Kinetics 1
1 For the hypothetical reaction A+B=> products, the rate law is first order in A and first order in B. When the initial concentrations of A and B are .05 M and .08 M respectively, the initial rate is 1.6x10-3 M/s.
a) What is the form of the rate equation? b) What is the value and units of the rate constant? c) If the initial concentration of A were tripled what would happen to the rate? d) If the initial concentration of A and B were both tripled what would happen to the rate? e) If the initial concentration of A and B were both tripled what would happen to the rate constant? f) What would the initial rate be if the initial concentrations of A and B are .035 M and .098 M? respectively
2. a) At 215 C the rate of decomposition of CH3CN is first order with a rate constant of 2x10 -4 sec -1 . What is the half life of CH3CN at this temperature? (Answer = 3.5x10 3 sec) b) How much time would it take for 16 g of CH3CN to decompose so that only 1 gram remains? (Answer= 3.9 hours)
3.The following data are collected for the gas phase reaction:
NO + 1/2 Br2 = NOBr
| Experiment | [NO] M | [Br2] M | Initial rate M/sec |
| 1 | 0.1 | 0.1 | 12 |
| 2 | 0.1 | 0.2 | 24 |
| 3 | 0.3 | 0.1 | 108 |
a) What is the rate law and explain how you know.b) Calculate the value of the rate constant. (including units)c) What would be the initial rate if the concentration of NO is 0.4 and of bromine is 0.5?
4. The rate constant of a reaction is 1.45x10-4 s-1. What is the half life and what is the lifetime of this reaction.