Equal volumes of two equimolar solutions of reactants a and b are mixed, and the reaction a+b→c occurs. at the end of 1h, a is 90% reacted. how much of a will be left unreacted at the end of 2h if the reaction is: part a first order in a and zero order in b? express your answer in percent using two significant figures, leave the percent sign out of your answer. [a] = 1.0 % submitmy answersgive up correct part b first order in a and first order in b?

Question

Bria Shea

Chemistry

25 June, 19:44

Equal volumes of two equimolar solutions of reactants a and b are mixed, and the reaction a+b→c occurs. at the end of 1h, a is 90% reacted. how much of a will be left unreacted at the end of 2h if the reaction is: part a first order in a and zero order in b? express your answer in percent using two significant figures, leave the percent sign out of your answer. [a] = 1.0 % submitmy answersgive up correct part b first order in a and first order in b?

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Oswaldo Wallace · Answer 1

a) First order in A and zero order in B

ln [A] = (ln 0.1) (2) + ln Ao = ln 0.01 + ln Ao = ln 0.01 Ao = 1.0% of A will remain

b) First order in A and first order in B

1/[A] - 1/[A]0 = kt where t+=1 and k=9

[A]/[A]=1/19=0.053=5.3%

c) Zero order in both A and B

[A]0-[A] = kt

Then at 2 hours [A]=0 All of it has reacted.