c) The overall rate law can be posed as: −d[RCOOR′]dt=k[RCOOR′]n[OH−]m What is the overall rate constant, k, for the reaction? (include appropriate units) k =
Hello i have the answers for part a and b but i dont know how to find part c (overall rate constant)
a) Consider the base hydrolysis of an ester.
RCOOR' + OH− → RCOO− + R'OH (where R and R' represent organic groups).
The kinetics of this reaction, for a particular ester, were studied using the isolation method.
When [OH−] >> [RCOOR'] a pseudo-rate law can be posed:
−d[RCOOR′]dt=k′[RCOOR′]n
With initial concentrations:
[OH−]0 = 0.900 M
[RCOOR']0 = 0.0010 M,
a plot of ln[RCOOR'] versus t gave a straight line with slope = -71.5 s-1 and y-intercept = -6.91.
order n = 1 and k' = 71.5 /s
b) When [OH−] << [RCOOR'] a pseudo-rate law can be posed:
−d[OH−]dt=k′′[OH−]m
With initial concentrations:
[OH−]0 = 0.0015 M
[RCOOR']0 = 0.600 M
a plot of ln[OH-] versus t gave a straight line with slope = -47.7 s-1 and y-intercept = -6.50.
order m = 1 and k'' = 47.7 /s
c) The overall rate law can be posed as:
−d[RCOOR′]dt=k[RCOOR′]n[OH−]m
What is the overall rate constant, k, for the reaction? (include appropriate units)
k =
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