CHEMISTRY COMMUNITY

CH4(g) + 2H2S(g)-------> CS2(g) + 4H2(g)
a.) 2.00 mol of CH4, 2.00 mol of CS2, 4.00 mol of H2S, and 4.00 mol of H2 are mixed in a 500 ml vessel at 960 K. Kc=0.046 for this reaction. Show using calculations if this reaction is at equilibrium. If not, which direction will the reaction process?
b.) Fully describe what will happen if the volume decreased at constant temperature.
How do you do this problem?

Since the problem gives you Kc, you must convert moles of the reactants to pressure values (using PV=nRT).

Find the reaction quotient, Q, and compare that value to Kc. If the values are equal, then the reaction is at equilibrium. If Q>Kc, then reverse reaction is favored. If Q<Kc, then forward reaction is favored.

If the volume decreases, then the reaction will favor side with less gas (since pressure increased, we want less gas molecules according to Le Chatelier's).

Kc, you must convert moles of the reactants to pressure values using PV=nRT the ideal gas law