Question 1

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 2

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?

Accepted Answer

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

Question 3

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

Accepted Answer

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) $t 1 / 2 = \frac { k } { [ \mathrm {~A} ] _ { 0 } }$ 
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 4

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

Accepted Answer

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)  $\frac { 1.386 } { k }$ 
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 5

A reaction with an activation energy of 61.0 kJ mol-1 has a rate constant of 0.0345 L mol-1 s-1 at 301 K.What is the rate constant at 401 K?

Accepted Answer

A) 1.92 L mol-1 s-1 
B) 7.90 × 10-5 L mol-1 s-1 
C) 0.0445 L mol-1 s-1 
D) 0.345 L mol-1 s-1 
E) 15.1 L mol-1 s-1 
A) 1.92 L mol-1 s-1 
B) 7.90 × 10-5 L mol-1 s-1 
C) 0.0445 L mol-1 s-1 
D) 0.345 L mol-1 s-1 
E) 15.1 L mol-1 s-1

Question 6

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s-1 and an activation energy,Ea,of 68.4 kJ mol-1 at 305 K.

Accepted Answer

A) 4.1 × 103 s-1 
B) 8.1 × 103 s-1 
C) 8.1 × 1015 s-1 
D) 4.1 × 1015 s-1 
E) 1.0 × 104 s-1 
A) 4.1 × 103 s-1 
B) 8.1 × 103 s-1 
C) 8.1 × 1015 s-1 
D) 4.1 × 1015 s-1 
E) 1.0 × 104 s-1

Question 7

The decomposition of $\mathrm { N } _ { 2 }$ $\mathrm { O } _ { 5 }$ in solution in carbon tetrachloride proceeds via the reaction 
2N2O5 (soln)? $4 \mathrm { NO } _ { 2 }$ (soln)+ $\mathrm { O } _ { 2 }$ (soln)
The reaction is first order and has a rate constant of 4.82 × $10 ^ { - 3 }$ $s ^ { - 1 }$ at 64 °C.If the reaction is initiated with 0.073 mol in a 1.00 L vessel,how many moles remain after 151 s?

Accepted Answer

A) 0.077 mol 
B) 0.053 mol 
C) 0.038 mol 
D) 15 mol 
E) 0.035 mol 
A) 0.077 mol 
B) 0.053 mol 
C) 0.038 mol 
D) 15 mol 
E) 0.035 mol

Question 8

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

Accepted Answer

A) mol L-1 s-1 
B) mol L-1 s 
C) L mol-1 s-1 
D) M2 s-1 
E) s-1 
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 9

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

Accepted Answer

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. 
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 10

Which of the following is the characteristic of a zero-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.

Question 11

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

Accepted Answer

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(-Ea/RT) 
E) 
$\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \mid \ln \mathrm { A }$ 
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(-Ea/RT) 
E) 
$\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \mid \ln \mathrm { A }$

Question 12

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

Accepted Answer

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(-Ea/RT) 
E)  $\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \ln \mathrm { A }$ 
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(-Ea/RT) 
E)  $\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right) + \ln \mathrm { A }$

Question 13

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

Accepted Answer

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 
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

Question 14

What is the activation energy for a reaction that has a rate constant of 1.087 L mol-1 s-1 at 273 and 12.99 L mol-1 s-1 at 373 K?

Accepted Answer

A) 48.6 kJ mol-1 
B) 18.4 kJ mol-1 
C) 37.9 kJ mol-1 
D) 12.7 kJ mol-1 
E) 21.0 kJ mol-1 
A) 48.6 kJ mol-1 
B) 18.4 kJ mol-1 
C) 37.9 kJ mol-1 
D) 12.7 kJ mol-1 
E) 21.0 kJ mol-1

Question 15

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

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

Question 16

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 5.30 × 10 -6 L mol-1 s-1 at 298 K.At what temperature will the rate constant be 0.530 L mol-1 s-1?

Accepted Answer

A) 461 K 
B) 410 K 
C) 310 K 
D) 495 K 
E) 328 K 
A) 461 K 
B) 410 K 
C) 310 K 
D) 495 K 
E) 328 K

Question 17

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g).
If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment,what is the rate of appearance of NO2 at that moment?

Accepted Answer

A) 0.800 mol min-1 
B) 1.60 mol min-1 
C) 3.20 mol min-1 
D) 6.40 mol min-1 
A) 0.800 mol min-1 
B) 1.60 mol min-1 
C) 3.20 mol min-1 
D) 6.40 mol min-1

Question 18

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?

Accepted Answer

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 
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 19

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?

Accepted Answer

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

Question 20

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

Accepted Answer

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. 
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.

Exam 13: Chemical Kinetics

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.

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?

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

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

A reaction with an activation energy of 61.0 kJ mol-1 has a rate constant of 0.0345 L mol-1 s-1 at 301 K.What is the rate constant at 401 K?

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s-1 and an activation energy,Ea,of 68.4 kJ mol-1 at 305 K.

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

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

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

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

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

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

What is the activation energy for a reaction that has a rate constant of 1.087 L mol-1 s-1 at 273 and 12.99 L mol-1 s-1 at 373 K?

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: [] Initial Rate 0.20 0.250 0.40 0.500 0.60 0.750

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 5.30 × 10 -6 L mol-1 s-1 at 298 K.At what temperature will the rate constant be 0.530 L mol-1 s-1?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g). If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment,what is the rate of appearance of NO2 at that moment?

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?

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?

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

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Filters

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.

A reaction with an activation energy of 61.0 kJ mol^-1 has a rate constant of 0.0345 L mol^-1 s^-1 at 301 K.What is the rate constant at 401 K?

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s^-1 and an activation energy,E_a,of 68.4 kJ mol^-1 at 305 K.

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

What is the activation energy for a reaction that has a rate constant of 1.087 L mol^-1 s^-1at 273 and 12.99 L mol^-1 s^-1 at 373 K?

A reaction with an activation energy of 71.6 kJ mol^-1 has a rate constant of 5.30 × 10 ^-6 L mol^-¹ s^-1 at 298 K.At what temperature will the rate constant be 0.530 L mol^-1 s^-1?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g)→ 4NO₂(g)+ O₂(g). If the rate of disappearance of N₂O₅ is equal to 1.60 mol min^-1 at a particular moment,what is the rate of appearance of NO₂ at that moment?

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?

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

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