For the reaction, $A_{2} + B + C \to A C + A B$ , it is found that tripling the concentration of $A_{2}$ triples the rate, doubling the concentration of C doubles the rate and doubling the concentration of B has no effect.
(a) What is the rate law?
(b) Why the change in concentration of B has no effect?

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Solution

$A_{2} + B + C \to A C + A B$
A) $R a t e l a w = K [A] [C]$
B) Change in concentration of B has no effect of Rate because it has order equals zero with respect to B

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For the reaction, A2+B+C→AC+AB, it is found that tripling the concentration of A2 triples the rate, doubling the concentration of C doubles the rate and doubling the concentration of B has no effect.(a) What is the rate law?(b) Why the change in concentration of B has no effect?

A2+B+C→AC+ABA) Ratelaw=K[A][C]B) Change in concentration of B has no effect of Rate because it has order equals zero with respect to B

$A_{2} + B + C \to A C + A B$
A) $R a t e l a w = K [A] [C]$
B) Change in concentration of B has no effect of Rate because it has order equals zero with respect to B