The equilibrium constant, K, for the following reaction is 1.80x10-2 at 698 K. 2HI(g) =H2(g) + 12(9) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.326 M HI, 4.38x10-2 M H2 and 4.38x10-2 M 12. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.214 mol of HI(g) is added to the flask? [HI] = [H2] - [12]