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SmartWork5 Chemistry II Chapter 13

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This deck covers key questions and answers related to chemical reactions and rate laws, based on Chapter 13 of SmartWork5 Chemistry II.

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Nitrous oxide decomposes to nitrogen and oxygen in the following reaction:

2N2​O(g) -----> 2N2​(g) + O2​(g)

Using this concentration versus time plot, answer the following questions.

Part 1: The green curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

Part 2: The blue curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

Part 1: N2O

Part 2: N2

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Key Terms

Term
Definition

Nitrous oxide decomposes to nitrogen and oxygen in the following reaction:

2N2​O(g) -----> 2N2​(g) + O2​(g)

Using this concentration versus time plot, answer the following questions.

Part 1: The green curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

Part 2: The blue curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

Part 1: N2O

Part 2: N2

Dinitrogen pentoxide (N2O5) decomposes as follows to nitrogen dioxide and nitrogen trioxide:

N2O5(g) -----> NO2(g) + NO3(g)

Calculate the average rate of the reaction between consecutive measurement times in the following table.

Part 1: Express every answer to two significant figures.

Rate 1:

Part 2:

Rate 2=

Part 3:

Rate 3=

Part 4:

Rate 4=

Part 1:
Rate 1= 4.9 x 10^10 molecules/(cm^3 x s)
Part 2:
Rate 2= 3.1 x 10^10 molecules/(cm^3 x s)
Part 3:
Rate 3= 2.0 x 10^10 molecu...

Hydrogen gas reduces NO to N2 in the following reaction:
2H2(g) + 2NO(g) <------> 2H2O(g) + N2(g)
The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results:
Experiment / [H2]0 (M) / [NO]0 (M) / Initial Rate (M/s)
1 / .212 / .136 / .0389
2 / .212 / .272 / .0781
3 / .424 / .544 / .618
4 / .848 / .544 / 2.48
Part 1: Choose the correct rate law for the reaction at 1500°C.
Part 2: Determine the rate constant for the reaction at 1500°C.

Part 1: A. Rate= k[H2]^2[NO]
Part 2: 6.36 M^-xs^-1

Given a reaction between an organic molecule, denoted as A, and NaSH, we observe the following observations. Using the observations, write a rate law for the reaction.
(a) The rate triples when the concentration of [A] is tripled and the concentration of [NaSH] is held constant.
(b) The rate is decreased when the concentration of [A] is doubled and the concentration of [NaSH] is cut by a factor of 3.
(c) The rate doubles when the concentration of [A] is cut in half and the concentration of [NaSH] is quadrupled.
(d) The rate increases with an increase in temperature.
Write the rate law.

Rate = k[A][NaSH]

Atmospheric chemistry involves highly reactive, odd-electron molecules such as the hydroperoxyl radical HO2, which decomposes into H2O2 and O2. The following data was obtained at 298 K.
Part 1: Determine the rate law for the reaction. Do not add multiplication symbols to your answer.
Part 2: Determine the value of the rate constant at 298 K.

Part 1: Rate = k[HO2]
Part 2: 0.854 us^-1

The reaction 2A → A2​​​​​ was experimentally determined to be second order with a rate constant, k, equal to 0.0265 M-1min-1. If the initial concentration of A was 3.25 M, what was the concentration of A (in M) after 180.0 min?

.197 M

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SmartWork5 Chemistry II Chapter 13
TermDefinition

Nitrous oxide decomposes to nitrogen and oxygen in the following reaction:

2N2​O(g) -----> 2N2​(g) + O2​(g)

Using this concentration versus time plot, answer the following questions.

Part 1: The green curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

Part 2: The blue curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

Part 1: N2O

Part 2: N2

Dinitrogen pentoxide (N2O5) decomposes as follows to nitrogen dioxide and nitrogen trioxide:

N2O5(g) -----> NO2(g) + NO3(g)

Calculate the average rate of the reaction between consecutive measurement times in the following table.

Part 1: Express every answer to two significant figures.

Rate 1:

Part 2:

Rate 2=

Part 3:

Rate 3=

Part 4:

Rate 4=

Part 1:
Rate 1= 4.9 x 10^10 molecules/(cm^3 x s)
Part 2:
Rate 2= 3.1 x 10^10 molecules/(cm^3 x s)
Part 3:
Rate 3= 2.0 x 10^10 molecules/(cm^3 x s)
Part 4:
Rate 4= 1.0 x 10^10 molecules/(cm^3 x s)

Hydrogen gas reduces NO to N2 in the following reaction:
2H2(g) + 2NO(g) <------> 2H2O(g) + N2(g)
The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results:
Experiment / [H2]0 (M) / [NO]0 (M) / Initial Rate (M/s)
1 / .212 / .136 / .0389
2 / .212 / .272 / .0781
3 / .424 / .544 / .618
4 / .848 / .544 / 2.48
Part 1: Choose the correct rate law for the reaction at 1500°C.
Part 2: Determine the rate constant for the reaction at 1500°C.

Part 1: A. Rate= k[H2]^2[NO]
Part 2: 6.36 M^-xs^-1

Given a reaction between an organic molecule, denoted as A, and NaSH, we observe the following observations. Using the observations, write a rate law for the reaction.
(a) The rate triples when the concentration of [A] is tripled and the concentration of [NaSH] is held constant.
(b) The rate is decreased when the concentration of [A] is doubled and the concentration of [NaSH] is cut by a factor of 3.
(c) The rate doubles when the concentration of [A] is cut in half and the concentration of [NaSH] is quadrupled.
(d) The rate increases with an increase in temperature.
Write the rate law.

Rate = k[A][NaSH]

Atmospheric chemistry involves highly reactive, odd-electron molecules such as the hydroperoxyl radical HO2, which decomposes into H2O2 and O2. The following data was obtained at 298 K.
Part 1: Determine the rate law for the reaction. Do not add multiplication symbols to your answer.
Part 2: Determine the value of the rate constant at 298 K.

Part 1: Rate = k[HO2]
Part 2: 0.854 us^-1

The reaction 2A → A2​​​​​ was experimentally determined to be second order with a rate constant, k, equal to 0.0265 M-1min-1. If the initial concentration of A was 3.25 M, what was the concentration of A (in M) after 180.0 min?

.197 M

The dimerization of ClO is second order in ClO.
2CIO(g) <------> CI2O2
Part 1: Use the following data to determine the value of k at 350 K.
Part 2: Use the data above to determine the value the half-life at 350 K.

Part 1: 6.75 x 10^-6 cm^3/molecules x s
Part 2: 0.712 s