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### Integrated Rate Laws when a =/= 1

Posted: Fri Mar 02, 2018 1:24 pm
For a reaction like 2H2O2 --> 2H2O + O2, should we integrate a rate law using a = 2 or just use the ones given to us on the constant sheet? I know that the integrated first-order rate law for this would be ln[A] = ln[A]0 - 2kt, but I remember being told to just use the a = 1 rate law. Can someone clarify why?

### Re: Integrated Rate Laws when a =/= 1

Posted: Fri Mar 02, 2018 11:23 pm
I am not sure if I will be able to exactly answer your question, but I think each order has it's own integrated rate law. To find the order, I suggest using the given concentrations and if time is also given, then plot each type of integrated rate law and see what the order is based off of that.

### Re: Integrated Rate Laws when a =/= 1

Posted: Fri Mar 02, 2018 11:23 pm
I am not sure if I will be able to exactly answer your question, but I think each order has it's own integrated rate law. To find the order, I suggest using the given concentrations and if time is also given, then plot each type of integrated rate law and see what the order is based off of that.

### Re: Integrated Rate Laws when a =/= 1

Posted: Sat Mar 03, 2018 12:10 pm
Why is the integrated first-order rate law for that chemical equation ln[A] = ln[A]0 - 2kt?

### Re: Integrated Rate Laws when a =/= 1

Posted: Sun Mar 04, 2018 2:16 pm
Because to find the first order integrated rate law, we integrate (-1/a)d[A]/dt = -k[A], where a is the coefficient of the reactant.