Question 1

For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

Accepted Answer

A) The rate will decrease by a factor of 1/9.00. 
B) The rate will decrease by a factor of 1/3.00. 
C) The rate will increase by a factor of 3.00. 
D) The rate will increase by a factor of 9.00. 
A) The rate will decrease by a factor of 1/9.00. 
B) The rate will decrease by a factor of 1/3.00. 
C) The rate will increase by a factor of 3.00. 
D) The rate will increase by a factor of 9.00. D

Question 2

A catalyst is needed in the hydrogenation of double bonds. In the first step, the reactants must come into contact with a metal surface. This step is known as

Accepted Answer

A) adsorption. 
B) diffusion. 
C) reaction. 
D) desorption. 
E) none of the above 
A) adsorption. 
B) diffusion. 
C) reaction. 
D) desorption. 
E) none of the above A

Question 3

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

Accepted Answer

A) zero order 
B) first order 
C) second order 
D) third order 
E) impossible to determine 
A) zero order 
B) first order 
C) second order 
D) third order 
E) impossible to determine B

Question 4

Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction)
Mechanism
A2 ⇌ 2A fast
A + B → AB slow

Accepted Answer

A) Rate = k[A][B] 
B) Rate = k[A2][B] 
C) Rate = k[A2][B]1/2 
D) Rate = k[A2] 
E) Rate = k[A2]1/2[B] 
A) Rate = k[A][B] 
B) Rate = k[A2][B] 
C) Rate = k[A2][B]1/2 
D) Rate = k[A2] 
E) Rate = k[A2]1/2[B]

Question 5

Given the following rate law, how does the rate of reaction change if the concentration of X is doubled? Rate = k [X]2[Y]3

Accepted Answer

A) The rate of reaction will increase by a factor of 9. 
B) The rate of reaction will increase by a factor of 2. 
C) The rate of reaction will increase by a factor of 8. 
D) The rate of reaction will increase by a factor of 4. 
E) The rate of reaction will remain unchanged. 
A) The rate of reaction will increase by a factor of 9. 
B) The rate of reaction will increase by a factor of 2. 
C) The rate of reaction will increase by a factor of 8. 
D) The rate of reaction will increase by a factor of 4. 
E) The rate of reaction will remain unchanged.

Question 6

Match the following.

-Ea

Accepted Answer

A) activation energy 
B) half-life 
C) reaction order 
D) rate constant 
E) frequency factor 
A) activation energy 
B) half-life 
C) reaction order 
D) rate constant 
E) frequency factor

Question 7

Calculate the temperature if a reaction has a rate constant, k, of 1234 s-1, a frequency factor, A, of 1.34 × 1014 s-1, and an activation energy, Ea, of 79.6 kJ mol-1.

Accepted Answer

A) 298 K 
B) 341 K 
C) 377 K 
D) 418 K 
E) 447 K 
A) 298 K 
B) 341 K 
C) 377 K 
D) 418 K 
E) 447 K

Question 8

Match the following.

-k

Accepted Answer

A) activation energy 
B) half-life 
C) reaction order 
D) rate constant 
E) frequency factor 
A) activation energy 
B) half-life 
C) reaction order 
D) rate constant 
E) frequency factor

Question 9

Determine the rate law and the value of k for the following reaction using the data provided: S2O82⁻(aq)+ 3 I⁻(aq)→ 2 SO42⁻(g)+ I3⁻(aq)[S2O82⁻]i (M)[I⁻]i (M)Initial Rate (M-1 s-1)
0.30 0.42 4.54
0.44 0.42 6.65
0.44 0.21 3.33

Accepted Answer

A) Rate = 120 M-2 s-1 [S2O82⁻]2[I⁻] 
B) Rate = 36 M-1 s-1 [S2O82⁻][I⁻] 
C) Rate = 86 M-2 s-1 [S2O82⁻][I⁻]2 
D) Rate = 195 M-3 s-1 [S2O82⁻]2[I⁻]2 
E) Rate = 23 M-1/2 s-1 [S2O82⁻][I⁻]1/2 
A) Rate = 120 M-2 s-1 [S2O82⁻]2[I⁻] 
B) Rate = 36 M-1 s-1 [S2O82⁻][I⁻] 
C) Rate = 86 M-2 s-1 [S2O82⁻][I⁻]2 
D) Rate = 195 M-3 s-1 [S2O82⁻]2[I⁻]2 
E) Rate = 23 M-1/2 s-1 [S2O82⁻][I⁻]1/2

Question 10

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.

Accepted Answer

A) 160. kJ mol-1 
B) 240. kJ mol-1 
C) 417 kJ mol-1 
D) 127 kJ mol-1 
E) 338 kJ mol-1 
A) 160. kJ mol-1 
B) 240. kJ mol-1 
C) 417 kJ mol-1 
D) 127 kJ mol-1 
E) 338 kJ mol-1

Question 11

Identify a homogeneous catalyst.

Accepted Answer

A) SO2 over vanadium (V)oxide 
B) Pd in H2 gas 
C) Pt with methane 
D) H2SO4 with concentrated HCl 
E) N2 and H2 catalyzed by Fe 
A) SO2 over vanadium (V)oxide 
B) Pd in H2 gas 
C) Pt with methane 
D) H2SO4 with concentrated HCl 
E) N2 and H2 catalyzed by Fe

Question 12

The rate of disappearance of HBr in the gas phase reaction 2HBr(g)→ H2(g)+ Br2(g)
Is 0.301 mol L-1 s-1 at 150 °C. The rate of appearance of Br2 is ________ mol L-1 s-1.

Accepted Answer

A) 1.66 
B) 0.151 
C) 0.0906 
D) 0.602 
E) 0.549 
A) 1.66 
B) 0.151 
C) 0.0906 
D) 0.602 
E) 0.549

Question 13

What is the overall order of the following reaction, given the rate law? 2NO(g)+ H2(g)→ N2(g)+ 2H2O(g)Rate = k[NO]2[H2]

Accepted Answer

A) 1st order 
B) 2nd order 
C) 3rd order 
D) 4th order 
E) 0th order 
A) 1st order 
B) 2nd order 
C) 3rd order 
D) 4th order 
E) 0th order

Question 14

If the concentration of a reactant is 6.25%, how many half-lives has it gone through?

Accepted Answer

A) 7 
B) 6 
C) 3 
D) 4 
E) 5 
A) 7 
B) 6 
C) 3 
D) 4 
E) 5

Question 15

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]

Accepted Answer

A) The rate of reaction will increase by a factor of 2. 
B) The rate of reaction will increase by a factor of 4. 
C) The rate of reaction will increase by a factor of 5. 
D) The rate of reaction will decrease by a factor of 2. 
E) The rate of reaction will remain unchanged. 
A) The rate of reaction will increase by a factor of 2. 
B) The rate of reaction will increase by a factor of 4. 
C) The rate of reaction will increase by a factor of 5. 
D) The rate of reaction will decrease by a factor of 2. 
E) The rate of reaction will remain unchanged.

Question 16

The reaction that occurs in a Breathalyzer, a device used to determine the alcohol level in a person's bloodstream, is given below. If the rate of appearance of Cr2(SO4)3 is 1.64 mol min-1 at a particular moment, what is the rate of disappearance of C2H6O at that moment? 2K2Cr2O7 + 8H2SO4 + 3C2H6O → 2Cr2(SO4)3 + 2K2SO4 + 11H2O

Accepted Answer

A) 0.547 mol min-1 
B) 1.09 mol min-1 
C) 2.46 mol min-1 
D) 4.92 mol min-1 
A) 0.547 mol min-1 
B) 1.09 mol min-1 
C) 2.46 mol min-1 
D) 4.92 mol min-1

Question 17

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 8.14 L mol-1 s-1 at 350 K. At what temperature will the rate constant be one-half?

Accepted Answer

A) 175 K 
B) 340 K 
C) 385 K 
D) 331 K 
E) 279 K 
A) 175 K 
B) 340 K 
C) 385 K 
D) 331 K 
E) 279 K

Question 18

Determine the missing initial rate for the following   order reaction given the following information:

Accepted Answer

A) 0.48 mol L-1 s-1 
B) 0.38 mol L-1 s-1 
C) 0.91 mol L-1 s-1 
D) 1.3 mol L-1 s-1 
E) 0.84 mol L-1 s-1 
A) 0.48 mol L-1 s-1 
B) 0.38 mol L-1 s-1 
C) 0.91 mol L-1 s-1 
D) 1.3 mol L-1 s-1 
E) 0.84 mol L-1 s-1

Question 19

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

Accepted Answer

A) 4.21 g 
B) 183 g 
C) 54.8 g 
D) 76.3 g 
E) 67.5 g 
A) 4.21 g 
B) 183 g 
C) 54.8 g 
D) 76.3 g 
E) 67.5 g

Question 20

Which of the following is the characteristic of a second-order reaction having only one reactant.

Accepted Answer

A) The rate of the reaction is not proportional to the concentration of the reactant. 
B) The rate of the reaction is proportional to the square of the concentration of the reactant. 
C) The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E) The rate of the reaction is directly proportional to the concentration of the reactant. 
A) The rate of the reaction is not proportional to the concentration of the reactant. 
B) The rate of the reaction is proportional to the square of the concentration of the reactant. 
C) The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E) The rate of the reaction is directly proportional to the concentration of the reactant.

Exam 13: Chemical Kinetics

For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

A catalyst is needed in the hydrogenation of double bonds. In the first step, the reactants must come into contact with a metal surface. This step is known as

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction) Mechanism A2 ⇌ 2A fast A + B → AB slow

Given the following rate law, how does the rate of reaction change if the concentration of X is doubled? Rate = k [X]2[Y]3

Match the following. -Ea

Calculate the temperature if a reaction has a rate constant, k, of 1234 s-1, a frequency factor, A, of 1.34 × 1014 s-1, and an activation energy, Ea, of 79.6 kJ mol-1.

Match the following. -k

Determine the rate law and the value of k for the following reaction using the data provided: S2O82⁻(aq)+ 3 I⁻(aq)→ 2 SO42⁻(g)+ I3⁻(aq)[S2O82⁻]i (M)[I⁻]i (M)Initial Rate (M-1 s-1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.

Identify a homogeneous catalyst.

The rate of disappearance of HBr in the gas phase reaction 2HBr(g)→ H2(g)+ Br2(g) Is 0.301 mol L-1 s-1 at 150 °C. The rate of appearance of Br2 is ________ mol L-1 s-1.

What is the overall order of the following reaction, given the rate law? 2NO(g)+ H2(g)→ N2(g)+ 2H2O(g)Rate = k[NO]2[H2]

If the concentration of a reactant is 6.25%, how many half-lives has it gone through?

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 8.14 L mol-1 s-1 at 350 K. At what temperature will the rate constant be one-half?

Determine the missing initial rate for the following order reaction given the following information:

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

Which of the following is the characteristic of a second-order reaction having only one reactant.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

For a reaction that follows the general rate law, Rate = k[A][B]², what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

Given the following proposed mechanism, predict the rate law for the overall reaction. A₂ + 2B → 2AB (overall reaction) Mechanism A₂ ⇌ 2A fast A + B → AB slow

Given the following rate law, how does the rate of reaction change if the concentration of X is doubled? Rate = k [X]²[Y]³

Match the following. -E_a

Calculate the temperature if a reaction has a rate constant, k, of 1234 s^-1, a frequency factor, A, of 1.34 × 10¹⁴ s^-1, and an activation energy, E_a, of 79.6 kJ mol^-1.

Determine the rate law and the value of k for the following reaction using the data provided: S₂O₈²⁻(aq)+ 3 I⁻(aq)→ 2 SO₄²⁻(g)+ I₃⁻(aq)[S₂O₈²⁻]_i(M)[I⁻]_i (M)Initial Rate (M^-1s^-1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33

The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15 s^-1 at 298 K and a rate constant of 8.66 × 10^-7 s^-1 at 425 K. Determine the activation energy for this reaction.

The rate of disappearance of HBr in the gas phase reaction 2HBr(g)→ H₂(g)+ Br₂(g) Is 0.301 mol L^-1 s^-1 at 150 °C. The rate of appearance of Br₂ is ________ mol L^-1 s^-1.

What is the overall order of the following reaction, given the rate law? 2NO(g)+ H₂(g)→ N₂(g)+ 2H₂O(g)Rate = k[NO]²[H₂]

A reaction with an activation energy of 71.6 kJ mol^-1 has a rate constant of 8.14 L mol^-1 s^-1 at 350 K. At what temperature will the rate constant be one-half?