Question

The relationship between $K_p$ and $K_c$ is correctly shown as :

• A. $K_c=K_p{\left(RT\right)}^{\Delta n}$
• B. $K_p=K_c{\left(RT\right)}^{-\Delta n}$
• C. $K_p=K_c{\left(RT\right)}^{\Delta n}$
• D. $K_c=K_p{\left(RT\right)}^{-\Delta n}$

Answer 1

Answer: (C), (D)

The correct options are
C $K_p=K_c{\left(RT\right)}^{\Delta n}$
D $K_c=K_p{\left(RT\right)}^{-\Delta n}$

The relationship between $K_p$ and $K_c$ is correctly shown as $K_p=K_c{\left(RT\right)}^{\Delta n}$ or

$K_c=K_p{\left(RT\right)}^{-\Delta n}$.

$K_c$ and $K_p$ are the equilibrium constants of gaseous mixtures.

However, the difference between the two constants is that $K_c$ is defined by molar concentrations, whereas $K_p$ is defined by the partial pressures of the gasses inside a closed system.