Hydrogen sulfide decomposes according to the following reaction, for which Kc=9.30×108 at 700∘C, 2H2S(g)⇌2H2(g)+S2(g) If 0.45 mol of H2S is placed in a 3.0 -L container, what is the equilibrium concentration of H2g at 700∘C?
Hydrogen sulfide decomposes according to the following reaction, for which Kc=9.30×108 at 700∘C, 2H2S(g)⇌2H2(g)+S2(g) If 0.45 mol of H2S is placed in a 3.0 -L container, what is the equilibrium concentration of H2g at 700∘C?