Question

Show proper I.C.E. setup!!!!!!!!!!!! and calculations please! units and correct significant figures also! Thanks so much!

In the reaction below, 1.00 mol CH_4, 2.00 mol H₂S, 1.00 mol CS₂, and 2.00 mol H₂are mixed in an evacuated 250.0 mL reactor at 960degrees celsius, whereK_c=0.036. If[CH₄] = 5.56 M at equilibrium, calculate the equilibrium concentrations of the other three chemicals.

CH₄(g) + 2H₂S(g) <-------> CS₂(g) + 4H₂(g)

Equilibrium Concentration H₂S=

Equilibrium Concentration CS₂=

Equilibrium Concentration H₂=

Answer 1

Molarity of CH4 = number of moles of CH4/Volume of solution (L) = 4M

Molarity of H2S = 8M

Molarity of CS2 = 4M

Molarity of H2 = 8M

CH₄(g) + 2H₂S(g) <-------> CS₂(g) + 4H₂(g)

Since CH4 concentration is higher than the previous concentration, hence the reaction is proceeding in the backward direction

4+x        8+2x                 4-x         8-4x

4 + x = 5.56

x = 1.56

Equlibrium concentration of H2S = 8 + 2x = 8 + 2(1.56) = 11.12 M

Equilbrium concentration of CS2 = 4 - x = 4 - 1.56 = 2.44 M

Equilibrium concentration of H2 = 8 - 4x = 8 - 4(1.56) = 1.76 M