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We are given that this is a first order reaction, 2A -> B + C, given that [A]0 = 0.153 mol/L and that after 115sec the conc. of B rises to 0.034 mol/L. How would we go about solving for [A]?
Using the balanced mock chemical reaction, you can use stoichiometry to convert from [B] to [A]. Then, using the concentration of A that you solve in this manner, you can use the integrated rate law of the first order. Hope this helps.
^to add on, you have to subtract the new [A] from the initial [A]. so when you use the molar ratio to get [A] when [B] = .034 mol/L, you should get [A] = .068 mol/L. then you have to subtract from the initial: .153 - .068 = .085 mol/L. this is the [A] you should use for your computation
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