Question 1

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

Accepted Answer

All of the statements are true for a first-order reaction under constant conditions. The half-life is the time required for the concentration of the reactant to decrease by half, and it is constant for a given reaction. It can be calculated using the reaction rate constant, which is also constant for first-order reactions. The half-life does not depend on the initial reactant concentration, only on the rate constant.

Question 2

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂ → 2NO + O₂ In a particular experiment at 300 °C, [NO₂] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO₂ for this period is __________ M/s.

Accepted Answer

C

Question 3

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

Accepted Answer

C

Question 4

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

Accepted Answer

The answer of Of the following, all are valid units...

Question 5

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10^-⁴s^-1. If [CH₃-NC] is 1.00 × 10^-³ initially, [CH₃-NC] is __________ after 1.000 × 10³ s.

Accepted Answer

The integrated rate law for a first-order reaction is:ln[A]t = -kt + ln[A]0where [A]t is the concentration of the reactant at time t, k is the rate constant, and [A]0 is the initial concentration of the reactant.Substituting the given values into the integrated rate law, we get:ln(1.00 × 10^-3) = -(6.29 × 10^-4 s^-1)(1.000 × 10^3 s) + ln[CH3-N≡C]0Solving for [CH3-N≡C]0, we get:[CH3-N≡C]0 = 5.33 × 10^-4

Question 6

A compound decomposes by a first-order process. If 17.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is __________.

Accepted Answer

The answer of A compound decomposes by a first-order process....

Question 7

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

Accepted Answer

The rate constant is defined as the proportionality constant between the rate and the concentrations of reactants raised to their respective orders in the rate law. In this case, the rate law is rate = k[D][X], which indicates a second order reaction with respect to both reactants. The units of rate are usually expressed as mol L^-1 s^-1, while the units of concentration are mol L^-1. Therefore, to obtain the units of the rate constant k, we need to cancel out the units of concentration and time by dividing the rate units by the concentration units raised to their respective orders. This gives: k = rate/([D][X]) = (mol L^-1 s^-1)/(mol L^-1)^2 = L mol^-1 s^-1. So, the correct answer is B.

Question 8

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

Accepted Answer

The question is not providing enough information to determine the order of the reaction with respect to OH^-. Without further information or data, it is impossible to determine the order of the reaction with respect to OH^-. However, it is important to note that the order of a reaction can only be determined experimentally through various methods like the method of initial rates, integrated rate laws, and the graphical method.

Question 9

The rate law for this reaction is rate = __________.

Accepted Answer

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

Question 10

The rate law for a reaction is rate = k [A][B]² Which one of the following statements is false?

Accepted Answer

The reaction is third order overall, not second order. It is first order in A and second order in B, making it third order overall.

Question 11

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

Accepted Answer

According to the rate law, rate = k[NO][O3]. 
Plugging in the given initial concentrations and initial rate: 
1.15 x 10^-4 M/s = k(0.10 M)(0.010 M) 
Solving for k: k = 230 M^-1 s^-1.

Question 12

Of the units below, __________ are appropriate for a first-order reaction rate constant.

Accepted Answer

The correct units for a first-order reaction rate constant are s^-1. Option B has the correct units of s^-1, indicating that it is suitable for a first-order reaction rate constant. The other units listed are not appropriate for a first-order reaction rate constant.

Question 13

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 14

At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N₂O₅(g)→ 4NO₂(g)+ O₂ (g) When the rate of formation of O₂ is 2.2 × 10^-4 M/s, the rate of decomposition of N₂O₅ is __________ M/s.

Accepted Answer

The stoichiometry of the reaction shows that 2 moles of N2O5 decompose to produce 1 mole of O2. Therefore, the rate of decomposition of N2O5 is twice the rate of formation of O2, which is 4.4 × 10^-4 M/s.

Question 15

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 16

The magnitude of the rate constant is __________.

Accepted Answer

The answer of The magnitude of the rate constant is...

Question 17

What is the overall order of the reaction?

Accepted Answer

The answer of What is the overall order of the...

Question 18

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is __________.

Accepted Answer

The answer of A compound decomposes by a first-order process....

Question 19

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

Accepted Answer

Oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than in air. This means that more oxygen is available for the combustion reaction to occur, resulting in a more vigorous burning of the splint.

Question 20

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...

Quiz 14: Chemical Kinetics

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

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂ → 2NO + O₂ In a particular experiment at 300 °C, [NO₂] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO₂ for this period is __________ M/s.

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

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

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10^-⁴s^-1. If [CH₃-NC] is 1.00 × 10^-³ initially, [CH₃-NC] is __________ after 1.000 × 10³ s.

A compound decomposes by a first-order process. If 17.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is __________.

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

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

The rate law for this reaction is rate = __________.

The rate law for a reaction is rate = k [A][B]² Which one of the following statements is false?

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

Of the units below, __________ are appropriate for a first-order reaction rate constant.

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.

At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N₂O₅(g) → 4NO₂(g) + O₂ (g) When the rate of formation of O₂ is 2.2 × 10^-4 M/s, the rate of decomposition of N₂O₅ is __________ M/s.

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

The magnitude of the rate constant is __________.

What is the overall order of the reaction?

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is __________.

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

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

Quiz 14: Chemical Kinetics

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

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300 °C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO2 for this period is __________ M/s.

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

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

The reaction CH3-N≡C → CH3-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10-4s-1. If [CH3-NC] is 1.00 × 10-3 initially, [CH3-NC] is __________ after 1.000 × 103 s.

A compound decomposes by a first-order process. If 17.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is __________.

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

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

The rate law for this reaction is rate = __________.

The rate law for a reaction is rate = k [A][B]2 Which one of the following statements is false?

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

Of the units below, __________ are appropriate for a first-order reaction rate constant.

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.

At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N2O5(g) → 4NO2 (g) + O2 (g) When the rate of formation of O2 is 2.2 × 10-4 M/s, the rate of decomposition of N2O5 is __________ M/s.

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

The magnitude of the rate constant is __________.

What is the overall order of the reaction?

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is __________.

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

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

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂ → 2NO + O₂ In a particular experiment at 300 °C, [NO₂] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO₂ for this period is __________ M/s.

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

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10^-⁴s^-1. If [CH₃-NC] is 1.00 × 10^-³ initially, [CH₃-NC] is __________ after 1.000 × 10³ s.

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

The rate law for a reaction is rate = k [A][B]² Which one of the following statements is false?

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.

At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N₂O₅(g) → 4NO₂(g) + O₂ (g) When the rate of formation of O₂ is 2.2 × 10^-4 M/s, the rate of decomposition of N₂O₅ is __________ M/s.

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