7. Consider the following: CH4(g)+H2O(g)CO(g)+3H2(g) The reaction starts with a mixture of 0.15MCH4,0.30MH2O,0.40MCO, and 0.60MH2 and is allowed to reach equilibrium. At equilibrium the concentration of CH4 is found to be 0.05M. Calculate the equilibrium constant, Kc, for the reaction. 8. Nitric oxide, an important air pollutant, is produced in automobile engines at elevated temperatures according to the reaction: N2(g)+O2(g)2NO(g)H0=+180.5kJ What is the effect of increasing the pressure on this equilibrium, assuming no change in temperature? 9. Consider the decomposition of limestone, CaCO3, represented by the equation: CaCO3(s)CaO(s)+CO2(g)H=+178.5kJ What is the effect on the equilibrium position of (a) An increase in pressure? (b) Adding a catalyst? 10. The initial step of the Ostwald process for the industrial production of nitric acid is the oxidation of ammonia to nitric oxide: 4NH3(g)+5O2(g)4NO(g)+6H2O(g)H=905.6kJ What is the effect of the equilibrium position: (a) The temperature is increased? (b) A platinum catalyst is added? (c) The pressure is increased by adding helium gas