Deck 13: Chemical Kinetics

Question 1

Given the following balanced equation,determine the rate of reaction with respect to [O₂].
2SO₂(g)+ O₂(g)? 2SO₃(g)

A)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$
B)Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$
C)Rate = - $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$
D)Rate = + $\frac { 2 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Answer 1

Rate = - $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$

Question 2

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl₂ loss is 4.84 × 10^-2 mol L^-1 s^-1,what is the rate of formation of NOCl? 2NO(g)+ Cl₂(g)→ 2NOCl(g)

A)4.84 × 10^-2 mol L^-1 s^-1
B)2.42 × 10^-2 mol L^-1 s^-1
C)1.45 × 10^-1 mol L^-1 s^-1
D)9.68 × 10^-2 mol L^-1 s^-1
E)1.61 × 10^-2 mol L^-1 s^-1

Answer 2

9.68 × 10^-2 mol L^-1 s^-1

Question 3

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \\\hline 0.10 & 0.020 \\0.20 & 0.080 \\0.30 & 0.180\end{array}$$

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

Answer 3

second order

Question 4

Given the following balanced equation,determine the rate of reaction with respect to [O₂].If the rate of formation of O₂ is 6.94 × 10^-1 mol L^-1 s^-1,what is the rate of the loss of O₃? 2O₃(g)→ 3O₂(g)

A)0.463 mol L^-1 s^-1
B)1.04 mol L^-1 s^-1
C)2.08 mol L^-1 s^-1
D)0.231 mol L^-1 s^-1
E)4.16 mol L^-1 s^-1

Question 5

Given the following balanced equation,determine the rate of reaction with respect to [O₃].If the rate of loss of O₃ is 3.91 × 10^-1 mol L^-1 s^-1,what is the rate of the formation of O₂? 2O₃(g)→ 3O₂(g)

A)2.61 mol L^-1 s^-1
B)0.937 mol L^-1 s^-1
C)0.261 mol L^-1 s^-1
D)0.587 mol L^-1 s^-1
E)0.817 mol L^-1 s^-1

Question 6

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } { [ \mathrm { A } ] ( \mathrm { mol } \mathrm { L }^{ - 1 } )} & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \mathrm {~s} ^ { - 1 } \right) \\\hline 0.0143 & 3.00 \times 10 ^ { - 3 } \\0.0429 & 9.00 \times 10 ^ { - 3 } \\0.0715 & 1.5 \times 10 ^ { - 2 }\end{array}$$

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

Question 7

Given the following balanced equation,determine the rate of reaction with respect to [SO₂].
2SO₂(g)+ O₂(g)? 2SO₃(g)

A)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 2 } \right] } { \mathrm { D } t }$
B)Rate = + $\frac { 1 } { 2 }$ $\frac { \left. \Delta [\mathrm { SO } _ { 2 } \right] } { \Delta t }$
C)Rate = - $\frac { \Delta \left[ \mathrm { SO } _ { 2 } \right] } { \mathrm { D } t }$
D)Rate = + $\frac { 2 \Delta \left[ \mathrm { SO } _ { 2 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 8

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].
2NO(g)+ Cl₂(g)? 2NOCl(g)

A)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta [ \mathrm { NOCl } ] } { \Delta t }$
B)Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta [ \mathrm { NOCl } ] } { \Delta t }$
C)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta [ \mathrm { NO } ] } { \Delta t }$
D)Rate = - $\frac { 2 \Delta [ \mathrm { NOCl } ] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 9

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of NO loss is 1.68 × 10^-2 mol L^-1 s^-1,what is the rate of formation of NOCl? 2NO(g)+ Cl₂(g)→ 2NOCl(g)

A)1.68 × 10^-2 mol L^-1 s^-1
B)3.81 × 10^-2 mol L^-1 s^-1
C)5.05 × 10^-2 mol L^-1 s^-1
D)6.14 × 10^-2 mol L^-1 s^-1
E)1.45 × 10^-2 mol L^-1 s^-1

Question 10

Given the following balanced equation,determine the rate of reaction with respect to [SO₃].If the rate of SO₂ loss is 1.19 × 10^-3 mol L^-1 s^-1,what is the rate of formation of SO₃? 2SO₂(g)+ O₂(g)→ 2SO₃(g)

A)3.56 × 10^-3 mol L^-1 s^-1
B)1.19 × 10^-3 mol L^-1 s^-1
C)1.78 × 10^-3 mol L^-1 s^-1
D)1.42 × 10^-2 mol L^-1 s^-1
E)7.12 × 10^-3 mol L^-1 s^-1

Question 11

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L }^{ - 1} \mathrm {~s} ^ { - 1 } \right) \\\hline 0.20 & 0.0050 \\0.40 & 0.020 \\0.80 & 0.080\end{array}$$

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

Question 12

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2O₃(g)? 3O₂(g)

A)Rate = - $\frac { 2 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$
B)Rate = - $\frac { 2 } { 3 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$
C)Rate = + $\frac { 1 } { 3 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$
D)Rate = + $\frac { 3 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 13

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \\\hline 0.20 & 0.250 \\0.40 & 0.500 \\0.60 & 0.750\end{array}$$

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

Question 14

Write a balanced reaction for which the following rate relationships are true. Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { N } _ { 2 } \mathrm { O } _ { 5 } \right] } { \Delta t }$ = $\frac { 1 } { 4 }$ $\frac { \Delta \left[ \mathrm { NO } _ { 2 } \right] } { \Delta t }$ = $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$

A)2N₂O₅ ? 4NO₂ + O₂
B)4NO₂ + O₂ ? 2N₂O₅
C)2N₂O₅ ? NO₂ + 4O₂
D) $\frac { 1 } { 4 } \mathrm { NO } _ { 2 } + \mathrm { O } _ { 2 } \rightarrow \frac { 1 } { 2 } \mathrm {~N} _ { 2 } \mathrm { O } _ { 5 }$
E) $\frac { 1 } { 2 } \mathrm {~N} _ { 2 } \mathrm { O } _ { 5 } \rightarrow \frac { 1 } { 4 } \mathrm { NO } _ { 2 } + \mathrm { O } _ { 2 }$

Question 15

Given the following balanced equation,determine the rate of reaction with respect to [H₂].
N₂(g)+ 3H₂(g)? 2NH₃(g)

A)Rate = + $\frac { 3 \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$
B)Rate = - $\frac { 2 } { 3 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$
C)Rate = + $\frac { 3 } { 2 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$
D)Rate = - $\frac { 1 } { 3 }$ $\frac { \Delta \left[ \mathrm { H } _ { 2 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 16

Given the following balanced equation,determine the rate of reaction with respect to [NH₃]. N₂(g)+ 3H₂(g)? 2NH₃(g)

A)Rate = + $\frac { 2 \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }$
B)Rate = - $\frac { 2 \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }$
C)Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }$
D)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 17

Given the following balanced equation,determine the rate of reaction with respect to [SO₃].
2SO₂(g)+ O₂(g)? 2SO₃(g)

A)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \mathrm { D } t }$
B)Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \Delta t }$
C)Rate = - $\frac { \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \mathrm { D } t }$
D)Rate = + $\frac { 2 \Delta \left[ \mathrm { SO } _ { 3 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 18

Given the following balanced equation,determine the rate of reaction with respect to [O₃].
2O₃(g)? 3O₂(g)

A)Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 3 } \right] } { \Delta t }$
B)Rate = - $\frac { 1 } { 3 }$ $\frac { \Delta \left[ \mathrm { O } _ { 3 } \right] } { \Delta t }$
C)Rate = + $\frac { 1 } { 3 }$ $\frac { \Delta \left[ \mathrm { O } _ { 3 } \right] } { \mathrm { D } t }$
D)Rate = + $\frac { 3 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 3 } \right] } { \Delta t }$
E)It is not possible to determine the answer without more information.

Question 19

Given the following balanced equation,determine the rate of reaction with respect to [SO₃].If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1,what is the rate of formation of SO₃? 2SO₂(g)+ O₂(g)→ 2SO₃(g)

A)3.56 × 10^-3 mol L^-1 s^-1
B)1.19 × 10^-3 mol L^-1 s^-1
C)1.78 × 10^-3 mol L^-1 s^-1
D)1.42 × 10^-2 mol L^-1 s^-1
E)7.12 × 10^-3 mol L^-1 s^-1

Question 20

Write a balanced reaction for which the following rate relationships are true. Rate = $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { N } _ { 2 } \right] } { \Delta t }$ = $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$ = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { N } _ { 2 } \mathrm { O } \right] } { \Delta t }$

A) $\frac { 1 } { 2 }$ N₂ + O₂ ? $\frac { 1 } { 2 }$ N₂O
B)2N₂O ? 2N₂ + O₂
C)N₂O ? N₂ + 2O₂
D) $\frac { 1 } { 2 }$ N₂O ? $\frac { 1 } { 2 }$ N₂ + O₂
E)2N₂ + O₂ ? 2N₂O

Question 21

What is the overall order of the following reaction,given the rate law? NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)Rate = k[NO][O₃]

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

Question 22

What is the overall order of the following reaction,given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]¹[Y]²

A)3rd order
B)5th order
C)2nd order
D)1st order
E)0th order

Question 23

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

Question 24

What is the overall order of the following reaction,given the rate law? X + 2 Y → 4 Z Rate = k[X][Y]

A)3rd order
B)5th order
C)2nd order
D)1st order
E)0th order

Question 25

What is the unit of k in the following rate law?
Rate = k[X][Y]

A)mol L^-1 s^-1
B)mol L^-1 s
C)L mol^-1 s^-1
D) $\frac { \mathrm { M } ^ { 2 } } { \mathrm {~s} }$
E) $\frac { \mathrm { s } } { \mathrm { M } ^ { 2 } }$

Question 26

What is the unit of k in a zero-order reaction?

A)mol L^-1 s^-1
B)mol L^-1 s
C)L mol^-1 s^-1
D)M² s^-1
E)s^-1

Question 27

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

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 28

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

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 29

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

Question 30

Determine the missing initial rate for the following $\frac{3}{2}$ order reaction given the following information: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \\\hline 0.0174 & 0.16 \\0.0361 & ? \\0.0996 & 2.2\end{array}$$

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 31

What is the unit of k in a first-order reaction?

A)mol L^-1 s^-1
B)mol L^-1 s
C)L mol^-1 s^-1
D)M² s^-1
E)s^-1

Question 32

Determine the missing initial rate for a reaction with an order of $\frac{2}{5}$ given the following information: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \mathrm {~s} ^ { - 1 } \right) \\\hline 9.74 \times 10 ^ { - 5 } & 4.6 \times 10 ^ { - 3 } \\6.83 \times 10 ^ { - 4 } & ? \\9.74 \times 10 ^ { - 4 } & 1.2 \times 10 ^ { - 2 }\end{array}$$

A)6.0 × 10^-3 mol L^-1 s^-1
B)2.8 × 10^-2 mol L^-1 s^-1
C)7.3 × 10^-3 mol L^-1 s^-1
D)9.74 × 10^-3 mol L^-1 s^-1
E)1.0 × 10^-2 mol L^-1 s^-1

Question 33

What is the unit of k in the following rate law? Rate = k[X]²

A)mol L^-1 s^-1
B)mol L^-1 s
C)L mol^-1 s^-1
D)L mol^-2 s^-1
E)M² s^-1

Question 34

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \\\hline 0.35 & 0.038 \\0.70 & 0.038 \\1.05 & 0.038\end{array}$$

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

Question 35

What is the unit of k in the following rate law? Rate = k[X][Y]^1/2

A)mol L^-1 s^-1
B)L mol^-1 s^-1
C)L mol^-1/2 s^-1
D)L^1/2 mol^-1/2 s^-1
E)L mol^-1 s^-1/2

Question 36

What is the unit of k in the following rate law?
Rate = k[X][Y]²

A) $\frac { 1 } { \mathrm {~mol} \mathrm {~L} ^ { - 1 } \mathrm {~s} ^ { 2 } }$
B) $\frac { 1 } { \mathrm { M } ^ { 2 } \mathrm {~s} }$
C)M² s
D) $\frac { \mathrm { M } ^ { 2 } } { \mathrm {~s} }$
E) $\frac { 1 } { \mathrm { M } ^ { 3 } \mathrm {~s} }$

Question 37

What is the unit of k in a second-order reaction?

A)mol L^-1 s^-1
B)mol L^-1 s
C)L mol^-1 s^-1
D)M² s^-1
E)s^-1

Question 38

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

Question 39

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

Question 40

Determine the missing initial rate for the following $\frac{1}{2}$ order reaction given the following information: $$\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L }^{ - 1 }\mathrm {~s} ^ { - 1 } \right) \\\hline 0.8456 & 0.0326 \\0.6843 & 0.0293 \\0.4321 & ?\end{array}$$

A)0.0352 mol L^-1 s^-1
B)0.0301 mol L^-1 s^-1
C)0.0215 mol L^-1 s^-1
D)0.0233 mol L^-1 s^-1
E)0.0280 mol L^-1 s^-1

Question 41

Which of the following represents the integrated rate law for a zeroth-order reaction?

A) $\ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } = - k t$
B)
$\frac { 1 } { [ \mathrm {~A} ] _ { t } } - \frac { 1 } { [ \mathrm {~A} ] _ { 0 } } = k t$
C)[A]_t - [A]₀ = -kt
D)k = Ae^(-E_a/RT)
E) $\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \ln \mathrm { A }$

Question 42

What data should be plotted to show that experimental concentration data fit a first-order reaction?

A) $\frac { 1 } { [ \text { reactant] } }$ vs.time
B)[reactant] vs.time
C)ln[reactant] vs.time
D)ln(k)vs. $\frac { 1 } { T }$
E)ln(k)vs.E_a

Question 43

Which of the following represents the equation for a zero-order half-life?

A) $t 1 / 2 = \frac { 1 } { k [ \mathrm {~A} ] _ { 0 } }$
B) $t 1 / 2 = \frac { 0.693 } { k }$
C) $t 1 / 2 = \frac { [ \mathrm { A } ] _ { 0 } } { 2 k }$
D) $t 1 / 2 = \frac { 2 k } { [ \mathrm {~A} ] _ { 0 } }$
E) $t 1 / 2 = \frac { k } { [ \mathrm {~A} ] _ { 0 } }$

Question 44

What data should be plotted to show that experimental concentration data fit a zeroth-order reaction?

A)ln[reactant] vs.time
B) $\frac { 1 } { [ \text { reactant] } }$ vs.time
C)ln(k)vs. $\frac { 1 } { T }$
D)ln(k)vs.E_a
E)[reactant] vs.time

Question 45

Which of the following represents the equation for a second-order half-life?

A) $t 1 / 2 = \frac { 1 } { k [ \mathrm {~A} ] _ { 0 } }$
B) $t 1 / 2 = \frac { 0.693 } { k }$
C) $t 1 / 2 = \frac { [ \mathrm { A } ] _ { 0 } } { 2 k }$
D) $t 1 / 2 = \frac { 2 k } { [ \mathrm {~A} ] _ { 0 } }$
E) $t 1 / 2 = \frac { k } { [ \mathrm {~A} ] _ { 0 } }$

Question 46

Which of the following represents the integrated rate law for a second-order reaction?

A) $\ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } = - k t$
B) $\frac { 1 } { [ \mathrm {~A} ] _ { t } } - \frac { 1 } { [ \mathrm {~A} ] _ { 0 } } = k t$
C)[A]_t - [A]₀ = -kt
D)k = Ae^(-E_a/RT)
E) $\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \ln \mathrm { A }$

Question 47

Which of the following statements is FALSE?

A)The average rate of a reaction decreases during a reaction.
B)It is not possible to determine the rate of a reaction from its balanced equation.
C)The rate of zero-order reactions is not dependent on concentration.
D)The half-life of a first-order reaction is dependent on the initial concentration of reactant.
E)None of the above statements is false.

Question 48

Which of the following represents the equation for a first-order half-life?

A)
$t 1 / 2 = \frac { 1 } { k [ \mathrm {~A} ] _ { 0 } }$
B) $t 1 / 2 = \frac { 0.693 } { k }$
C) $t 1 / 2 = \frac { [ \mathrm { A } ] _ { 0 } } { 2 k }$
D) $t 1 / 2 = \frac { 2 k } { [ \mathrm {~A} ] _ { 0 } }$
E) $t 1 / 2 = \frac { k } { [ \mathrm {~A} ] _ { 0 } }$

Question 49

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

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 50

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

A)3
B)1
C)1.75
D)2.75
E)2

Question 51

Determine the rate law and the value of k for the following reaction using the data provided: NO₂(g)+ O₃(g)→ NO₃(g)+ O₂(g)[NO₂]_i (M)[O₃]_i (M)Initial Rate (M^-1 s^-1)
0.10 0.33 1.42
0.10 0.66 2.84
0.25 0.66 7.10

A)Rate = 1360 M^-2.5 s^-1[NO₂]^2.5[O₃]
B)Rate = 227 M^-2.5 s^-1[NO₂][O₃]^2.5
C)Rate = 43 M^-1 s^-1[NO₂][O₃]
D)Rate = 430 M^-2 s^-1[NO₂]²[O₃]
E)Rate = 130 M^-2 s^-1[NO₂][O₃]²

Question 52

Determine the rate law and the value of k for the following reaction using the data provided: S₂O₈^2-(aq)+ 3 I^- (aq)→ 2 SO₄^2- (g)+ I₃^- (aq)[S₂O₈^2-]_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

A)Rate = 120 M^-2 s^-1 [S₂O₈^2-]²[I^-]
B)Rate = 36 M^-1 s^-1 [S₂O₈^2-][I^-]
C)Rate = 86 M^-2 s^-1 [S₂O₈^2-][I^-]²
D)Rate = 195 M^-3 s^-1 [S₂O₈^2-]²[I^-]²
E)Rate = 23 M^-1/2 s^-1 [S₂O₈^2-][I^-]^1/2

Question 53

Determine the rate law and the value of k for the following reaction using the data provided: 2N₂O₅(g)→ 4NO₂(g)+ O₂(g)[N₂O₅]_i (M)Initial Rate (M^-1 s^-1)
0.093 4.84 × 10^-4
0.186 9.67 × 10^-4
0.279 1.45 × 10^-3

A)Rate = 5.6 × 10^-2 M^-1 s^-1[N₂O₅]²
B)Rate = 6.0 × 10^-1 M^-2 s^-1[N₂O₅]³
C)Rate = 1.6 × 10^-3 M^1/2 s^-1[N₂O₅]^1/2
D)Rate = 1.7 × 10^-2 M^-1/2 s^-1[N₂O₅]^3/2
E)Rate = 5.2 × 10⁻³ s^-1[N₂O₅]

Question 54

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

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 55

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

A)1
B)3
C)1.5
D)2.5
E)2

Question 56

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g)+ O₂(g)→ 2NO₂(g)[NO]_i (M)[O₂]_i (M)Initial Rate (M^-1 s^-1)
0.030 0.0055 8.55 × 10^-3
0.030 0.0110 1.71 × 10^-2
0.060 0.0055 3.42 × 10^-2

A)Rate = 57 M^-1 s^-1[NO][O₂]
B)Rate = 3.8 M^-1/2 s^-1[NO][O₂]^1/2
C)Rate = 3.1 × 10⁵ M^-3 s^-1[NO]²[O₂]²
D)Rate = 1.7 × 10³ M^-2 s^-1[NO]²[O₂]
E)Rate = 9.4 × 10³ M^-2 s^-1[NO][O₂]²

Question 57

Determine the rate law and the value of k for the following reaction using the data provided: CO(g)+ Cl₂(g)→ COCl₂(g)[CO]_i (M)[Cl₂]_i (M)Initial Rate (M¹ s^-1)
0.25 0.40 0.696
0.25 0.80 1.97
0.50 0.80 3.94

A)Rate = 11 M^-3/2 s^-1 [CO][Cl₂]^3/2
B)Rate = 36 M^-1.8 s^-1 [CO][Cl₂]^2.8
C)Rate = 17 M^-2 s^-1 [CO][Cl₂]²
D)Rate = 4.4 M^-1/2 s^-1 [CO][Cl₂]^1/2
E)Rate = 18 M^-3/2 s^-1 [CO]²[Cl₂]^1/2

Question 58

Which of the following represents the integrated rate law for a first-order reaction?

A) $\ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } = - k t$
B) $\frac { 1 } { [ \mathrm {~A} ] _ { t } } - \frac { 1 } { [ \mathrm {~A} ] _ { 0 } } = k t$
C)[A]_t - [A]₀ = -kt
D)k = Ae^(-E_a/RT)
E)
$\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \mid \ln \mathrm { A }$

Question 59

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

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 60

What data should be plotted to show that experimental concentration data fit a second-order reaction?

A)ln[reactant] vs.time
B)[reactant] vs.time
C)ln(k)vs. $\frac { 1 } { T }$
D) $\frac { 1 } { [ \text { reactant] } }$ vs.time
E)ln(k)vs.E_a

Question 61

The rate constant for the first-order decomposition of N₂O is 3.40 s^-1.What is the half-life of the decomposition?

A)0.491 s
B)0.204 s
C)0.236 s
D)0.424 s
E)0.294 s

Question 62

The rate constant for a second-order reaction is 0.54 L mol^-1 s^-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?

A)2.0 s
B)5.0 s
C)0.25 s
D)6.9 s
E)1.3 s

Question 63

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 mol L^-1.What is the rate constant for this reaction?

A)1.0 × 10^-2 L mol^-1 s^-1
B)4.5 × 10^-2 L mol^-1 s^-1
C)9.7 × 10^-2 L mol^-1 s^-1
D)2.2 × 10^-2 L mol^-1 s^-1
E)3.8 × 10^-2 L mol^-1 s^-1

Question 64

The half-life for the decay of radium is 1620 years.What is the rate constant for this first-order process?

A)4.28 × 10^-4 yr^-1
B)1.12 × 10^-4 yr^-1
C)2.33 × 10^-4 yr^-1
D)8.91 × 10^-4 yr^-1
E)6.17 × 10^-4 yr^-1

Question 65

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 2.88 mol L^-1,what is the concentration of N₂O₅ after 12.5 minutes?

A)0.124 mol L^-1
B)0.805 mol L^-1
C)2.82 mol L^-1
D)0.355 mol L^-1
E)0.174 mol L^-1

Question 66

Which of the following reactions would you predict to have the smallest orientation factor?

A)X₂ + Y₂ → 2XY
B)NOCl₂ + NO → 2 NOCl
C)N₂ + O₂ → 2NO
D)N + O₂ → NO₂
E)All of these reactions should have nearly identical orientation factors.

Question 67

Derive an expression for a "1/4-life" for a first-order reaction.

A) $\frac { \ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } } { - k }$
B) $\frac { 0.347 } { k }$
C) $\frac { \ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } } { - 4 k }$
D) $\frac { 4 } { k }$
E) $\frac { 1.386 } { k }$

Question 68

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

A)6
B)5
C)7
D)6.5
E)7.5

Question 69

The rate constant for a zero-order reaction is 0.54 L mol^-1 s^-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?

A)2.0 s
B)5.0 s
C)0.25 s
D)6.9 s
E)1.3 s

Question 70

The second-order decomposition of NO₂ has a rate constant of 0.255 L mol^-1 s^-1.How much NO₂ decomposes in 4.00 s if the initial concentration of NO₂ (1.00 L volume)is 1.33 mol L^-1?

A)1.8 mol
B)0.85 mol
C)0.48 mol
D)0.77 mol
E)0.56 mol

Question 71

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10^-4 s^-1.If the initial concentration of cyclopropane is 1.33 mol L^-1,what is the concentration of cyclopropane after 644 s?

A)0.43 mol L^-1
B)0.15 mol L^-1
C)0.94 mol L^-1
D)0.86 mol L^-1
E)0.67 mol L^-1

Question 72

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

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

Question 73

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?

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

Question 74

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

A)83.4 g
B)16.6 g
C)50.0 g
D)36.6 g
E)63.4 g

Question 75

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 L mol^-1 s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 mol L^-1?

A)4.55 mol L^-1
B)0.258 mol L^-1
C)3.87 mol L^-1
D)2.20 mol L^-1
E)2.39 mol L^-1

Question 76

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1.If the initial concentration of N₂O is 10.9 mol L^-1,what is the concentration of N₂O after 9.6 s?

A)7.4 × 10^-3 mol L^-1
B)1.0 × 10^-3 mol L^-1
C)1.4 × 10^-3 mol L^-1
D)3.6 × 10^-3 mol L^-1
E)8.7 × 10^-3 mol L^-1

Question 77

Derive an expression for a "1/3-life" for a first-order reaction.

A) $\frac { \ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } } { - k }$
B) $\frac { 0.462 } { k }$
C) $\frac { \ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } } { - 3 k }$
D) $\frac { 1.099 } { k }$
E) $\frac { 3 } { k }$

Question 78

The rate constant for a first-order reaction is 0.54 L mol^-1 s^-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?

A)2.0 s
B)5.0 s
C)0.25 s
D)6.9 s
E)1.3 s

Question 79

Which of the following reactions would you predict to have the largest orientation factor?

A)NOF(g)+ NOF(g)→ 2NO(g)+ F₂(g)
B)Br₂(g)+ H₂C=CH₂(g)→ H₂BrC-CBrH₂(g)
C)NH₃(g)+ BCl₃(g)→ H₃N-BCl₃(g)
D)H(g)+ Cl(g)→ HCl(g)
E)All of these reactions should have nearly identical orientation factors.

Question 80

For a reaction,what generally happens if the temperature is increased?

A)a decrease in k occurs,which results in a faster rate
B)a decrease in k occurs,which results in a slower rate
C)an increase in k occurs,which results in a faster rate
D)an increase in k occurs,which results in a slower rate
E)there is no change to either k or the rate