Wednesday
September 3, 2014

Homework Help: AP CHEM

Posted by Jenn on Thursday, March 15, 2007 at 7:26pm.

I would really appreciate some help on this problem. =)

At 218 C, Kc = .00012 for the equilibrium

NH4HS(s)<==> NH3(g)+ H2S(g)

Calculate the equilibrium concentrations of NH3 and H2S if a sample solid NH4HS is placed in a closed vessel and decomposes until equilibrium is reached.

Part (B) If the flask has a volume of 0.500L, what is the minimum mass of NH4HS(s) that must be added to the flask to achieve equilibrium?

Write the Kc expression for the reaction.
Kc = 0.00012=(H2S)(NH3)
Since (H2S)=(NH3), then
(NH3)^2=(H2S)^2 = 0.00012
Solve for (NH3).

For part b, you know concentration of NH3 and H2S in mols/L. In 1/2 L there will be how many mols? And how many mols NH4HS provided this? And what is the mass of NH4HS that provides this many mols? Post your work if you get stuck.

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