All of the products are gases but I can't show that without using more than one line.
....(NH4)2CO3(s) = 2NH3 + CO2 + H2O
....solid...........2p......p.....p
So the total pressure of the system is due to the gases.
Total P = 2p + p + p = 0.8944 atm.
Solve for p and 2p and that gives you the partial pressures of each gas for part a.
b. Use PV = nRT and solve for n to find mols (NH4)2CO3 used, then convert to grams.
c. Write the Kp expression, substitute the partial pressures from a and solve for Kp.
Consider the following decomposition reaction of ammonium carbonate ((NH4)2CO3):
(NH4)2CO3 (s) 2 NH3 (g) + CO2 (g) + H2O (g)
In one experiment at 25.0°C, a sample of pure (NH4)2CO3 is placed in an evacuated 2.00 L vessel. At
equilibrium, the total pressure is found to be 0.8944 atm.
(a) Determine the equilibrium partial pressure of each gaseous species.
(b) Determine the mass of ammonium carbonate ((NH4)2CO3) that must have reacted in order to achieve
equilibrium.
(c) Determine the value of Kp assuming that the reaction temperature is 25.0°C.
for a) I started with PV=nRT to find the moles of ammonium carbonate, but I don't know where to go from there.
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