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The rate of the reaction $2NO + Cl_2 \rightarrow 2NOCl$ is given by the rate equation rate = $k[NO]^2[Cl_2]$. The value of the rate constant can be increased by
A
Increasing the temperature
B
Increasing the concentration of NO
C
Increasing the concentration of the $Cl_2$
D
Doing all of these
Detailed Solution
The rate constant k is characteristic of a reaction at a given temperature; it does not depend on the concentrations of the reactants.
Increasing [NO] or [$Cl_2$] increases the rate of the reaction, but the value of k stays the same.
The dependence of k on temperature is given by the Arrhenius equation: $k = Ae^{-E_a/RT}$
As T increases, $e^{-E_a/RT}$ increases, so k increases (roughly doubling for every 10 K rise).
Hence the rate constant can be increased by increasing the temperature.
Increasing [NO] or [$Cl_2$] increases the rate of the reaction, but the value of k stays the same.
The dependence of k on temperature is given by the Arrhenius equation: $k = Ae^{-E_a/RT}$
As T increases, $e^{-E_a/RT}$ increases, so k increases (roughly doubling for every 10 K rise).
Hence the rate constant can be increased by increasing the temperature.