The equilibrium constant for the following reaction is 1.42×10-3 at 179 °C.
Calculate the equilibrium constant for the following reactions
at 179 °C.
(a) PCl3(g)
+ Cl2(g)<-->
PCl5(g) K =
(b) 2
PCl5(g)<-->2
PCl3(g) + 2 Cl2(g)
K =
The equilibrium constant for the following reaction is 1.42×10-3 at 179 °C. PCl5(g)<-->PCl3(g) + Cl2(g) K...
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] =...
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The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.366 moles of PCl3 and 0.366 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = ____M [Cl2] = _____M [PCl5] = ____M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) ⇌ PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.253 moles of PCl3 and 0.253 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = ___ M [Cl2] = ___ M [PCl5] = ___M
The equilibrium constant, K, for the following reaction is 3.78×10-2 at 530 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 5.47 L container at 530 K contains 0.295 M PCl5, 0.106 M PCl3 and 0.106 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 12.1 L? [PCl5] = M [PCl3] = M [Cl2] = M please help me!...