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The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) __=__CH4(g) +...

The equilibrium constant, K, for the following reaction is 10.5 at 350 K.

  • 2CH2Cl2(g) __=__CH4(g) + CCl4(g)


An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.55×10-2 M CH2Cl2, 0.180M CH4 and 0.180 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.52×10-2 mol of CCl4(g) is added to the flask?

[CH2Cl2] = M
[CH4] = M
[CCl4] = M
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