Part A\ Consider the following reaction:\

A+B+C->D

\ The rate law for this reaction is as follows:\ Rate

=k([A][C]^(2))/([(B)]^((1)/(2)))

\ Suppose the rate of the reaction at certain initial concentrations of

A,B

, and

C

is

1.14\\\\times 10^(-2)(M)/(s)

.\ What is the rate of the reaction if the concentrations of

A

and

C

are doubled and the concentration of

B

is tripled?\ Rate

2=

\

(M)/(s)

\ Previous Answers\ Request Answer

Consider the following reaction: A+B+CD The rate law for this reaction is as follows: Rate=k[B]1/2[A][C]2 Suppose the rate of the reaction at certain initial concentrations of A,B, and C is 1.14102M/s. What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Consider the following reaction: A+B+CD The rate law for this reaction is as follows: Rate=k[B]1/2[A][C]2 Suppose the rate of the reaction at certain initial concentrations of A,B, and C is 1.14102M/s. What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled