The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2C12(g) CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.48×10-2 M CH2C12, 0.178 M CH4 and 0.178 M CC14. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.60×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CC14] = M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2C12(g) CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.48×10-2 M CH2C12, 0.178 M CH4 and 0.178 M CC14. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.60×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CC14] = M
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Chapter1: Chemical Foundations
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![The equilibrium constant, K, for the
following reaction is 10.5 at 350 K.
2CH2C12(g) CH4(g) + CC14(g) An equilibrium
mixture of the three gases in a 1.00 L flask
at 350 K contains 5.48×10-2 M CH2Cl2,
0.178 M CH4 and 0.178 M CC14. What will
be the concentrations of the three gases
once equilibrium has been reestablished, if
4.60×10-2 mol of CH2Cl2(g) is added to the
flask? [CH2Cl2] = M [CH4] = M [CC14] = M
The equilibrium constant, K, for the
following reaction is 1.29×10-2 at 600 K.
COC12(g) CO(g) + Cl2(g) An equilibrium
mixture of the three gases in a 1.00 L flask
at 600 K contains 0.242 M COCI2, 5.59×10-
2 M CO and 5.59×10-2 M Cl2. What will be
the concentrations of the three gases once
equilibrium has been reestablished, if
2.90×10-2 mol of Cl2(g) is added to the
flask? [COCI2] = M [CO] = M [C12] = M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fab66b314-8fcd-4d7e-b2b2-d03028712de6%2Ffc851004-01f4-4c8d-b58d-c76d0bcbaecf%2F5xi13yb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, K, for the
following reaction is 10.5 at 350 K.
2CH2C12(g) CH4(g) + CC14(g) An equilibrium
mixture of the three gases in a 1.00 L flask
at 350 K contains 5.48×10-2 M CH2Cl2,
0.178 M CH4 and 0.178 M CC14. What will
be the concentrations of the three gases
once equilibrium has been reestablished, if
4.60×10-2 mol of CH2Cl2(g) is added to the
flask? [CH2Cl2] = M [CH4] = M [CC14] = M
The equilibrium constant, K, for the
following reaction is 1.29×10-2 at 600 K.
COC12(g) CO(g) + Cl2(g) An equilibrium
mixture of the three gases in a 1.00 L flask
at 600 K contains 0.242 M COCI2, 5.59×10-
2 M CO and 5.59×10-2 M Cl2. What will be
the concentrations of the three gases once
equilibrium has been reestablished, if
2.90×10-2 mol of Cl2(g) is added to the
flask? [COCI2] = M [CO] = M [C12] = M
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