solid (NH4)2CO3 is placed in an evacuated container at 115C. When equilibrium is reached the total pressure inside the vessel is 0.473 atm. Some solid remain in the vessel at equilibrium. Calculate Kp.

..........(NH4)2CO3 ==> 2NH3 + CO2 + H2O

I..........solid.........0......0.....0
C..........solid........2p......p.....p
E..........solid........2p......p.....p

Kp = p^2NH3 * pCO2 * pH2O
Ptotal = pNH3 + pCO2 + pH2O
0.473 = 2p + p + p = 4p
Solve for p and substitute into Kp expression and solve for Kp.

To calculate the equilibrium constant (Kp) for the given reaction, we need to know the balanced equation of the reaction involving (NH4)2CO3.

Unfortunately, the given information does not provide us with the balanced equation, but we can use the provided information to determine the partial pressures of the gaseous components involved in the reaction.

The reaction likely involves the decomposition of (NH4)2CO3 into gaseous components, which are NH3 and CO2. The decomposition reaction is given by:

(NH4)2CO3(s) → 2NH3(g) + CO2(g)

Let's assume that x is the number of moles of (NH4)2CO3 that decompose. According to the balanced equation, we will form 2x moles of NH3 and x moles of CO2.

Now, we need to calculate the partial pressures of NH3 and CO2 at equilibrium. We know that the total pressure inside the vessel is 0.473 atm. Since the solid (NH4)2CO3 remains in the vessel at equilibrium, the partial pressures of NH3 and CO2 contribute towards the total pressure.

Using the ideal gas law, we can express the partial pressure of each gas in terms of moles and temperature.

For NH3:
P(NH3) = (2x/total moles) * Total Pressure
= (2x/(2x + x)) * 0.473 atm
= (2/3) * 0.473 atm
= 0.315 atm

For CO2:
P(CO2) = (x/total moles) * Total Pressure
= (x/(2x + x)) * 0.473 atm
= (1/3) * 0.473 atm
= 0.157 atm

Now, we have the partial pressures of NH3 and CO2 at equilibrium. To calculate Kp, we can express it as the ratio of the product of the partial pressures of the products to the product of the partial pressures of the reactants, with each raised to their respective stoichiometric coefficients.

Kp = (P(NH3))^2 * P(CO2)

Substituting the values we have calculated:
Kp = (0.315 atm)^2 * 0.157 atm

By multiplying these values, we can determine the value of Kp.