It seems like there's a mistake in your question. The reaction rate for the reaction XA + YB - ZC is usually expressed as -d[A]/dt = k[A]^x[B]^y, where k is the rate constant, and x and y are the orders of the reaction with respect to A and B. The term -d[B_1.5 is not clear. Could you please clarify or correct your question?

Question

It seems like there's a mistake in your question. The reaction rate for the reaction XA + YB -> ZC is usually expressed as -d[A]/dt = k[A]^x[B]^y, where k is the rate constant, and x and y are the orders of the reaction with respect to A and B. The term -d[B_1.5 is not clear. Could you please clarify or correct your question?

Knowee AI · Accepted Answer

It seems like there's a mistake in your question. The reaction rate for the reaction XA + YB -> ZC is usually expressed as -d[A]/dt = k[A]^x[B]^y, where k is the rate constant, and x and y are the orders of the reaction with respect to A and B. The term -d[B_1.5 is not clear. Could you please clarify or correct your question?

For the reaction, XA + YB - ZC, -d[A]_-d[B_1.5

Question

Solution

Similar Questions

Upgrade your grade with Knowee