I came across this question from the 2000 AP exam, and it seemed easy and so I answered it by now I don't know if it's right!!
H2S(g) 2 H2(g) + S2(g)
(a reverse reaction!)
When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g sample of H2S(g) is introduced into an
evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72 ×10-2 mol of S2(g) is present at equilibrium.
(a) Calculate the equilibrium concentration, in mol L-1, of the following gases in the container at 483 K.
(i) H2(g)
(ii) H2S(g)
(b) Calculate the partial pressure of S2(g) in the container at equilibrium at 483 K.
Thank you!
2007-02-06
05:29:20
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4 answers
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asked by
Anonymous