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Chemistry / SmartWork5 Chemistry II Chapter 13

SmartWork5 Chemistry II Chapter 13

Chemistry10 CardsCreated 10 months ago

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

Nitrous oxide decomposes to nitrogen and oxygen in the following reaction:
2N2O(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:

2N2O(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

Term	Definition
Nitrous oxide decomposes to nitrogen and oxygen in the following reaction: 2N2O(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