Chemistry, 26.03.2020 21:03, estefaniapenalo
When heated, hydrogen sulfide gas decomposes according to the equation: 2H2S(g) ā 2H2(g) + 2S2(g) A 6.75 gram sample of H2S(g) is introduced into an evacuated rigid 0.75 L container. The sealed container is heated to 283 K and 6.42 x 10 ^ā2 mol of S2 gas is present at equilibrium.
a. Calculate the equilibrium concentration, in mol/L, of the H2(g) in the container at 283 K.
b. Calculate the equilibrium concentration, in mol/L, of the H2S(g) in the container at 283 K.
c. Calculate the value of the equilibrium constant, Kc, for the decomposition reaction at 283 K.
d. Calculate the partial pressure of S2(g) in atm in the container at equilibrium at 283 K.
e. Calculate the value of the equilibrium constant, Kc, for the reaction
H2(g) + 1/2 S2(g) ā H2S (g) at 283 K.
Answers: 2
due to stoichiometry and the reaction extent, turns out:![K=\frac{[H_2]_{eq}^2[S_2]_{eq}}{[H_2S]_{eq}^2}](/tpl/images/0565/7677/a5ff5.png)
![[H_2S]_0=\frac{6.75g/(34g/mol)}{0.75L} =0.265M](/tpl/images/0565/7677/26ae9.png)
![[S_2]_{eq}=x=\frac{6.42x10^{-2}mol}{0.75L}=0.0856M](/tpl/images/0565/7677/c4de0.png)
![[H_2]_{eq}=2x=2*0.0856M=0.171M](/tpl/images/0565/7677/0a782.png)
![[H_2S]_{eq}=0.265M-2x=0.265M-2*0.0856M=0.0938M](/tpl/images/0565/7677/de91b.png)
![p_{S_2}=[S_2]RT= 0.0856\frac{mol}{L}*0.082\frac{atm*L}{mol*K}*283K=1.99atm](/tpl/images/0565/7677/136fa.png)
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When heated, hydrogen sulfide gas decomposes according to the equation: 2H2S(g) ā 2H2(g) + 2S2(g) A...
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