The equilibrium constant, K, for the following reaction is 1.80E-2 at 698 K. 2 HI(g) H₂(g) + 12(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.302 M HI, 4.05E-2 M H₂ and 4.05E-2 M 12. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.266 mol of HI(g) is added to the flask? [HI] = [H₂] = [12] = M M M

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