Consider the following reaction; A + B → C
| Experiment | Initial [A] | Initial [B] | Rate of formation of C (m/s) |
| 1 | 0.10 M | 1.0 M | 2.1 x 10-3 |
| 2 | 0.20 M | 1.0 M | 8.4 x 10-3 |
| 3 | 0.20 M | 2.0 M | 8.4 x 10-3 |
What is the order of reaction with respect to A and B?
Answer & explanation
Correct answer: option 1
r = k[A]x[B]y
2.1 x 10-3 = k[0.1]x[1]y ......(i)
8.4 x 10-3 = k[0.2]x[1]y ......(ii)
8.4 x 10-3 = k[0.2]x[2]y ......(iii)
Dividing equation (ii) by (i)
\(\frac{8.4 × 10^{-3}}{2.1 × 10^{-3}}\) = \(\frac{k[0.2]^x[1]^y}{k[0.1]^x[1]^y}\)
4 = 2x
22 = 2x
x = 2
Dividing equation (iii) by (ii)
\(\frac{8.4 × 10^{-3}}{8.4 × 10^{-3}}\) = \(\frac{k[0.2]^x[2]^y}{k[0.2]^x[1]^y}\)
1 = 2y
20 = 2y
y = 0
r = k[A]2[B]0