The overall order of a reaction is determined by summing the exponents of the concentration terms in the rate law.
In this case, the rate law is given as \( \text{Rate} = k[A]^2[B] \).
The exponent of \( [A] \) is 2 and the exponent of \( [B] \) is 1.
Therefore, the overall order is \( 2 + 1 = 3 \).
Reaction Rate Data
Sl. No. | [A] (mol L−1) | [B] (mol L−1) | Initial rate (mol L−1 s−1) |
---|---|---|---|
1 | 0.1 | 0.1 | 0.05 |
2 | 0.2 | 0.1 | 0.10 |
3 | 0.1 | 0.2 | 0.05 |
Sl. No. | [A] (mol L-1) | [B] (mol L-1) | Initial rate (mol L-1 s-1) |
---|---|---|---|
1 | 0.1 | 0.1 | 0.05 |
2 | 0.2 | 0.1 | 0.10 |
3 | 0.1 | 0.2 | 0.05 |