This was collected in a kinetics experiment for the disproportion of A2 in a buffered solution:
3 A2 --> products
The generic rate law for the reaction is rate = k[A2]^p
[A2]0 : 0.10
Time for Color Change: 7.50 minutes
How would I find Rate(min^-1) with these? Please show me?
3 A2 --> products
The generic rate law for the reaction is rate = k[A2]^p
[A2]0 : 0.10
Time for Color Change: 7.50 minutes
How would I find Rate(min^-1) with these? Please show me?
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Change in concentration/time.
0.10/7.5 therefore (if the final concentration of A2 was zero).
0.10/7.5 therefore (if the final concentration of A2 was zero).