QUESTION 1

When the reactant concentration ([A]) is plotted against time for some reaction, a linear plot is observed with a slope of 0.18 M min^-1. The initial concentration of A is 0.2 M. Based on this, which of the following may be concluded?

		The reaction is first order.
		The reaction is second order.
		The reaction rate is 0.18 M min-1.
		The halflife is 0.556 min.
		The rate constant is 0.18 M min-1.

QUESTION 2

The overall reaction NO₂ + CO CO₂ + NO has a rate law of rate = k[NO₂][CO] at high temperature. Which of the following is consistent with this information?

		The overall reaction could be the mechanism. That is, NO2 + CO CO2 + NO is an elementary step.
		The rate limiting step must be bimolecular.
		A plausible mechanism is 1. NO2 + NO2 NO3 + NO (slow) 2. NO3 + CO NO2 + CO2 (fast)
		A plausible mechanism is 1. NO2 + NO2 NO3 + NO (fast equilibrium) 2. NO3 + CO NO2 + CO2 (slow)
		CO2 is a reagent in the rate limiting step.

QUESTION 3

Radon-222 is an inert gas that is produced by uranium decomposition in rock deposits. The decomposition of radon-222 is first order with k = 0.007 d^-1. How many days will it take for a dose to decrease to 1/4^th of its original amount?

QUESTION 4

A first-order reaction has k = 3.35 10^-3 s^-1. How much of the reactant is left after 1200 s if you start with 0.599 M of the reactant?

QUESTION 5

Initial rate data are collected for I + OCl OI + Cl. Based on this data, what is the numerical value of the rate constant?

I	OCl	Rate
0.20 M	0.05 M	0.619 M/s
0.20 M	0.100 M	2.476 M/S
0.300 M	0.05 M	0.619 M/s