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



23
1