How do you solve for c? The question is determine the rate constant for each of the following 1st-order reactions, in each case expressed for the rate of loss
(c)2A-->B + C,given that[A]0 = 0.153mol L 1 and that after 115 s the concentration of B rises to 0.034 mol L 1.
Question 15.23
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Re: Question 15.23
You find the concentration of A used up, which is stoichiometry since you're given the concentration of B that rises. Then you subtract the concentration of A used up from the initial concentration of A for the final concentration. After that, since it's a first order reaction you use the equation ln[A] = -kt + ln[A]0 to solve for the rate constant, since you know t = 115 seconds.
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Re: Question 15.23
You use stoichiometry to figure out how much of A is used up to form B. From the equation you gave, A should be used up half as fast as B is created, so you would multiply B by 2 and subtract it from A. Then you use the equation ln([A]/[A0]=-kt to find how much time has elapsed.
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