The following graph shows how $T_{1/2}$ (half-life) of a reactant $R$ changes with the initial reactant concentration $a_0$. The order of the reaction will be:

Assuming the reaction $2NO_{(g)} + Cl_{2(g)} \longrightarrow 2NOCl_{(g)}$ occurs in a single elementary step,we can say that

$A$ reaction is of second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled,keeping everything else constant,the rate of the reaction will...

Write the equation for a pseudo first order reaction. Write the rate law and the rate constant.

The rate equation for the reaction $2A + B \longrightarrow \text{products}$ is $\text{rate} = k[A][B]^2$. If $k$ at $T \, K$ is $5.0 \times 10^{-6} \, mol^{-2} \, L^2 \, s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \, mol \, L^{-1}$ and $[B] = 0.1 \, mol \, L^{-1}$ is:

For an elementary reaction,$2A + B \to C + D$,the molecularity is: