Explanation:
[C5H5N](M) [CH3I](M) Rate(M/s)
1.00 X 10-4 1.00 X 10-4 7.5 X 10-7
2.00 X 10-4 2.00 X 10-4 3.0 X 10-6
2.00 X 10-4 4.00 X 10-4 6.1 X 10-6
Doubling the concentration of CH3I causes the rate to increase by a factor of 2. The reaction is first order with respect to CH3I.
Doubling both concentrations increases the rate of reaction by a factor of 4. In addition with the order of CH3I, we can conclude that the reaction is also first order with respect to C5H5N.
Rate Law;
Rate = k [C5H5N] [CH3I]
Rate constant;
Picking experiment 1;
Rate = k [C5H5N] [CH3I]
7.5 X 10-7 = 1.00 X 10-4 * 1.00 X 10-4 * k
k = 7.5 X 10-7 / 1.00 x 10-8
k = 7.5 x 10^1 = 75
Predict the initial rate for initial concentrations of [C5H5N] = 1.5 X 10-4 M and [CH3I] = 6.1 X 10-5 M
Rate = k [C5H5N] [CH3I]
Rate = 75 * 1.5 X 10-4 * 6.1 X 10-5
Rate = 686.25 x 10-9
Rate = 6.8625 x 10-7M/s
