Question

Taking the reaction, $A+2B\to Products$, to be of the second order, which of the following may be the correct rate law expressions?

• A. $\frac{dx}{dt}=k\left[A\right]\left[B\right]$
• B. $\frac{dx}{dt}=k\left[A\right][B{]}^2$
• C. $\frac{dx}{dt}=k[A{]}^2$
• D. $\frac{dx}{dt}=k_1\left[A\right]+k_2[B{]}^2$

Answer 1

Answer: (A), (C)

$\frac{dx}{dt}=k\left[A\right]\left[B\right]$
$\frac{dx}{dt}=k[A{]}^2$

option A and C are correct as the sum of their exponents equals to 2