The equilibrium constant, K_{c}, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, K_{p}, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation

K_{p} = K_{c} (RT)^{Δn}

where R = 0.08206 L•atm/(K•mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles product - sum moles reactants). For example, consider the reaction

N_{2}(g) + 3H_{2}(g) ⇌ 2NH_{3}(g)

for which Δn = 2 - (1 + 3) = -2

Part A.

For the reaction

3A(g) + 3B(g) ⇌ C(g)

K_{c} = 29.8 at a temperature of 293°C. Calculate the value of K_{p}. Express your answer numerically.

Part B.

For the reaction

X(g) + 3Y(g) ⇌ 2Z(g)

K_{p} = 3.41 x 10^{-2} at a temperature of 203°C. Calculate the value of K_{c}. Express your answer numerically.

Equilibrium Expressions

Equilibrium Expressions

Equilibrium Expressions

Equilibrium Expressions