Rate Constant Problem: Find n & Rate Constant

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To determine the rate constant (k) and the reaction order (n) from the given equation k' = k[OH-]^n, the first step is to log both sides, resulting in log k' = log k + n log([OH-]). This can be rearranged to the linear form log k' = n log([OH-]) + log k, where the slope (m) represents n. By analyzing the slope, n is found to be 1.04. Once n is established, k can be calculated using the values of k' and [OH-].
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Question in the link. How do I go from here and get the rate constant and n values?
 
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Equation: k' = k[OH- ]^n

k' and [OH-] measured / calculated

Log both sides of the equation above

log k' = log (k[OH- ]^n )
log k' = log k + n log([OH- ]

which is the same as

log k' = n log([OH- ] + log k
Which you can look at as y = mx + b

m = n, therefore slope = n, n = 1.04
calculate k after that
 

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