Determine the rate law and calculate the rate constant for the chemical reaction.
Experimental data was collected for the following reaction: 2A + B → C

experiment [A] (M) [B] (M) initial rate M/s

1 0.550 0.300 7.11 × 10–4

2 0.550 0.150 3.56 × 10–4

3 0.278 0.150 3.56 × 10–4

The rate law is [B]

Explanation:

In Trials 1 and 2, the concentration of B changes and A is the same so you can see how changes in B affect the rate. In this case, 0.300/0.150=2 and 7.11 x 10^-4 / 3.56 x 10^-4= 2. Since there 2^1=2, we can say that the reaction order of B is 1.

Similarly, if we look at trials 2 and 3, the concentration of B is constant, while A is changing. In this case, the rate has not changed at all with a change in concentration of A, so this means that A has 0 order.

Therefore, the rate law is just [B].

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