Question

2A + B + 2C ? D + E

Answer 1

Answer:

C Rate $=k [A]^{2} [B][C]^{-1}$

Explanation:

In order to determine the correct rate law, let's use Trial 1 as baseline. Therefore:

An increase in [A] in Trial 2 by a factor of $\sqrt{2}$ leads to an increase in the rate of reaction by a factor of 2 (i.e. the reaction rate is doubled). Thus, there is second order in [A].

Similarly,

An increase in [B] in Trial 3 by a factor of 1.667 leads to an increase in the rate of reaction by a factor of 1.667. Thus, there is first order in [B].

Futhermore,

An increase in [C] in Trial 4 by a factor of 1.71 leads to a decrease in the rate of reaction by 1.71. Thus, there is inverse first order in [C].

Therefore, the correct rate law is:

Rate $=k [A]^{2} [B][C]^{-1}$