Chemical Kinetics (Chpt 12 Zumdahl 7th ed.)

Which of the following is the primary reason for the increase in the rate of a reaction with an increase in temperature?
1. The fraction of high energy molecular collisions increases
2. Reactant molecules collide more frequently at higher temperatures
3. The pressure exerted by the reactant molecules increases
4. The vapor pressure of the reactant molecules increases
5. The Activation Energy decreases with an increase in temperature
Which statement below is true considering the following reaction:
H2(g) + Cl2(g) ==> 2HCl(g)
1. ΔG is large and positive therefore reaction rate is very fast
2. ΔG is large and negative therefore reaction rate is very fast
3. ΔG = 0 indicating the reaction rate is not significant
4. The ΔG for this reaction is not related to reaction rate
5. The "U+0394"G for this reaction is large and positive indicating that the reaction is spontaneous
If the half-life of a decomposition reaction decreases as the amount of reactant initially present increases, which of the following terms could describe the reaction?
1. Zero Order
2. First Order
3. Second Order
4. Exothermic
5. Spontaneous
For which reaction orders is half-life always constant?
1. Zero order
2. 1st order
3. 2nd order
4. Both choices B and C
5. Choices A, B, and C
The rate constant _____________?
1. always shows an exponential increase with absolute temp (K).
2. increases with decreasing concentration.
3. usually increases with pressure (for gasses).
4. is the same for a given reaction at a specified temperature.
5. never changes irrespective of temperature (it is a constant).
Radioactive nuclear decay is a first order process. An initial sample of 80.0 g of a radioactive isotope is found to decay to 20.0 g after 12 days. When was there 40.0 g of the isotope present?
1. After 2 days
2. After 4 days
3. After 6 days
4. After 8 days
5. After 10 days
If both ΔH and Ea for the forward direction are known, the reverse reaction would have and Ea value of _____________?
1. (-ΔH + Ea)
2. (ΔH + Ea)
3. ( Ea)
4. (- Ea)
5. None of these choices describe Ea for the reverse reaction
Consider the irreversible reaction of Nitrogen Monoxide with Bromine, which is given by the following overall balanced equation:
2 NO(g) + Br2(g) ==> 2 NOBr(g)
The reaction is thought to proceed by the following two-step mechanism:
NO(g) + Br2(g) ==> NOBr(g) + Br(g) (Slow)
NO(g) + Br(g) ==> NOBr(g) (Fast)

Which substance is considered an intermediate of the reaction?
1. NO(g)
2. Br2(g)
3. NOBr(g)
4. NOBr2(g)
5. Br(g)
What is the expected rate law for the reaction shown in Question 8?
1. Rxn Rate = k [NO] [Br2]
2. Rxn Rate = k [NO]
3. Rxn Rate = k [Br2]
4. Rxn Rate = k . [NO]^2
5. Rxn Rate = k [NO]^2 [Br2]
For two 1st order reactions:
A ===> B t(1/2) = 30.0 min
W ===> X t(1/2) = 60.0 min
Which of the following statements is true
1. doubling A will have 1/2 the effect on half-life that doubling the concentration of B would have
2. a certain mass of A will react twice as fast as the same mass of W
3. a certain mass of W will react twice as fast as the same mass of A
4. the rate constant (k) is lower for A ===> B than for W ===> X
5. 4 moles of A will react more quickly than 4 moles of W

Chemical Kinetics (Chapter 14 Brown, Lemay and others 11th ed.)

Quiz