At 1127 K and 1 atom pressure, a gaseous mixture of CO and CO 2 in equilibrium with soild carbon has 90.55% CO by mass C (s) + CO 2 (g) ⇌ 2CO (g) Calculate K c for this reaction at the above temperature.

Question

Philoid · Accepted Answer

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 (K_p) 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 K_c = Equilibrium constant

K_p = 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

At 1127 K and 1 atom pressure, a gaseous mixture of CO and CO2 in equilibrium with soild carbon has 90.55% CO by massC (s) + CO2 (g) ⇌ 2CO (g)Calculate Kc for this reaction at the above temperature.

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 K_c for this reaction at the above temperature.