The experiment can be extended to determine the order of reaction m with respect to [OH-] by varying the concentration of hydroxide ions [OH-] Assume that the value of the pseudo-rate constant k’ was measured for two different concentrations of [OH-]. The value of k’ was found to be 0.13 at [OH-] = 0.2 M, and 0.061 when [OH-] =0.1 M. Show how you can rearrange and combine the following two equations (see equation 4) to solve for m.
0.13 = k’ = k[0.2]m and 0.061 = k’ = k[0.1]m
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I have the same question on a lab I am doing now and I have no idea how to do it either.
same
To determine the order of reaction (m) with respect to [OH-], we can rearrange and combine the given equations as follows:
Equation 1:
0.13 = k' = k[0.2]^m
Equation 2:
0.061 = k' = k[0.1]^m
To solve for m, we can set the two equations equal to each other:
k[0.2]^m = k[0.1]^m
Since the k values are the same in both equations, we can cancel them out:
[0.2]^m = [0.1]^m
Now, we can take the logarithm of both sides to simplify the equation:
log[0.2]^m = log[0.1]^m
Using the logarithmic property log(a^b) = b * log(a), the equation becomes:
m * log(0.2) = m * log(0.1)
The m term can be canceled out from both sides:
log(0.2) = log(0.1)
Finally, we can solve for m by dividing both sides by log(0.2):
m = log(0.1) / log(0.2)
Using a calculator, we can find the value of m.