6. The equilibrium concentrations of H2,I2, and HI at 700K are 0.0058M+0.105M, and 0.190M respectively. Calculate the value of the equilibrium constant, K8, for the reaction: H2(g)+I2(g)2HI(g) at 700K. 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 CH2 is found to be 0.05M. Calculate the equilibrium constant. Ka 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)AH0=+180.5kJ What is the effect of increasing the pressure on this equilibrium, assining no change in temperature