Question 1

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g)→ (g)+ (g) Is 0.301 mol L^-1 At 150 °C.The rate of appearance of Is ________ mol L^-1 .

Accepted Answer

The answer of The rate of disappearance of HBr in...

Question 2

For the second-order reaction A → products,the following data are obtained:
[A] = 1.512 M,t = 0 min
[A] = 1.490 M,t = 1.0 min
[A] = 1.469 M,t = 2.0 min
What is the initial rate of the reaction in the experiment?

Accepted Answer

The answer of For the second-order reaction A → products,the...

Question 3

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(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

According to the balanced equation, for every 2 mol of N₂O₅ that reacts, 4 mol of NO₂ is produced. Therefore, the rate of appearance of NO₂ is twice the rate of disappearance of N₂O₅. Thus, the rate of appearance of NO₂ is 2 x 1.60 mol min^-1 = 3.20 mol min^-1. Therefore, the correct answer is (C).

Question 4

For a reaction with a second order rate constant,what is the correct unit?

Accepted Answer

For a second order reaction, the rate constant has units of M^-1 time^-1 to ensure that the rate of reaction (which has units of M time^-1) is consistent with the concentration terms in the rate equation.

Question 5

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g)→ (g)+ (g) Is 0.130 mol L^-1 At 150 °C.The rate of reaction is ________ mol L^-1 .

Accepted Answer

The answer of The rate of disappearance of HBr in...

Question 6

For the reaction: A → Products concentration-time data are:

What is the order of this reaction with respect to [A]?

Accepted Answer

The answer of For the reaction: A → Products concentration-time...

Question 7

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(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?

Accepted Answer

The rate of appearance of $NO_2$ is 0.560 mol/min, and since the stoichiometry of $NO_2$ to $O_2$ in the reaction is 4:1, the rate of appearance of $O_2$ is one fourth of that of $NO_2$, which is $0.560 \, \text{mol/min} \div 4 = 0.140 \, \text{mol/min}$.

Question 8

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

Accepted Answer

According to the given rate law, the rate of the reaction is directly proportional to the concentration of A to the power of 1. Therefore, if the concentration of A is increased by a factor of 5, the rate of the reaction will also increase by the same factor (5).

Question 9

For the second-order reaction A → products,the following data are obtained:
[A] = 3.024 M,t = 0 min
[A] = 2.935 M,t = 1.0 min
[A] = 2.852 M,t = 2.0 min
What is the concentration of [A] after 4 min?

Accepted Answer

The answer of For the second-order reaction A → products,the...

Question 10

In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,at what time will [A] = 0.200 M?

Accepted Answer

For a first-order reaction, the rate constant k can be calculated using the formula k = (1/t) * ln([A]₀/[A]). Using the given concentrations and time, k is found. Then, using this k, the time for [A] to reach 0.200 M can be calculated using the same formula.

Question 11

For the second order reaction A → products,the following data are obtained:
[A] = 1.512 M,t = 0 min
[A] = 1.490 M,t = 1.0 min
[A] = 1.469 M,t = 2.0 min
What is the concentration of [A] in the experiment after 4.0 min for the reaction?

Accepted Answer

The answer of For the second order reaction A →...

Question 12

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl][N]²?

Accepted Answer

The overall reaction order is determined by adding the exponents in the rate law. Here, the exponents are 1 (for Cl) and 2 (for N), giving a total of 1 + 2 = 3, indicating a third-order reaction.

Question 13

For the reaction: 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.At what temperature is the half-life 400.seconds?

Accepted Answer

The answer of For the reaction: 2 N₂O₅(g)→ 4 NO₂(g)+...

Question 14

For the reaction: 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂.What is the half-life at 350 K?

Accepted Answer

The answer of For the reaction: 2 N₂O₅(g)→ 4 NO₂(g)+...

Question 15

For the reaction: 2 NO₂(g)→ 2 NO(g)+ O₂(g)concentration-time data are: What is the order of the reaction with respect to [NO₂]?

Accepted Answer

The answer of For the reaction: 2 NO₂(g)→ 2 NO(g)+...

Question 16

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g). If the rate of appearance of O₂ is equal to 3.00 mol min^-1 at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

Accepted Answer

The stoichiometry of the reaction shows that 2 moles of N2O5 produce 1 mole of O2. Therefore, the rate of disappearance of N2O5 is twice the rate of appearance of O2. Thus, 3.00 mol min^-1 * 2 = 6.00 mol min^-1.

Question 17

In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,what is the half-life of the reaction?

Accepted Answer

The half-life of a first-order reaction is given by $t_{1/2} = \frac{0.693}{k}$, where $k$ is the rate constant. To find $k$, we use the first-order rate law: $\ln\left(\frac{[A]_0}{[A]}\right) = kt$. Substituting the given values, $\ln\left(\frac{0.400}{0.250}\right) = k \times 15.0$, we can solve for $k$ and then calculate $t_{1/2}$. The calculation yields a half-life of approximately 22.1 minutes.

Question 18

For the second-order reaction A → products,the following data are obtained:
[A] = 3.024 M,t = 0 min
[A] = 2.935 M,t = 1.0 min
[A] = 2.852 M,t = 2.0 min
What is the initial rate of the reaction?

Accepted Answer

The answer of For the second-order reaction A → products,the...

Question 19

The first-order reaction A → Products has a half-life,t_1/2,of 55.0 min at 25 °C and 6.8 min at 100 °C.What is the activation energy for this reaction?

Accepted Answer

The answer of The first-order reaction A → Products has...

Question 20

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

Accepted Answer

Since the rate law is Rate = k[A][B], increasing the concentration of B by a factor of 3 means the rate will increase by a factor of $3^1 = 3$, and since B appears to the first power, the rate increases by a factor of 3 squared, which is 9.

Quiz 20: Chemical Kinetics

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g) → (g) + (g) Is 0.301 mol L^-1 At 150 °C.The rate of appearance of Is ________ mol L^-1 .

For the second-order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the initial rate of the reaction in the experiment?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(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?

For a reaction with a second order rate constant,what is the correct unit?

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g) → (g) + (g) Is 0.130 mol L^-1 At 150 °C.The rate of reaction is ________ mol L^-1 .

For the reaction: A → Products concentration-time data are: What is the order of this reaction with respect to [A]?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(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?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

For the second-order reaction A → products,the following data are obtained: [A] = 3.024 M,t = 0 min [A] = 2.935 M,t = 1.0 min [A] = 2.852 M,t = 2.0 min What is the concentration of [A] after 4 min?

In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,at what time will [A] = 0.200 M?

For the second order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the concentration of [A] in the experiment after 4.0 min for the reaction?

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl][N]²?

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.At what temperature is the half-life 400.seconds?

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂.What is the half-life at 350 K?

For the reaction: 2 NO₂(g) → 2 NO(g) + O₂(g) concentration-time data are: What is the order of the reaction with respect to [NO₂]?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) . If the rate of appearance of O₂ is equal to 3.00 mol min^-1 at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,what is the half-life of the reaction?

For the second-order reaction A → products,the following data are obtained: [A] = 3.024 M,t = 0 min [A] = 2.935 M,t = 1.0 min [A] = 2.852 M,t = 2.0 min What is the initial rate of the reaction?

The first-order reaction A → Products has a half-life,t_1/2,of 55.0 min at 25 °C and 6.8 min at 100 °C.What is the activation energy for this reaction?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

Quiz 20: Chemical Kinetics

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g) → (g) + (g) Is 0.301 mol L-1 At 150 °C.The rate of appearance of Is ________ mol L-1 .

For the second-order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the initial rate of the reaction in the experiment?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(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?

For a reaction with a second order rate constant,what is the correct unit?

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g) → (g) + (g) Is 0.130 mol L-1 At 150 °C.The rate of reaction is ________ mol L-1 .

For the reaction: A → Products concentration-time data are: What is the order of this reaction with respect to [A]?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(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?

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

For the second-order reaction A → products,the following data are obtained: [A] = 3.024 M,t = 0 min [A] = 2.935 M,t = 1.0 min [A] = 2.852 M,t = 2.0 min What is the concentration of [A] after 4 min?

In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,at what time will [A] = 0.200 M?

For the second order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the concentration of [A] in the experiment after 4.0 min for the reaction?

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl ][N]2?

For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is: = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol.At what temperature is the half-life 400.seconds?

For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is: = k[N2O5] At 300 K,the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2.What is the half-life at 350 K?

For the reaction: 2 NO2(g) → 2 NO(g) + O2(g) concentration-time data are: What is the order of the reaction with respect to [NO2]?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g) . If the rate of appearance of O2 is equal to 3.00 mol min-1 at a particular moment,what is the rate of disappearance of N2O5 at that moment?

In the first-order,reaction A → products,[A] = 0.400 M initially and 0.250 M after 15.0 min,what is the half-life of the reaction?

For the second-order reaction A → products,the following data are obtained: [A] = 3.024 M,t = 0 min [A] = 2.935 M,t = 1.0 min [A] = 2.852 M,t = 2.0 min What is the initial rate of the reaction?

The first-order reaction A → Products has a half-life,t1/2,of 55.0 min at 25 °C and 6.8 min at 100 °C.What is the activation energy for this reaction?

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g) → (g) + (g) Is 0.301 mol L^-1 At 150 °C.The rate of appearance of Is ________ mol L^-1 .

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(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 rate of disappearance of HBr in the gas phase reaction 2 HBr(g) → (g) + (g) Is 0.130 mol L^-1 At 150 °C.The rate of reaction is ________ mol L^-1 .

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(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?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00?

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl][N]²?

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol.At what temperature is the half-life 400.seconds?

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) the rate law is: = k[N₂O₅] At 300 K,the half-life is 2.50 × 10⁴ seconds and the activation energy is 103.3 kJ/mol O₂.What is the half-life at 350 K?

For the reaction: 2 NO₂(g) → 2 NO(g) + O₂(g) concentration-time data are: What is the order of the reaction with respect to [NO₂]?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) . If the rate of appearance of O₂ is equal to 3.00 mol min^-1 at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

The first-order reaction A → Products has a half-life,t_1/2,of 55.0 min at 25 °C and 6.8 min at 100 °C.What is the activation energy for this reaction?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?