Question

The relation between $K_p$ and $K_c$ of a reversible reaction at fixed temperature is $K_p=K_c{\left(RT\right)}^{\Delta n}$.
If true enter 1, if false enter 0.

Answer 1

The relation between $K_p$ and $K_c$ of a reversible reaction at fixed temperature is $K_p=K_c{\left(RT\right)}^{\Delta n}$.

where,
$K_c$ is the equilibrium constant when the concentrations of the reactants are expressed in terms of molarity (moles per litre).
$K_p$ is the equilibrium constant when the concentrations of the reactants are expressed in terms of partial pressure.
$\Delta n=$ number of moles of products $-$ number of moles of reactants.

$R=$ gas constant.

$T=$ absolute temperature.