Chemistry Textbook
Self-Assessments
Hydrogen iodide decomposes according to the following reaction:
2HI(g) → H2(g) + I2(g).
If hydrogen gas is formed at the rate of 1.2×10-5 M/s, what is the rate of decomposition of hydrogen iodide?
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For the oxidation of ammonia, 4NH3+3O2⟶2N2+6H2O,
the rate of disappearance of NH3 at a certain instant was found to be 0.35 mol L‑1 s‑1. What is the rate of disappearance of O2 in the same instant?
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For the oxidation of ammonia, 4NH3+3O2⟶2N2+6H2O,
the rate of disappearance of NH3at a certain instant in time was found to be 0.55 mol L‑1 s‑1. What is the rate of the reaction in the same instant?
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Consider the reaction for ammonia synthesis: N2(g) + 3H2(g) ⟶ 2NH3(g). If the rate of the reaction at a certain instant is 1.2 × 10-3 M/s, what is the rate of disappearance of hydrogen (H2)?
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An experiment shows that the reaction,
2N2O5⟶2NO2+O2,
is a first order reaction. What is the rate law of the reaction?
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Nitric oxide, released by supersonic aircrafts flown in the stratosphere, reacts with ozone and can contribute to depletion of the ozone layer.
The reaction NO+O3⟶NO2+O2is first order with respect to both NO and O3.
When [NO] = 3.3 × 10−6 M and [O3] = 5.9 × 10−7 M, the rate of the reaction was found to be 4.3 × 10-5 mol/L/s. What is the rate constant of the reaction?
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The rate law for the reaction, H2(g)+2NO(g)⟶N2O(g)+H2O(g),
has been experimentally determined to be
rate = k[NO]2[H2].
How is the rate of the reaction affected when the concentration of NO is tripled and concentration of H2 is halved?
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Determine the rate law of the reaction, A + 2B ⟶ C, using the initial rate data provided below:
[A] (M)
[B] (M)
Initial Rate (M/s)
0.015
0.010
3.4×10-5
0.030
0.030
4.1×10-4
0.015
0.020
6.8×10-5
0.14
0.010
2.9×10-3
[A] (M)
[B] (M)
Initial Rate (M/s)
0.015
0.010
3.4×10-5
0.030
0.030
4.1×10-4
0.015
0.020
6.8×10-5
0.14
0.010
2.9×10-3
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The reaction of nitrogen dioxide with carbon monoxide is
2NO2(g) + CO(g) →NO(g)+CO2(g)
The kinetics of this reaction have been studied in the laboratory, and some initial rate data below 400 K is listed in the following table:
Experiment
[NO2] (M)
[CO] (M)
Initial Rate (M/s)
1
3.4 × 10−8
3.5 × 10−7
1.6 × 10−6
2
1.1 × 10−8
1.5 × 10−7
1.7 × 10−7
3
1.1 × 10−8
2.5 × 10−7
1.7 × 10−7
4
5.5 × 10−8
1.5 × 10−7
4.3 × 10−6
What is the rate law of the reaction?
Experiment
[NO2] (M)
[CO] (M)
Initial Rate (M/s)
1
3.4 × 10−8
3.5 × 10−7
1.6 × 10−6
2
1.1 × 10−8
1.5 × 10−7
1.7 × 10−7
3
1.1 × 10−8
2.5 × 10−7
1.7 × 10−7
4
5.5 × 10−8
1.5 × 10−7
4.3 × 10−6
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The decomposition of Sulfuryl chloride (SO2Cl2) to SO2and Cl2 according to the following reaction was determined to follow first order kinetics:
SO2Cl2(g) → SO2(g) + Cl2(g).
The rate constant of the reaction was determined to be 2.2 × 10-5 s-1. If the reaction started with 0.030 M SO2Cl2, what is the concentration of SO2Cl2 after 5 hours?
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The decomposition of Sulfuryl chloride (SO2Cl2) to SO2and Cl2 according to the following reaction was determined to follow first order kinetics:
SO2Cl2(g) → SO2(g) + Cl2(g).
The rate constant of the reaction was determined to be 2.2 × 10-5 s-1. If the reaction started with 0.030 M SO2Cl2, how much time does it take for the concentration to decrease to 0.028 M?
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The reaction of t-butyl chloride with water is first ordered with respect to t-butyl chloride. The rate constant of the reaction was determined to be 15 × 10−4s−1 at 25°C. How much time does it take for 15% of SO2Cl2 to decompose?
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The decomposition of nitrous oxide (N2O) over hot platinum surface is a zero-order reaction:
2N2O(g) → 2N2(g) + O2(g).
The rate constant of the reaction is 1.2 × 10-3 M/s at 565 o How much time does it take for the reactant concentration to decrease from 0.100 M to 0.072 M?
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The second order reaction, A → products, yields a linear plot when ______ is plotted on the X-axis and ____ is plotted on the Y-axis.
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For the reaction 2A → B, the following plot was obtained. What is the rate law of the reaction?
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How is the rate constant determined from the linear plot yield by the zero-order reaction, A → Products?
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Determine the rate constant from the following plot yielded for the first order reaction, X → Y
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In a first order reaction, if the concentration of the reactant dropped from 650 mM to 230 mM in 25 seconds, what is the half-life of the reaction?
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Radioactive decay follows first order kinetics.
Since plants stop absorbing carbon-14 when begin to decay, the amount of carbon-14 left behind is used to reveal the age of the tree. The half-life of carbon-14 isotope is 5730 years. If 65% of carbon-14 is still left in an ancient piece of wood, how long ago was the tree dead?
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Holmium-166 isotope is a short-lived medical isotope that was developed in the recent years for diagnosis and treatment of liver tumors.
The half-life of Holmium-99 is 26.8 hours. What fraction of the isotope will be left after 42 hours?
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In a first order reaction, X → Y, it takes 50 min for concentration of X to decrease to half of its initial concentration. If the initial concentration of X is 0.70 M, how much time does it take for its concentration to decrease to 4.38 × 10-2 M?
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