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Question
1 mol of CH4, 1 mole of CS2 and 2 mol of H2S are 2 mol of H2 are mixed in a 500 ml flask. The equilibrium constant for the reaction Kc = 4 x 10-2 mol2 lit-2. In which direction will the reaction proceed to reach equilibrium?
Solution
CH4(g) + 2 H2S (g) ⇌ CS2(g) + 4H2(g)
Kc = 4 x 10-2 mol2 lit-2
Volume = 500 ml = `1/2`L
[CH4]in = `(1 "mol")/(1/2 "L")` = 2 mol L-1
[CH2]in = `(1 "mol")/(1/2 "L")` = 2 mol L-1
`["H"_2"S"]_"in" = (2 "mol")/(1/2 "L")`= 4 mol L-1
`["H"_2]_"in" = (2 "mol")/(1/2 "L")`= 4 mol L-1
Q = `(["CS"_2]["H"_2]^4)/(["CH"_4]["H"_2"S"]^2)`
`= ([2][4]^4)/([2][2]^2)`
= 64 mol2 lit-2
Q > KC.
∴ The reaction will proceed in the reverse direction to reach the equilibrium.
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