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February 7, 2016

# Homework Help: Chemistry.

Posted by Jill on Monday, November 22, 2010 at 4:14pm.

Ca(HCO3)2(s) decomposes at elevated temperatures according to the stoichiometric equation Ca(HCO3)2(s)-> CaCO3(s) + H2O(g) + CO2(g)

a.) If pure Ca(HCO3)2(s) is put into a sealed vessel, the air is pumped out, and the vessel and its contents are heated, the total pressure is 0.235 bar. Determine Kp under these conditions.

b.) If the vessel initially also contains 0.105 bar H2O(g), what is the partial pressure of CO2(g) at equilibrium?
• Chemistry. - DrBob222, Tuesday, November 23, 2010 at 12:19am

Ca(HCO3)2(s)-> CaCO3(s) + H2O(g) + CO2(g)

Total pressure is 0.235 bar. Since the mole ratio is 1:1, the partial pressure H2O and partial pressure of CO2 must be the same; therefore, 2x = 0.235 and x = 0.235/2.
Then Kp = P(CO2)*P(H2O) = ??

b).
.....CO2 + H2O
...0.105 bar..0
.... + x....+x
final is 0.105+x and x
Substitute into Kp expression and solve for x.

• Chemistry. - Anonymous, Thursday, April 25, 2013 at 9:52pm

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