The rate law for the reaction $A + B \rightarrow P$ is found to be rate $= k[A]^2[B]$.
The rate constant of the reaction at 300 K is $6.0\ \text{M}^{-2}\text{s}^{-1}$. Calculate the rate of the reaction when $[A] = 1\ \text{M}$ and $[B] = 0.2\ \text{M}$

If for a first-order reaction, $[A]_0 = 1.0\ \text{M}$ and $[A]_t = 0.25\ \text{M}$ after 276 s, find the value of the rate constant (k).

The equation for the rate constant is $k = Ae^{-E_a/RT}$.
A chemical reaction will proceed more rapidly if there is a decrease in

What is the oxidation state of chromium in the final product when KI reacts with acidified potassium dichromate solution?