Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(?)+H2O(?)⇌3H2(?)+CO(?)CH4(g)+H2O(g)⇌3H2(g)+CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C?

For the following reaction, the equilibrium constant Keq is 6.40 x 10-7 at 2000°C. 2CO2 (g)  2CO (g) + O2 (g) If 0.250 moles of CO2(g) is introduced into a 1.00 L vessel, calculate the equilibrium concentrations of CO(g) and O2(g) at this temperature.

At a certain temperature, the equilibrium constant K for the following reaction is 0.71: N2(g) + O2(g) =2 NO(g) Use this information to complete the following table. Suppose a 43. L reaction vessel is filled with 1.0 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K =0 2 NO(g) N,(9)+O2(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 3 N2(9)+30,(9) 6 NO(g)

Consider the following reaction where Kc = 7.00 × 10-5 at 673 K. NH₂I(s) NH3(g) + HI(g) A reaction mixture was found to contain 0.0532 moles of NHI(s), 0.00571 moles of NH3(g), and 0.00837 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction must run in the forward direction to reach equilibrium. © must run in the reverse direction to reach equilibrium. O is at equilibrium.