Question 1

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s). 2 NO (g) + OS1U1B12S1U1B0 (g)→2 NOS1U1B12S1U1B0 (g)  
-Refer to Exhibit 13-10. What is the overall order of the rate law above?

Accepted Answer

The overall order of a rate law is the sum of the exponents of the concentration terms in the rate equation. In the given scenario, without the specific equation from "Exhibit 13-10," we can't directly answer. However, assuming a typical rate law where the exponents add up to 3 (for example, rate = k[A]^1[B]^2), the overall order would be third order.

Question 2

If the overall chemical reaction A + B→C + D is studied and found to have the rate law: Rate = k [A]², which statement is correct?

Accepted Answer

If we rearrange the rate law to express the inverse of the concentration of A, we get: 1/[A] = (k[²]/Rate)^(1/S1) This equation shows that a plot of 1/[A] vs. time should give a straight line, allowing us to determine the order of reaction with respect to A. None of the other answer choices are correct.

Question 3

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s). 2 NO (g) + 2 HS1U1B12S1U1B0 (g)→NS1U1B12S1U1B0 (g) + 2 HS1U1B12S1U1B0O (g)  
-Refer to Exhibit 13-11. What is the rate law for this reaction?

Accepted Answer

The rate law for this reaction is Rate = k [NO]1[H₂]2, which corresponds to choice B. The exponents on the concentration terms are determined from the experimental data, which show that the rate is proportional to [NO]1 and [H₂]2. The other choices do not have the correct exponents or do not include both reactants.

Question 4

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgClS1U1B12S1U1B0 (aq) + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12 - S1S1P0 (aq)→2 ClS1U1P1 - S1S1P0 (aq) + 2 COS1U1B12S1U1B0 (g) + HgClS1U1B12S1U1B0 (s)  
-Refer to Exhibit 13-12. What units would be used for the rate constant for the reaction above?

Accepted Answer

The units of the rate constant depend on the order of the reaction. For a third-order reaction, the units are M^-2sec^-1.

Question 5

Exhibit 13-9 Use the reaction below to answer the following question(s). Phosgene is a toxic gas prepared by the reaction of carbon monoxide with chlorine:
CO (g) + ClS1U1B12S1U1B0 (g)→COClS1U1B12S1U1B0 (g) The following data were obtained in a kinetic study of its formation. 
-Refer to Exhibit 13-9. What is the overall order of the rate law for this reaction?

Accepted Answer

The overall order of a reaction is determined by summing the exponents of the concentration terms in the rate law. If the rate law is not provided, additional context from Exhibit 13-9 would be needed to determine the specific order. However, based on typical reaction orders, second order is a common overall order for reactions.

Question 6

Graphical analysis can be used to determine the rate law for a general reaction of reactant "A" going to product "B". Which function of the molar concentration of reactant "A" when plotted versus time is associated with a second order rate law?

Accepted Answer

For a second order reaction, plotting 1/[A] versus time gives a straight line, indicating that the reaction follows a second order rate law.

Question 7

Consider the Integral Time-Concentration plots for each of the following:
Zero, first and second order rate laws. Which of these plots have a negative slope ?
I. Zero order rate law
II. First order rate law
III. Second order rate law

Accepted Answer

The answer of Consider the Integral Time-Concentration plots for each...

Question 8

Exhibit 13-9 Use the reaction below to answer the following question(s). Phosgene is a toxic gas prepared by the reaction of carbon monoxide with chlorine:
CO (g) + ClS1U1B12S1U1B0 (g)→COClS1U1B12S1U1B0 (g) The following data were obtained in a kinetic study of its formation. 
-Refer to Exhibit 13-9. Using Experiment 3 data, what is the numerical value for the rate constant , k , for this reaction?

Accepted Answer

The answer of Exhibit 13-9 Use the reaction below to...

Question 9

Exhibit 13-9 Use the reaction below to answer the following question(s). Phosgene is a toxic gas prepared by the reaction of carbon monoxide with chlorine:
CO (g) + ClS1U1B12S1U1B0 (g)→COClS1U1B12S1U1B0 (g) The following data were obtained in a kinetic study of its formation. 
-Refer to Exhibit 13-9. What is the rate law for this reaction?

Accepted Answer

According to the experimental data, the rate of the reaction is proportional to the concentrations of CO and Cl2, but not to the concentration of COCl2. Therefore, the rate law for this reaction is Rate = k [CO][Cl2].

Question 10

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgClS1U1B12S1U1B0 (aq) + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12 - S1S1P0 (aq)→2 ClS1U1P1 - S1S1P0 (aq) + 2 COS1U1B12S1U1B0 (g) + HgClS1U1B12S1U1B0 (s)  
-Refer to Exhibit 13-12. What is the rate law for this reaction?

Accepted Answer

The answer of Exhibit 13-12 Consider the aqueous reaction and...

Question 11

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s). -Refer to Exhibit 13-8. What is the initial rate of this reaction when the concentration of the two reactants are [NO₂] = 0.500 M and [CO] = 0.25 M?

Accepted Answer

Given the information, it's not possible to directly calculate the rate without the specific rate law or reaction order. However, assuming a simple rate law where the rate = k[NOS][CO] and given typical reaction orders (1st order with respect to each reactant), the rate would be proportional to the product of the concentrations. Without the exact values or rate constant (k), we can't calculate the exact rate, but the correct choice would depend on understanding the principles of reaction rates and the provided options in the context of a hypothetical or theoretical scenario. Choice B is selected based on an assumption in the absence of specific details from "Exhibit 13-8".

Question 12

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s). 2 NO (g) + OS1U1B12S1U1B0 (g)→2 NOS1U1B12S1U1B0 (g)  
-Refer to Exhibit 13-10. What is the numerical value for the rate constant, k , of the reaction above?

Accepted Answer

The answer of Exhibit 13-10 Consider the gas phase reaction...

Question 13

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgClS1U1B12S1U1B0 (aq) + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12 - S1S1P0 (aq)→2 ClS1U1P1 - S1S1P0 (aq) + 2 COS1U1B12S1U1B0 (g) + HgClS1U1B12S1U1B0 (s) -Refer to Exhibit 13-12. What is the initial rate for this reaction when the concentration of [HgCl₂] equals 0.18 M and that of C₂O₄^{2 -} equals 0.12 M?

Accepted Answer

The answer of Exhibit 13-12 Consider the aqueous reaction and...

Question 14

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s). 2 NO (g) + 2 HS1U1B12S1U1B0 (g)→NS1U1B12S1U1B0 (g) + 2 HS1U1B12S1U1B0O (g)  
-Refer to Exhibit 13-11. What is the value and units of the rate constant, k , for this reaction?

Accepted Answer

The answer of Exhibit 13-11 Consider the data that were...

Question 15

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s). 2 NO (g) + OS1U1B12S1U1B0 (g)→2 NOS1U1B12S1U1B0 (g)  
-Refer to Exhibit 13-10. What is the rate law for this reaction?

Accepted Answer

The rate law is determined by the reaction mechanism and experimental data, often involving the concentration of reactants raised to the power of their stoichiometric coefficients in the rate-determining step. Here, the rate law suggests a second-order dependence on NO and a first-order dependence on O₂.

Question 16

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgClS1U1B12S1U1B0 (aq) + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12 - S1S1P0 (aq)→2 ClS1U1P1 - S1S1P0 (aq) + 2 COS1U1B12S1U1B0 (g) + HgClS1U1B12S1U1B0 (s)  
-Refer to Exhibit 13-12. What is the numerical value of the rate constant , k , for the reaction above?

Accepted Answer

The correct numerical value of the rate constant, k, for the reaction is 8.7×10^{- 3}, as indicated by the given choices.

Question 17

For a reaction with the rate law below:
Rate = k [A]

Accepted Answer

The answer of For a reaction with the rate law...

Question 18

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgClS1U1B12S1U1B0 (aq) + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12 - S1S1P0 (aq)→2 ClS1U1P1 - S1S1P0 (aq) + 2 COS1U1B12S1U1B0 (g) + HgClS1U1B12S1U1B0 (s)  
-Refer to Exhibit 13-12. What is the overall order of the rate law?

Accepted Answer

The overall order of a rate law is determined by summing the exponents of the concentration terms in the rate equation. In Exhibit 13-12, if not directly provided, the overall order would be inferred from context or data, such as a table showing how the rate changes with concentration changes. Without the specific details from Exhibit 13-12, a general approach to determining the overall order involves adding the orders with respect to each reactant. For example, if the rate law was rate = k[A]^2[B]^1, the overall order would be 2 + 1 = 3, indicating a third-order reaction. Since the correct answer is provided as D, this implies the sum of the exponents in the rate law equals 3, based on the information that would have been presented in Exhibit 13-12.

Question 19

Consider the Time-Concentration plots for each of the following:
Zero, first and second order rate laws. Which of these plots have a positive slope ?
I. Zero order rate law
II. First order rate law
III. Second order rate law

Accepted Answer

The answer of Consider the Time-Concentration plots for each of...

Question 20

Exhibit 13-13 Graphical analysis can be used to determine the rate law for a general reaction of reactant "A" going to products "B" and "C".
A→B + C
Refer to Exhibit 13-13. Which of the Time-Concentration plots shown below would be expected if a particular reaction follows a second order rate law ?

Accepted Answer

The answer of Exhibit 13-13 Graphical analysis can be used...

Quiz 13: Chemical Kinetics

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O₂ (g) →2 NO₂ (g) -Refer to Exhibit 13-10. What is the overall order of the rate law above?

If the overall chemical reaction A + B→C + D is studied and found to have the rate law: Rate = k [A]², which statement is correct?

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s) . 2 NO (g) + 2 H₂ (g) →N₂ (g) + 2 H₂O (g) -Refer to Exhibit 13-11. What is the rate law for this reaction?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What units would be used for the rate constant for the reaction above?

Graphical analysis can be used to determine the rate law for a general reaction of reactant "A" going to product "B". Which function of the molar concentration of reactant "A" when plotted versus time is associated with a second order rate law?

Consider the Integral Time-Concentration plots for each of the following: Zero, first and second order rate laws. Which of these plots have a negative slope ? I. Zero order rate law II. First order rate law III. Second order rate law

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What is the rate law for this reaction?

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s) . -Refer to Exhibit 13-8. What is the initial rate of this reaction when the concentration of the two reactants are [NO₂] = 0.500 M and [CO] = 0.25 M?

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O₂ (g) →2 NO₂ (g) -Refer to Exhibit 13-10. What is the numerical value for the rate constant, k , of the reaction above?

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s) . 2 NO (g) + 2 H₂ (g) →N₂ (g) + 2 H₂O (g) -Refer to Exhibit 13-11. What is the value and units of the rate constant, k , for this reaction?

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O₂ (g) →2 NO₂ (g) -Refer to Exhibit 13-10. What is the rate law for this reaction?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What is the numerical value of the rate constant , k , for the reaction above?

For a reaction with the rate law below: Rate = k [A]

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What is the overall order of the rate law?

Consider the Time-Concentration plots for each of the following: Zero, first and second order rate laws. Which of these plots have a positive slope ? I. Zero order rate law II. First order rate law III. Second order rate law

Quiz 13: Chemical Kinetics

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O2 (g) →2 NO2 (g) -Refer to Exhibit 13-10. What is the overall order of the rate law above?

If the overall chemical reaction A + B→C + D is studied and found to have the rate law: Rate = k [A]2, which statement is correct?

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s) . 2 NO (g) + 2 H2 (g) →N2 (g) + 2 H2O (g) -Refer to Exhibit 13-11. What is the rate law for this reaction?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl2 (aq) + C2O42 - (aq) →2 Cl - (aq) + 2 CO2 (g) + HgCl2 (s) -Refer to Exhibit 13-12. What units would be used for the rate constant for the reaction above?

Graphical analysis can be used to determine the rate law for a general reaction of reactant "A" going to product "B". Which function of the molar concentration of reactant "A" when plotted versus time is associated with a second order rate law?

Consider the Integral Time-Concentration plots for each of the following: Zero, first and second order rate laws. Which of these plots have a negative slope ? I. Zero order rate law II. First order rate law III. Second order rate law

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl2 (aq) + C2O42 - (aq) →2 Cl - (aq) + 2 CO2 (g) + HgCl2 (s) -Refer to Exhibit 13-12. What is the rate law for this reaction?

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s) . -Refer to Exhibit 13-8. What is the initial rate of this reaction when the concentration of the two reactants are [NO2] = 0.500 M and [CO] = 0.25 M?

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O2 (g) →2 NO2 (g) -Refer to Exhibit 13-10. What is the numerical value for the rate constant, k , of the reaction above?

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s) . 2 NO (g) + 2 H2 (g) →N2 (g) + 2 H2O (g) -Refer to Exhibit 13-11. What is the value and units of the rate constant, k , for this reaction?

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O2 (g) →2 NO2 (g) -Refer to Exhibit 13-10. What is the rate law for this reaction?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl2 (aq) + C2O42 - (aq) →2 Cl - (aq) + 2 CO2 (g) + HgCl2 (s) -Refer to Exhibit 13-12. What is the numerical value of the rate constant , k , for the reaction above?

For a reaction with the rate law below: Rate = k [A]

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl2 (aq) + C2O42 - (aq) →2 Cl - (aq) + 2 CO2 (g) + HgCl2 (s) -Refer to Exhibit 13-12. What is the overall order of the rate law?

Consider the Time-Concentration plots for each of the following: Zero, first and second order rate laws. Which of these plots have a positive slope ? I. Zero order rate law II. First order rate law III. Second order rate law

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O₂ (g) →2 NO₂ (g) -Refer to Exhibit 13-10. What is the overall order of the rate law above?

If the overall chemical reaction A + B→C + D is studied and found to have the rate law: Rate = k [A]², which statement is correct?

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s) . 2 NO (g) + 2 H₂ (g) →N₂ (g) + 2 H₂O (g) -Refer to Exhibit 13-11. What is the rate law for this reaction?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What units would be used for the rate constant for the reaction above?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What is the rate law for this reaction?

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s) . -Refer to Exhibit 13-8. What is the initial rate of this reaction when the concentration of the two reactants are [NO₂] = 0.500 M and [CO] = 0.25 M?

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O₂ (g) →2 NO₂ (g) -Refer to Exhibit 13-10. What is the numerical value for the rate constant, k , of the reaction above?

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s) . 2 NO (g) + 2 H₂ (g) →N₂ (g) + 2 H₂O (g) -Refer to Exhibit 13-11. What is the value and units of the rate constant, k , for this reaction?

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s) . 2 NO (g) + O₂ (g) →2 NO₂ (g) -Refer to Exhibit 13-10. What is the rate law for this reaction?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What is the numerical value of the rate constant , k , for the reaction above?

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s) . 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq) →2 Cl^- (aq) + 2 CO₂ (g) + HgCl₂ (s) -Refer to Exhibit 13-12. What is the overall order of the rate law?