2A + 3B + C ⟶ D + E

The rate constant for this reaction is 0.25, and the reaction is second order in A and is first order in B and C.

Which option correctly gives the rate of the reaction if [A] is 0.4 M, [B] is 0.1 M and [C] is 0.2 M?

I don't see any options. But write the rate constant expression and compare it with the options. Post your work if you get stuck.

I got it, 8.0 × 10^-4

To determine the rate of the reaction, you need to use the rate equation, which is derived from the stoichiometry of the balanced chemical equation and the given reaction orders.

The rate equation for this reaction can be written as follows:

Rate = k[A]^2[B][C]

Where:
- [A], [B], and [C] are the concentrations of A, B, and C, respectively.
- k is the rate constant.

Given that the reaction is second order in A and first order in B and C and the rate constant is 0.25, we can substitute the given concentrations into the rate equation to calculate the rate of the reaction.

Rate = k[A]^2[B][C]
= (0.25)(0.4 M)^2(0.1 M)(0.2 M)

Calculating the value gives us:

Rate = (0.25)(0.16)(0.1)(0.2)
= 0.008

Therefore, the correct rate of the reaction, using the given concentrations, is 0.008 M/s.

2.0 x 10^-3 is wrong