The equilibrium constant, K, for the following reaction is 7.00×10^-5 at 673 K.
NH4I(s) → NH3(g) + HI(g)
An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.380 mol NH4I, 8.37×10^-3 M NH3, and 8.37×10^-3 M HI.
If the concentration of HI(g) is suddenly increased to 1.24×10^-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?
[NH3] = M
[HI] = M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K.
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 CCl4.
What will be the concentrations of the three gases once equilibrium has been reestablished if 0.129 mol of CH4(g) is added to the flask?
2CH2Cl2(g) → CH4(g) + CCl4(g)
[CH2Cl2] = M
[CH4] = M
[CCl4] = M
The equilibrium constant, K, for the following reaction is 1.29×10^-2 at 600 K.
COCl2(g) → CO(g) + Cl2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.240 M COCl2, 5.57×10^-2 M CO, and 5.57×10^-2 M Cl2.
What will be the concentrations of the three gases once equilibrium has been reestablished if 4.48×10^-2 mol of CO(g) is added to the flask?
[COCl2] = M
[CO] = M
[Cl2] = M