Question

Part A Consider the following reaction: A + B + C \rightarrow D The rate law for this reaction is as follows: Rate = k \frac{[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 = 1.368 \cdot 10^{-1} M/s

          Part A
Consider the following reaction:
A + B + C \rightarrow D
The rate law for this reaction is as follows:
Rate = k \frac{[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 = 1.368 \cdot 10^{-1} M/s

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 ×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 = 1.368 ·10^-1 M/s

Added by Linda B.

Computer Science and Information Technology

Trishna Knowledge Systems 2018 Edition

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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 x 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