 Chemistry Practice Questions VIII with Answers

1) A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]0, what is the new rate if the concentration of [A] is increased to 0.200 M?

• A) 0.0200 M/s
• B) 0.0400 M/s
• C) 0.0600 M/s
• D) 0.0800 M/s
• E) 0.100 M/s

2) A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]1, what is the new rate if the concentration of [A] is increased to 0.200 M?

• A) 0.0200 M/s
• B) 0.0400 M/s
• C) 0.0600 M/s
• D) 0.0800 M/s
• E) 0.100 M/s

3) A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]2, what is the new rate if the concentration of [A] is increased to 0.200 M?

• A) 0.0200 M/s
• B) 0.0400 M/s
• C) 0.0600 M/s
• D) 0.0800 M/s
• E) 0.100 M/s

4) Identify the methods used to monitor a reaction as it occurs in the reaction flask.

• A) polarimeter
• B) spectrometer
• C) pressure measurement
• D) none of the above
• E) all of the above

5) Write a balanced reaction for which the following rate relationships are true. 6) Write a balanced reaction for which the following rate relationships are true. 7) What is the overall order of the following reaction, given the rate law?

NO(g) + O3(g) → NO2(g) + O2(g)      Rate = k[NO][O3]

• A) 1st order
• B) 2nd order
• C) 3rd order
• D) 1 order
• E) 0th order

8) What data should be plotted to show that experimental concentration data fits a first-order reaction?

• A) 1/[reactant] vs. time
• B) [reactant] vs. time
• C) ln[reactant] vs. time
• D) ln(k) vs. 1/T
• E) ln(k) vs. Ea

9) What data should be plotted to show that experimental concentration data fits a second-order reaction?

• A) ln[reactant] vs. time
• B) [reactant] vs. time
• C) ln(k) vs. 1/T
• D) 1/[reactant] vs. time
• E) ln(k) vs. Ea

10) What data should be plotted to show that experimental concentration data fits a zeroth-order reaction?

• A) ln[reactant] vs. time
• B) 1/[reactant] vs. time
• C) ln(k) vs. 1/T
• D) ln(k) vs. Ea
• E) [reactant] vs. time

11) Which of the following statements is FALSE?

• A) The average rate of a reaction decreases during a reaction.
• B) It is not possible to determine the rate of a reaction from its balanced equation.
• C) The rate of zero-order reactions is not dependent on concentration.
• D) The half-life of a first-order reaction is dependent on the initial concentration of reactant.
• E) None of the statements is FALSE.

12) Carbon-14 has a half-life of 5720 years and this is a first-order reaction. If a piece of wood has converted 75% of the carbon-14, then how old is it?

• A) 11440 years
• B) 2375 years
• C) 4750 years
• D) 4290 years
• E) 1430 years

13) Carbon-14 has a half-life of 5720 years and this is a first-order reaction. If a piece of wood has converted 25% of the carbon-14, then how old is it?

• A) 11440 years
• B) 2375 years
• C) 4750 years
• D) 4290 years
• E) 1430 years

14) The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life of the decomposition?

• A) 0.491 s
• B) 0.204 s
• C) 0.236 s
• D) 0.424 s
• E) 0.294 s

15) The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M. What is the rate constant for this reaction?

• A) 1.0 × 10-2 M-1s-1
• B) 4.5 × 10-2 M-1s-1
• C) 9.7 × 10-2 M-1s-1
• D) 2.2 × 10-2 M-1s-1
• E) 3.8 × 10-2 M-1s-1

16) The half-life for the decay of radium is 1620 years. What is the rate constant for this first-order process?

• A) 4.28 × 10-4 yr-1
• B) 1.12 × 10-4 yr-1
• C) 2.33 × 10-4 yr-1
• D) 8.91 × 10-4 yr-1
• E) 6.17 × 10-4 yr-1

17) The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1. If the initial concentration of cyclopropane is 1.33 M, what is the concentration of cyclopropane after 644 s?

• A) 0.43 M
• B) 0.15 M
• C) 0.94 M
• D) 0.86 M
• E) 0.67 M

18) The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 M, what is the concentration of N2O after 9.6 s?

• A) 7.4 × 10-3 M
• B) 1.0 × 10-3 M
• C) 1.4 × 10-3 M
• D) 3.6 × 10-3 M
• E) 8.7 × 10-3 M

19) The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1. How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

• A) 4.55 M
• B) 0.258 M
• C) 3.87 M
• D) 2.20 M
• E) 2.39 M

20) The first-order decay of radon has a half-life of 3.823 days. How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

• A) 4.21 g
• B) 183 g
• C) 54.8 g
• D) 76.3 g
• E) 67.5 g Can’t find the questions that you need?