Missing information:
Equilibrium reaction: NH2COONH4(s)⇌2NH3(g)+CO2(g)
Answer:
14.43 atm
Explanation:
The equilibrium occurs when in a reversible reaction, the velocity of the formation of the products is equal to the velocity of the formation of the reactants. When this occurs, the concentration and partial pressures remain constant. To characterize the equilibrium there's the equilibrium constant, which can be based on the concentration (Kc) or based on the gases partial pressure (Kp).
The conversion between them is:
Kp = Kc*(RT)⁻ⁿ
Where n is the variation of the coefficients of the gas substances (reactants - products) so, n = 0 - (2+1) = -3
Kp = Kc*(RT)³
R is the gas constant (0.082 atm.L/mol.K), and T is the temperature ( 240°C = 513 K), so:
Kp = 0.006*(0.082*513)³
Kp = 446.6
The value of Kp is also the ratio between the multiplication of the partial pressures of the products divided by the partial pressure of the reactants, each one elevated by the coefficient of the substance, and only for gas substances, so:
Kp = (pNH3)²*(pCO2)
Doing an equilibrium chart
NH3 CO2
0 0 Intial
+2x x Reacts (stoichiometry is 2:1)
2x x Equilibrium
446.6 = (2x)²*x
4x³ = 446.6
x³ = 111.65
x = ∛111.65
x = 4.81 atm
pNH3 = 2*4.81 = 9.62 atm
pCO2 = 4.81 atm
By Dalton's law, the total pressure of a gas mixture is the sum of the partial pressure of the substances:
P = 9.62 + 4.81 = 14.43 atm
