reducing agent than Bromine or iodine, it readily accepts their electrons forming the chloride ion.
Cl2 + 2 Br- = 2 Cl- + Br2
The bromide ion (assuming the unknown halide is bromide) being a stronger reducing agent/weaker oxidizing agent than Chlorine would readily lose it's electrons and get oxidized to it's elemental form changing the colour of the aqueous layer to brown.
That is : Br2- = Br2 + 2e
The fill in the blanks could be filled with stronger, elemental form and mineral oil.
Identification of a halide:In the case when the halide is not known so it should be stronger. The halide should be oxidized with respect to the elemental form and it should change the color of mineral oil. Due to this, halide should be oxidized for elemental halogen i.e. more soluble for mineral oil.
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Calculate the mass percent of carbon in the following molecule: Mn3[Mn(CO)4]3
Answer:
21.63 %
Explanation:
The molar mass of Mn₃[Mn(CO)₄]₃ is 665.64 g/mol.
Let's assume we have 1 mol of Mn₃[Mn(CO)₄]₃, if that were the case then we would have 665.64 grams.
There are 12 C moles per Mn₃[Mn(CO)₄]₃, with that in mind we calculate the weight of 12 C moles:
12 mol C * 12 g/mol = 144 gFinally we calculate the mass percent of carbon:
144 g / 665.64 g * 100% = 21.63 %What is the best tool for making a decorative zucchini or celery twist
Answer:
don't knoe sorry
Explanation:
A student measured the gram weight of a metal object to be 5.88g. According to the supplier the object weighs 5.97g. What is the error in the student's measurement?
A. -0.09
B. +0.09
Answer:
–0.09
Explanation:
From the question given above, the following data were obtained:
Measured value = 5.88 g
Actual value = 5.97 g
Error =?
The error in the student's measurement can be obtained as follow:
Error = Measured value – Actual value
Error = 5.88 – 5.97
Error = –0.09
Therefore, the error in the student's measurement is –0.09
Which of the following two periods contain the same number of element?
A. 2 & 3
B.3 & 4
c. 4 & 6
D. 2 & 4
Answer:
4 and 6
Explanation:
Period 4 has 18 elements and so does period 6.
g in the following three compounds(1,2,3) arrange their relative reactivity towards the reagent CH3Cl / AlCl3. Justify your order
Answer:
3 > 2> 1
Explanation:
Aromatic compounds undergo electrophilic substitution reaction with several electrophiles.
Some substituted benzenes are more reactive towards electrophilic aromatic substitution than unsubstituted benzene.
Certain groups of substituents increase the ease with which an aromatic compound undergoes aromatic substitution.
If we look at the compounds closely, we will notice that only toluene leads to easy reaction with CH3Cl / AlCl3. Thus is due to the +I inductive effect of -CH3 which stabilizes the negatively charged intermediate produced in the reaction.
Suppose a 48. L reaction vessel is filled with 1.6 mol of Br2 and 1.6 mol of OCl2. What can you say about the composition of the mixture in the vessel at equilibrium
Answer:
There will be very little of BrOCl BrCl
Explanation:
Based on the equilibrium:
Br2(g) + OCl2(g) ⇄ BrOCl(g) + BrCl(g)
The equilibrium constant, Kc, is:
Kc = 1.58x10⁻⁵ = [BrOCl] [BrCl] / [Br2] [OCl2]
As Kc is <<< 1, in equilibrium, the concentration of products will remain lower regard to the concentration of the reactants. That means, right answer is;
There will be very little of BrOCl BrClIn lipid bilayers, there is an order-to-disorder transition similar to the melting of a crystal. Comparing a lipid bilayer that is made up mostly of palmitoleic acid to one made up mostly of palmitic acid, which would have a higher melting transition temperature
Answer:
The lipid bilayer made up of Palmitic acid will have a higher melting transition temperature
Explanation:
The one with a higher melting transition temperature is the lipid layer with a higher melting temperature
Melting temperature of palmitoleic acid = -0.5°C
Melting temperature of palmitic acid = 62.9°C
Hence the lipid bilayer made up of Palmitic acid will have a higher melting transition temperature
Which statement BEST describes the strength of ionic and covalent bonds
Ionic bonds are the strongest type of chemical bond and, therefore, most compounds remain solid with very high melting points
The statement best describes the strength of ionic and covalent bonds is that ionic bond is the strongest bond and has very high melting point.
What are different types of bonding in chemistry?A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures. The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds, or through the sharing of electrons as in covalent bonds.
Types of Chemical Bonds includes-
Ionic Bonds.
Covalent Bonds.
Hydrogen Bonds.
Polar Bonds.
Generally, ionic bonds are much stronger than covalent bonds. In ionic bonds, there is complete transfer of electrons between elements to form a stable compound. While in covalent bond, there is only sharing of electrons between two elements to form a stable compound.
Therefore, The statement best describes the strength of ionic and covalent bonds is that ionic bond is the strongest bond and has very high melting point.
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Calculate the mass of Na2S needed if a solution containing 2g of Hg(NO3)2 was added to Na2S solution.
( Hg= 200.59, N= 14, O= 16, Na= 23, S=32)
Answer:
1.433g of HgS are produced
Explanation:
A Solution Containing 2.0 Grams Of Hg(NO3)2 Was Added To A Solution Containing 2.0 Grams Of Na2S. Calculate the mass of the HgS that was formed (it is a precipitate) according to this reaction:
Based on the reaction:
Na2S + Hg(NO3)2 → HgS + 2NaNO3
To solve this question we need to find the moles of each reactant in order to find the limiting reactant. The moles of limiting reactant = moles of HgS:
Moles Na2S -Molar mass: 78.0452 g/mol-
2.0g * (1mol / 78.0452g) = 0.0256 moles Na2S
Moles Hg(NO3)2 -324.7g/mol-
2.0g * (1mol / 324.7g) = 0.006159 moles Hg(NO3)2
As the reaction is 1:1, and moles of Hg(NO3)2 < moles Na2S
The moles of Hg(NO3)2 = Moles HgS = 0.006159 moles
The mass is:
Mass HgS -Molar mass: 232.66g/mol-:
0.006159 moles * (232.66g/mol) =
1.433g of HgS are produced
What is the cell potential of an electrochemical cell that has the half-reactions shown below?
Ag⁺ + e⁻ → Ag
Fe → Fe³⁺ + 3e⁻
Answer:
E°(Ag⁺/Fe°) = 0.836 volt
Explanation:
3Ag⁺ + 3e⁻ => Ag°; E° = +0.800 volt
Fe° => Fe⁺³ + 3e⁻ ; E° = -0.036 volt
_________________________________
Fe°(s) + 3Ag⁺(aq) => Fe⁺³(aq) + 3Ag°(s) ...
E°(Ag⁺/Fe°) = E°(Ag⁺) - E°(Fe°) = 0.800v - ( -0.036v) = 0.836 volt
Which one of the following is an example of a balanced chemical reaction?
a. 8HCl + 2KMnO4 → 3Cl2 + 2MnO2 + 4H2O + 2KCl.
b. 6HCl + 2KMnO4 → 2Cl2 + 2MnO2 + 4H2O + 2KCl.
c. 2HCl + 2KMnO4 → Cl2 + MnO2 + 2H2O + 2KCl.
d. HCl + KMnO4 → Cl2 + MnO2 + H2O + KCl.
e. HCl + KMnO4 → Cl2 + MnO2 + 2H2O + KCl.
Answer:
Option a.
Explanation:
To determine which is a balanced chemical reaction, see the stoichiometry.
Stoichiometry coefficients are the numbers that appear before the compounds. These numbers indicate moles of substance.
Notice that the number of elements must be the same in both sides of the equation.
In this case, option a is the balanced chemical reaction.
8HCl + 2KMnO₄ → 3Cl₂ + 2MnO₂ + 4H₂O + 2KCl
8 moles of HCl react to 2 moles of potassium permanganate in order to produce 2 moles of magnessium dioxide, 3 moles of chlorine, 2 moles of potassium chloride and 4 moles of water.
8 H, 8 Cl, 2 K, 2 Mn and 8 O
Suppose you perform a titration of an unknown weak acid solution. You start with 4.00 mL of the weak acid and find that it takes 14.2 mL of 0.0500 M NaOH to reach the equivalence point. What is the concentration of the unknown weak acid solution
Answer:
0.1775 M
Explanation:
The reaction that takes place is:
HA + NaOH → NaA + H₂OWhere HA is the unknown weak acid.
At the equivalence point all HA moles are converted by NaOH. First we calculate how many NaOH moles reacted, using the given concentration and volume:
0.0500 M NaOH * 14.2 mL = 0.71 mmol NaOHThat means that in 4.00 mL of the weak acid solution, there were 0.71 weak acid mmoles. With that in mind we can now calculate the concentration:
0.71 mmol HA / 4.00 mL = 0.1775 MAccording to the kinetic-molecular theory, gas molecules have
ANSWER:
Part
A. Less energy than molecules of a solid.
B. strong interactions between molecules.
C. little distance between molecule
D. weak interactions between molecules.
Answer:
The choose ( D )
weak interactions between molecules.
Answer:
Explanation:
el a
Which equation expresses the solubility product of Zn3(PO4)2?
a. Ksp = [Zn2+][PO43]
b. Ksp = [Zn2+]3 [PO43]2
c. Ksp = 6[Zn2+][PO43]2
d. Ksp = 108[Zn2+][PO43]2
⇒b. Ksp = [Zn2+]3 [PO43]2
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Diethyl ether (C2H5 )2O vaporizes at room temperature. If the vapor exerts a pressure of 233 mm Hg in a flask at 25 °C, what is the density of the vapor?
Answer: The density of the given vapor is 0.939 g/L.
Explanation:
Given: Pressure = 233 mm Hg (1 mm Hg = 0.00131579 atm) = 0.31 atm
Temperature = [tex]25^{o}C[/tex] = (25 + 273) K = 298 K
According to the ideal gas equation,
[tex]PV = \frac{m}{M}RT[/tex]
where,
P = pressure
V = volume
m = mass
M = molar mass
R = gas constant = 0.0821 L atm/mol K
T = temperature
This formula can be re-written as follows.
[tex]PM = \frac{m}{V}RT[/tex] (where, [tex]Density = \frac{mass (m)}{Volume (V)}[/tex] )
Hence, formula used to calculate density of diethy ether (molar mass = 74.12 g/mol) vapor is as follows.
[tex]d = \frac{PM}{RT}[/tex]
Substitute values into the above formula as follows.
[tex]d = \frac{PM}{RT}\\= \frac{0.31 atm \times 74.12 g/mol}{0.0821 L atm/mol K \times 298 K}\\= \frac{22.9772}{24.4658}\\= 0.939 g/L[/tex]
Thus, we can conclude that the density of the given vapor is 0.939 g/L.
What should be done if a spectrophotometer reports an absorbance that is too high? Select one: Reposition the cuvette in the spectrophotometer. Pour out half the volume of the sample. Restart the spectrophotometer and try again. Dilute the sample. g
Answer:
The sample should be diluted
Explanation:
According to Beer Lambert's law, the absorbance of a sample depends on the concentration of the sample.
Hence, if the concentration of the sample is very high, the spectrophotometer will also report a very high value of absorbance.
When this is the case, the sample should simply be diluted and the readings are taken again using the spectrophotometer.
A sample of calcium fluoride was decomposed into the constituent elements. Write a balanced chemical equation for the decomposition reaction. If the sample produced 294 mg of calcium, how many g of fluorine were formed
Answer:
A sample of calcium fluoride was decomposed into the constituent elements. Write a balanced chemical equation for the decomposition reaction. If the sample produced 294 mg of calcium, how many g of fluorine was formed
Explanation:
The balanced chemical equation for the decomposition of calcium fluoride is shown below:
[tex]CaF_2(s)->Ca(s)+F_2(g)[/tex]
The sample produced 294 g of calcium then, how many grams of fluorine is formed?
From the balanced chemical equation,
1 mol of CaF2 forms 1mol of calcium and 1 mol of fluorine.
That is:
40g of calcium and 38.0 g of fluorine are formed.
then,
If 294 g of calcium is formed then how many grams of fluorine is formed?
[tex]294g Ca * 38g F2 / 40g Ca\\=279.3 g F_2[/tex]
Hence, 279.3 g of fluorine will be formed.
a laser emits light with a frequency of 4.69 x 10 to the 14th power s - 1 calculate the wavelength of this light.
Answer:
6.40x10^-7
Explanation:
answer with work is attached.
Enough of a monoprotic acid is dissolved in water to produce a 1.211.21 M solution. The pH of the resulting solution is 2.882.88 . Calculate the Ka for the acid.
Answer:
1.44 × 10⁻⁶
Explanation:
Step 1: Given data
Concentration of the acid (Ca): 1.21 MpH of the solution: 2.88Step 2: Calculate the concentration of H⁺ ions
We will use the definition of pH.
pH = -log [H⁺]
[H⁺] = antilog -pH = antilog -2.88 = 1.32 × 10⁻³ M
Step 3: Calculate the acid dissociation constant of the acid (Ka)
For a weak monoprotic acid, we will use the following expression.
Ka = [H⁺]²/Ca
Ka = (1.32 × 10⁻³)²/1.21 = 1.44 × 10⁻⁶
Ammonium phosphate is an important ingredient in many solid fertilizers. It can be made by reacting aqueous phosphoric acid with liquid ammonia. Calculate the moles of phosphoric acid needed to produce 1.80 mol of ammonium phosphate. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Answer:
Explanation:
The reaction is
H3Po4+3NH3\to→ (NH4)3PO4
Given,7.10g NH3=7.10g/molar mass of NH3
=7.10g/(17.031g/mol)
=0.416mol
From the reaction
3 mol ammonia reacted and produced 1 mole of ammoniam phosphate
So,One mole ammonia reacted and produced 1/ 3 mole ammonium phosphate.
And Also,0.416 mole ammonium reacted and produced (1/3)0.416=0.138 mole ammonium phosphate.
Hence 0.138mole=0.138mole*149.08 g/mole
=20.573gm ammonium phosphate produced.
Hence 20.573g of ammonium phosphate is produced by the reaction of 7.10 g of ammonia.
A buffer is prepared containing 0.75 M NH3 and 0.20 M NH4 . Calculate the pH of the buffer using the Kb for NH3. g
Answer:
pH=8.676
Explanation:
Given:
0.75 M [tex]NH_{3}[/tex]
0.20 M [tex]NH_{4}[/tex]
The objective is to calculate the pH of the buffer using the kb for [tex]NH_3[/tex]
Formula used:
[tex]pOH=pka+log\frac{[salt]}{[base]}\\[/tex]
pH=14-pOH
Solution:
On substituting salt=0.75 and base=0.20 in the formula
[tex]pOH=-log(1.77*10^{-5})+log\frac{0.75}{0.20}\\ =4.75+0.5740\\ =5.324[/tex]
pH=14-pOH
On substituting the pOH value in the above expression,
pH=14-5.324
Therefore,
pH=8.676
