Phosphorus pentachloride decomposes according to the chemical equation PCI,(g) = PCl, (g) + Cl,(g) K. = 1.80 at 250 °C A 0.1536 mol sample of PCI,(g) is injected into an empty 2.40 L reaction vessel held at 250 °C. Calculate the concentrations of PCI,(g) and PCI, (g) at equilibrium. [PCI,] = [PCI,] = %3D

A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00 L vessel at 700 K. These substances react according to H2 (g) + Br2 (g) 2HBr (g). At equilibrium, the vessel is found to contain 0.566g of H2. Calculate equilibrium concentrations for H2, Br, and HBr.

The equilibrium constant, K. , for the following reaction is 5.10×10-6 at 548 K. NH,CI(s)NH3(g) + HC(g) If an equilibrium mixture of the three compounds in a 5.06 L container at 54S K contains 3.27 mol of NH,Cl(s) and 0.488 mol of NH3, the number of moles of HCI |moles. present is

The equilibrium constant, K, for the following reaction is 3.92×10-2 at 531 K.PCl5(g) PCl3(g) + Cl2(g)An equilibrium mixture of the three gases in a 7.63 L container at 531 K contains 0.331 M PCl5,   0.114 M PCl3 and 0.114 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 18.0 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M     Submit Answer

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Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.3668 mol sample of PCI, (g) is injected into an empty 4.30 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCI, (g) at equilibrium. [PCl,] = M [PCI,] = M