Week 9&10 Achieve #5

[andrea guzman 1F]

HI the question is asking what the initial rate will be if [A] is halved and [B] is tripled.
A+ B-> C + D rate= k[A][B]^2
initial rate = 0.0280 M/s
I have looked at the feedback and i have (1/2) for a since its being halved but I'm not sure if B would be 3(2) or 2^3.

[Aditya Narashim 1K]

The concentration of B will be [3]^2 and A will be [1/2] there multiplied with k will be the over rate of the reaction.

[Deep Mehta]

B would be multiplied by 9 because B is second order. 3^2

[Drake Snyder 1F]

If the concentration for a second-order reactant is tripled, it will change by a factor of (3)^2. So for this question, calculations should be 1/2 x 9 x initial rate = new initial rate. Hope this helps!

[405972194]

If A is halved then the initial rate will also be halved since A is in first order. If B is tripled then the initial rate will be 9x larger since B is in second order, the rate will be 3^2 larger.