The equilibrium constant, K, for the following reaction is 9.25×10-3 at 692 K. NH4I(s) NH3(g) + HI(g) An equilibrium mixture in a 12.1 L container at 692 K contains 0.348 mol NH4I(s), 0.118 M NH3 and 7.84×10-2 M HI. 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 5.98 L? [NH3] = M [HI] = M
The equilibrium constant, K, for the following reaction is 9.25×10-3 at 692 K. NH4I(s) NH3(g) +...
The equilibrium constant, K, for the following reaction is 6.76×10-3 at 685 K. NH4I(s) NH3(g) + HI(g) An equilibrium mixture in a 11.7 L container at 685 K contains 0.229 mol NH4I(s), 0.101 M NH3 and 6.69×10-2 M HI. 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 6.27 L?
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 0.388 mol NH4I, 8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.46×10-2 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 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 0.335 mol NH4I, 8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.28×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?
(1). The equilibrium constant, K, for the following reaction is 1.32×10-3 at 565 K. NH4Cl(s) =NH3(g) + HCl(g) An equilibrium mixture in a 10.4 L container at 565 K contains 0.285 mol NH4Cl(s), 4.47×10-2 M NH3 and 2.95×10-2 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 4.25 L? [NH3] = M [HCl] = M
The equilibrium constant, K, for the following reaction is 2.57×10-4 at 549 K. NH4Cl(s) NH3(g) + HCl(g) An equilibrium mixture in a 14.3 L container at 549 K contains 0.321 mol NH4Cl(s), 1.97×10-2 M NH3 and 1.30×10-2 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 6.96 L? [NH3] = __________M [HCl] = ___________M
The equilibrium constant, K, for the following reaction is 0.186 at 332 K. NH4HS(s) (equilibrium) NH3(g) + H2S(g) An equilibrium mixture in a 16.2 L container at 332 K contains 0.322 mol NH4HS(s), 0.543 M NH3 and 0.343 M H2S. 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 8.20 L? [NH3] = M [H2S] = M
The equilibrium constant, K, for the following reaction is 1.30102 at 589 K. NH CH() =NH3(g) + HCI(g) An equilibrium mixture in a 13.0L container at 589 K contains 0.397 mol NH C18), 0.147 M NH3 and 8.84x102 M HCI. 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 6.66 L? M ho (NH3] = [HCI) M
1) The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.311 M HI, 4.18×10-2 M H2 and 4.18×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.85×10-2 mol of I2(g) is added to the flask? 2) The equilibrium constant, K, for the following reaction is 1.20×10-2 at...
The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.208 mol NH4Cl, 2.26×10-3 M NH3 and 2.26×10-3 M HCl. If the concentration of HCl(g) is suddenly increased to 3.80×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M [HCl] = M
The equilibrium constant, K, for the following reaction is 2.35×10-2 at 517 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 11.3 L container at 517 K contains 0.269 M PCl5, 7.94×10-2 M PCl3 and 7.94×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.27 L? [PCl5] = M [PCl3] = M [Cl2] =...