Consider the reaction
A + B → C + D
The initial rates for different initial concentrations of the reactants are given below :
Initial concentration (mol 1– 1Initial rate (mol 1 –1 s– 1)
| A | B | ||
| (i) | 1.0 | 1.0 | 2.0 x 10 – 3 |
| (ii) | 2.0 | 1.0 | 4.0 x 10– 3 |
| (iii) | 4.0 | 1.0 | 8.0 x 10– 3 |
| (iv) | 1.0 | 2.0 | 2.0 x 10– 3 |
| (v) | 1.0 | 4.0 | 2.0 x 10’3 |
(a) What are the orders with respect to A and B ?
(b) What is the overall order ?
(c) Write the rate law equation.
(d) Calculate the rate constant.
(e) Suggest a possible mechanism.
Answer:
According to equation A+B –> C +D
The initial rates is given by [A]m[B]n
(i) Initial rate = k[1]m[1]n =2.0 x 10-3
ii) Initial rate = k[2]m[1]n = 4.0 x 10-3
iii) Initial rate = k[4]m[1]n = 8.0 x 10-3
iv) Initial rate = k[1]m[2]n = 2.0 x 10-3
v) Initial rate = k[2]m[4]n = 2.0 x 10-3
Consider the reaction
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