Question 1

What is the rate constant (s^-1)for this reaction?

Accepted Answer

The rate constant is given as 7.8 × 10^-2^-2.

Question 2

What is the concentration (M)of [A] after 80.0 s?

Accepted Answer

Using the integrated rate law for a second-order reaction, we can solve for the concentration of A after 80.0 s:

1/[A] - 1/[A]₀ = kt

where [A]₀ is the initial concentration of A, k is the rate constant, t is time, and [A] is the concentration of A at time t.

Plugging in the values given in the problem:

1/[A] - 1/0.10 = (0.0220 M⁻¹s⁻¹)(80.0 s)

Solving for [A], we get:

[A] = 4.06 × 10⁻⁴ M

The answer is therefore D (4.06 × 10⁻⁴ M), which is closest to 4.06 × 10⁻⁴ M.

Question 3

Of the following,all are valid units for a reaction rate except ________.

Accepted Answer

Reaction rate is typically expressed in terms of concentration change over time, such as M/s (molarity per second) or mol/L-hr (moles per liter per hour). "mol/L" is a concentration unit, not a rate unit, and does not include a time component, making it invalid for expressing reaction rate.

Question 4

What is the order of the reaction with respect to ClO₂?

Accepted Answer

The order of the reaction with respect to ClO₂ is 2, indicating that the rate of reaction is proportional to the square of the concentration of ClO₂.

Question 5

Which one of the following graphs shows the correct relationship between concentration and time for a reaction that is second order in [A]?

Accepted Answer

The answer of Which one of the following graphs shows...

Question 6

The rate constant of a first-order process that has a half-life of 3.50 min is ________ s^-1.

Accepted Answer

The answer of The rate constant of a first-order process...

Question 7

The following reaction is second order in [A] and the rate constant is 0.025   : A → B
The concentration of A was 0.65 M at 33 s.The initial concentration of A was ________ M.

Accepted Answer

The answer of The following reaction is second order in...

Question 8

One difference between first- and second-order reactions is that ________.

Accepted Answer

The half-life of a first-order reaction is dependent on the initial concentration of the reactant ([A]0), while the half-life of a second-order reaction is dependent on the square of the initial concentration of the reactant ([A]0^2). Therefore, the half-life of a first-order reaction does not depend on [A]1/2, but the half-life of a second-order reaction does depend on [A]1/2.

Question 9

Which one of the following is not a valid expression for the rate of the reaction below? 4NH₃ + 7O₂ → 4NO₂ + 6H₂O

Accepted Answer

The answer of Which one of the following is not...

Question 10

The magnitude of the rate constant is ________.

Accepted Answer

The magnitude of the rate constant is 5.56.

Question 11

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction.At If is 1.00 × 10^-3 initially, is ________ M after

Accepted Answer

The answer of The reaction CH₃-N≡C → CH₃-C≡N Is a first-order...

Question 12

Under constant conditions,the half-life of a first-order reaction ________.

Accepted Answer

All the statements provided are characteristics of a first-order reaction's half-life. It is defined as the time required for the reactant concentration to decrease to half its initial value (A), remains constant regardless of the concentration (B and D), and can be calculated if the rate constant is known (C).

Question 13

Which of the following is correct regarding the overall order of the reaction?

Accepted Answer

The overall order of the reaction is determined by adding the individual orders of each reactant. The given reaction is ClO^- + OH^- → Cl^- + O2^- + H2O, therefore the individual orders are 2 for ClO^- and 1 for OH^-. Adding these together gives an overall order of 3 for the reaction. Therefore, choice C is correct.

Question 14

What is the order of the reaction with respect to OH^-?

Accepted Answer

The order of a reaction with respect to a specific reactant is determined by the exponent of its concentration in the rate law equation. The notation "OH^-" suggests a single unit (S1) of the reactant is involved in the rate-determining step, indicating a first-order reaction with respect to that reactant.

Question 15

The rate law of a reaction is rate = k[D][X].The units of the rate constant are ________.

Accepted Answer

The rate law is second order overall (first order in [D] and first order in [X]), so the units of the rate constant k are L mol^-1s^-1.

Question 16

What is the magnitude of the rate constant for the reaction?

Accepted Answer

The magnitude of the rate constant is 230, as indicated by the choice that matches the given value.

Question 17

The reaction 2NO₂ → 2NO + O₂ Follows second-order kinetics.At 300 °C,[NO₂] drops from 0.0100 M to 0.00650 M in 100.0 s.The rate constant for the reaction is ________ M^-1s^-1.

Accepted Answer

The answer of The reaction 2NO₂ → 2NO + O₂ Follows...

Question 18

The reaction A (aq)→ B (aq)is first order in [A].A solution is prepared with [A] = 1.22 M.The following data are obtained as the reaction proceeds: The rate constant for this reaction is ________ s^-1.

Accepted Answer

The answer of The reaction A (aq)→ B (aq)is first...

Question 19

A burning splint will burn more vigorously in pure oxygen than in air because ________.

Accepted Answer

Oxygen is necessary for combustion to occur, and the concentration of oxygen in pure oxygen is higher than in air, making the combustion reaction more vigorous. Oxygen is not a catalyst for combustion, nor is it a product of combustion. Nitrogen does not play a significant role in combustion, and its low concentration in pure oxygen does not catalyze the reaction.

Question 20

The rate law for this reaction is rate = ________.

Accepted Answer

The answer of The rate law for this reaction is...

Quiz 14: Chemical Kinetics

What is the rate constant (s^-1) for this reaction?

What is the concentration (M) of [A] after 80.0 s?

Of the following,all are valid units for a reaction rate except ________.

What is the order of the reaction with respect to ClO₂?

Which one of the following graphs shows the correct relationship between concentration and time for a reaction that is second order in [A]?

The rate constant of a first-order process that has a half-life of 3.50 min is ________ s^-1.

The following reaction is second order in [A] and the rate constant is 0.025 : A → B The concentration of A was 0.65 M at 33 s.The initial concentration of A was ________ M.

One difference between first- and second-order reactions is that ________.

Which one of the following is not a valid expression for the rate of the reaction below? 4NH₃ + 7O₂ → 4NO₂ + 6H₂O

The magnitude of the rate constant is ________.

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction.At If is 1.00 × 10^-3 initially, is ________ M after

Under constant conditions,the half-life of a first-order reaction ________.

Which of the following is correct regarding the overall order of the reaction?

What is the order of the reaction with respect to OH^-?

The rate law of a reaction is rate = k[D][X].The units of the rate constant are ________.

What is the magnitude of the rate constant for the reaction?

The reaction 2NO₂ → 2NO + O₂ Follows second-order kinetics.At 300 °C,[NO₂] drops from 0.0100 M to 0.00650 M in 100.0 s.The rate constant for the reaction is ________ M^-1s^-1.

The reaction A (aq) → B (aq) is first order in [A].A solution is prepared with [A] = 1.22 M.The following data are obtained as the reaction proceeds: The rate constant for this reaction is ________ s^-1.

A burning splint will burn more vigorously in pure oxygen than in air because ________.

The rate law for this reaction is rate = ________.

Quiz 14: Chemical Kinetics

What is the rate constant (s-1) for this reaction?

What is the concentration (M) of [A] after 80.0 s?

Of the following,all are valid units for a reaction rate except ________.

What is the order of the reaction with respect to ClO2?

Which one of the following graphs shows the correct relationship between concentration and time for a reaction that is second order in [A]?

The rate constant of a first-order process that has a half-life of 3.50 min is ________ s-1.

The following reaction is second order in [A] and the rate constant is 0.025 : A → B The concentration of A was 0.65 M at 33 s.The initial concentration of A was ________ M.

One difference between first- and second-order reactions is that ________.

Which one of the following is not a valid expression for the rate of the reaction below? 4NH3 + 7O2 → 4NO2 + 6H2O

The magnitude of the rate constant is ________.

The reaction CH3-N≡C → CH3-C≡N Is a first-order reaction.At If is 1.00 × 10-3 initially, is ________ M after

Under constant conditions,the half-life of a first-order reaction ________.

Which of the following is correct regarding the overall order of the reaction?

What is the order of the reaction with respect to OH-?

The rate law of a reaction is rate = k[D][X].The units of the rate constant are ________.

What is the magnitude of the rate constant for the reaction?

The reaction 2NO2 → 2NO + O2 Follows second-order kinetics.At 300 °C,[NO2] drops from 0.0100 M to 0.00650 M in 100.0 s.The rate constant for the reaction is ________ M-1s-1.

The reaction A (aq) → B (aq) is first order in [A].A solution is prepared with [A] = 1.22 M.The following data are obtained as the reaction proceeds: The rate constant for this reaction is ________ s-1.

A burning splint will burn more vigorously in pure oxygen than in air because ________.

The rate law for this reaction is rate = ________.

What is the rate constant (s^-1) for this reaction?

What is the order of the reaction with respect to ClO₂?

The rate constant of a first-order process that has a half-life of 3.50 min is ________ s^-1.

Which one of the following is not a valid expression for the rate of the reaction below? 4NH₃ + 7O₂ → 4NO₂ + 6H₂O

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction.At If is 1.00 × 10^-3 initially, is ________ M after

What is the order of the reaction with respect to OH^-?

The reaction 2NO₂ → 2NO + O₂ Follows second-order kinetics.At 300 °C,[NO₂] drops from 0.0100 M to 0.00650 M in 100.0 s.The rate constant for the reaction is ________ M^-1s^-1.

The reaction A (aq) → B (aq) is first order in [A].A solution is prepared with [A] = 1.22 M.The following data are obtained as the reaction proceeds: The rate constant for this reaction is ________ s^-1.