Question

Which one of the following changes could double the rate of the reaction 2 A(g) + B(g) + 3 C(g) → 3 D(g) + E(g) with the rate law Rate = k[A][B]²?

Answer 1

Answer:

Increasing B's concentration and decreasing A's concentration

Explanation:

Rate = k [A] [B] ^2

If we double the concentration of B then according to the equation given (Refer 1st line) rate will increase 4 times and simultaneously if we decrease the concentration of A i.e by half so it will balance the equation as

Rate = k [A/2] [4B] ([2B]^2)

4 will be cancelled by 2 and thus this change can double the rate.

Hope it helps

Answer 2

Answer:

Doubling A

Explanation:

Doubling the concentration of A would result in the doubling of the rate. If the concentration of B were doubled, it would result in the rate being quadrupled.