Integrated Rate Laws when a =/= 1

[Joanne Guan 1B]

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?

[Yashaswi Dis 1K]

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.

[Yashaswi Dis 1K]

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.

[404995677]

Why is the integrated first-order rate law for that chemical equation ln[A] = ln[A]0 - 2kt?

[Joanne Guan 1B]

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.