Question

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 5.51×10^-2 M CH₂Cl₂,   0.178 M CH₄ and 0.178 M CCl₄. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.79×10^-2 mol of CH₂Cl₂(g) is added to the flask?

[CH2Cl2]	=	____ M
[CH4]	=	____ M
[CCl4]	=	____M

The equilibrium constant, K, for the following reaction is 1.80×10^-4 at 298 K.

• NH₄HS(s) <------> NH₃(g) + H₂S(g)

An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.200 mol NH₄HS,   1.34×10^-2 M NH₃ and 1.34×10^-2 M H₂S. If the concentration of NH₃(g) is suddenly increased to 2.06×10^-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?

[NH3]	=	_____M
[H2S]	=	_____M

The equilibrium constant, K, for the following reaction is 1.18×10^-2 at 588 K.

• NH₄Cl(s) <------> NH₃(g) + HCl(g)

An equilibrium mixture in a 10.5 L container at 588 K contains 0.294 mol NH₄Cl(s), 0.140 M NH₃ and 8.43×10^-2 M HCl. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.27 L?

[NH3]	=	____ M
[HCl]	=	____ M

Answer 1