In: Chemistry
With the following data, use the method of initial rates to find the reaction orders with respect to NO and O2.:
Trial | [NO]o | [O2]o | Initial reaction rate, M/s |
1 | 0.020 | 0.010 | 0.028 |
2 | 0.020 | 0.020 | 0.057 |
3 | 0.040 | 0.020 | 0.227 |
Rate = K[NO]^m[O2]^n
0.028 = K(0.02)^m *(0.01)^n ------------------------> 1
0.057 = K(0.02)^m*(0.02)^n -------------------------> 2
0.227 = K(0.04)^m*(0.02)^n -------------------------> 3
eq 1 is divide with eq 2
0.028/0.057 = K(0.02)^m *(0.01)^n/K(0.02)^m*(0.02)^n
0.5 = (0.01/0.02)^n
(0.5)^1 = (0.5)^n
n = 1
eq 2 is divide with eq 3
0.057/0.227 = K(0.02)^m*(0.02)^n/K(0.04)^m*(0.02)^n
0.25 = (0.02/0.04)^m
0.25 = (0.5)^m
(0.5)^2 = (0.5)^m
m = 2
rate law
Rate = K[NO]^2[O2]^1
order with respect NO = 2
order with respect O2 = 1