The following reaction 2H₂S(g) = 2H2(g) + S2(g), Kc = 1.67 x 10-7 at 800°C is carried out at 800 °C with the following initial concentrations: [H₂S] = 0.100M, [H₂] = 0.100M, and [S₂] = 0.00 M. Find the equilibrium concentration of S2.

At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6.  Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M.  Your answer should have two significant figures.

A chemical engineer is studying the following reaction: 2 NO(g)+2H,(9) - N2(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel ΝΟ 6.78 atm O f increase Ot decrease O (no change) H, 2.93 atm ↑ increase OI decrease O (no change) A N2 5.23 atm f increase I decrease (no change) H, O 7.24 atm t increase I decrease (no change) NO 5.29 atm f increase I decrease (no change) H, 1.44 atm f increase OI decrease (no change) В N2 5.98 atm increase I decrease (no change) H, O 8.73 atm f increase O I decrease O (no change)…

The equilibrium constant K. for the reaction H2(g) + Br2(g) == 2HB1(g) is 2.18 × 10° at 730°C. Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.