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The equilibrium constant, K, for the following reaction is 1.29x102 at 600 K. COCI₂(g) CO(g) + Cl₂(g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.264 M COCI2, 5.83×10-2 M CO and 5.83x102 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.50x102 mol of Cl₂(g) is added to the flask? [CoCl₂] = [CO] [Cl₂] ΣΣΣ 3
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH₂Cl₂(9) CH4(9) + CCl4(9) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.55x10-2 M CH₂Cl₂, 0.180 M CH4 and 0.180 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.125 mol of CH4(g) is added to the flask? [CH₂Cl₂]- [CH4] [CC14] = M ΣΣΣ M M