At 1127 K and 1 atom pressure, a gaseous mixture of CO and CO2 in equilibrium with soild carbon has 90.55% CO by mass
C (s) + CO2 (g) ⇌ 2CO (g)
Calculate Kc for this reaction at the above temperature.
Let us assume that the total mass of the gaseous mixture is 100g
Therefore, mass of CO = 90.55g
And mass of CO2 = (100-90.55) = 9.45g
Number of moles of CO,
Numb we of moles of CO2,
Partial pressure of CO,
Partial pressure of CO2,
Equilibrium pressure constant (Kp) is defined as a number that expresses the relationship between the partial pressures of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature.
Therefore,
Also, we know that,
Where Kc = Equilibrium constant
Kp = 14.19 atm
R = 0.081 L atm/K mol
T = 1127 K
Δng = Sum of stochiometric coefficients of products – Sum of stochiometric coefficients of reactants = 2-1 = 1