Exam 13: Chemical Kinetics

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) $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.093 $\quad$ 4.84 × 10^-4 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.186 $\quad$ 9.67 × 10^-4 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.279 $\quad$ 1.45 × 10^-3

Calculate the activation energy,E_a,for a reaction with a frequency factor,A,of 6.10 × 10¹⁴ s^-1 and a rate constant of 13.0 s^-1 at 320 K.

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

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

Which of the following statements is TRUE?

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

Explain how the order of a reaction can be determined.

For the first-order reaction,2N₂O(g)? 2N₂(g)+ O₂(g),what is the concentration of N₂O after 3 half-lives if $0.25$ mol of N₂O is initially placed into a 1.00 L reaction vessel?

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

Calculate the temperature if a reaction has a rate constant,k,of 21.3 s^-1,a frequency factor,A,of 7.98 × 10¹³ s^-1,and an activation energy,E_a,of 102 kJ mol^-1.

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

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g)→ 4NO₂(g)+ O₂(g). If the rate of appearance of NO₂ is equal to 0.560 mol min^-1 at a particular moment,what is the rate of appearance of O₂ at that moment?

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

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) $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.030 $\quad$ 0.0055 $\quad$ 8.55 × 10^-3 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.030 $\quad$ 0.0110 $\quad$ 1.71 × 10^-2 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.060 $\quad$ 0.0055 $\quad$ 3.42 × 10^-2

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?

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

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) $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.10 $\quad$ 0.33 $\quad$$\quad$ 1.42 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.10 $\quad$ 0.66 $\quad$$\quad$ 2.84 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ 0.25 $\quad$ 0.66 $\quad$$\quad$ 7.10

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

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction?

Identify the rate-determining step.