Question

1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units of k for this reaction? If the concentration of air decreases by a factor of 2 and the concentration of b increases by a factor of 5 what happens to the rate?

2. for the forward reaction 2NO+Cl2=>2NOCl. determine the rate(m/s)for experiment #4 given [NO]°(M)=0.40M and [Cl2]°z(M)=0?20M. Rate?

3.The following data were collected over time for the forward reaction 2NO2=>2NO+O2 ( 1/[NO2]=100 at 0 seconds, 125 @50seconds, 150@100sec, 220@200secs,270@300secs. what is the order of reaction? what is the initial concentration of NO2? calculate the rate constant for the reaction with units.

4.Molecular iodine dissociates into iodine atoms at 625K: I2=>2I. with a rate constant of 0.271 s-1.if you start with 5.0*10^-2M I2 at 625K, what concentration of I2 will remain after 0.128, min assuming that the iodine atoms do not combine to form I2?
5. if the vessel is exactly 1.00L, how many grams of iodine atoms are created in this time?

6. derive an expression for the 1/4 life of a zeroth order reaction( that is time it takes for 1/4 of reactant to react)
7. the reaction: SO2Cl2 =>SO2 + Cl2 is first order in SO2Cl2. The rate constant for the reaction at 660k is 4.5E-2s-1. if we begin with an initial SOCl2 pressure of 450 torr, what is the pressure after 60 s? at what time will the pressure of SO2Cl2 decline to 1/10 of it's initial value?
8.The reaction A=>B is 1st order in [A]. consider the following data. time(s)0.0= 1.60[A](M),10.0s= 0.40M, 20s= 0.10M. what is the rate constant for this reaction? what is the half life of this reaction?