The equilibrium constant, K, for the following reaction is 10.5 at 350K. 2CH2Cl2(g)CH4(g)+CCl4(g) An equilibrium mixture of the three gases in a 1.00L flask at 350K contains 5.5110MCH2Cl2,0.178MCH4 and 0.178M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.83102mol of CH2Cl2(g) is added to the flask? [CH2Cl2][CH4]=[CCl4]==MMM 8 more group attempts remaining