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Sauron [17]
3 years ago
12

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 9

0% 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?
Chemistry
1 answer:
SVEN [57.7K]3 years ago
8 0

<span>a)    </span>First order in A and zero order in B

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

<span>b)    </span>First order in A and first order in B

<span>1/[A] – 1/[A]0= kt where t+=1 and k=9</span>

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

<span>c)    </span>Zero order in both A and B

<span>[A]0-[A] = kt</span>

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

 

<span> </span>

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