The total pressure at equilibrium is 0.07503 atm
The partial pressure of the product at equilibrium will be calculated as follows;
Kp = Kc[RT]³
given;
equilibrium constant Kc = 1.58 X 10⁻⁸
gas constant R = 0.0821 L.atm/mol.K
temperature T = (250 +273) = 523 k
Kp = 1.58 X 10⁻⁸ *(0.0821)³ *(523)³ = 1.251 X 10⁻³
NH₂COONH₄(s) ⇌ 2NH₃(g) + CO₂
NH₂COONH₄(s): Kp = 0, since it is in solid state
2NH₃(g) + CO₂: Kp = 1.251 X 10⁻³
I.C.E Analysis on the product
2NH₃(g) CO₂
I : 0 0
C : 2x x
E : (2x-0) (x-0)
At equilibrium, E: (2x-0)(x-0) = 1.251 X 10⁻³
(2x)(x) = 1.251 X 10⁻³
2x² = 1.251 X 10⁻³
x² = (1.251 X 10⁻³)/2
x² = 6.255 X 10⁻⁴
x = √(6.255 X 10⁻⁴)
x = 0.02501 atm
Partial pressure of 2NH₃(g) = 2x = 2(0.02501 atm) = 0.05002 atm
Partial pressure of CO₂ = x = 0.02501 atm
Total pressure = P(NH₃(g)) +P(CO₂)
Total pressure = 0.05002 atm + 0.02501 atm = 0.07503 atm
Therefore, the total pressure at equilibrium is 0.07503 atm
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