The equilibrium constant Kc for the reaction: PCl3(g) + Cl2(g) PCl5(g) is 490 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?
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The equilibrium constant Kc for the reaction: PCl3(g) + Cl2(g) PCl5(g) is 490 at 230°C. If...
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 0.249 moles of PCl3 and 0.249 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 1.80×10-2 at 698 K. 2HI(g) = H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and...
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 0.504 moles of PCl3 and 0.504 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 0.366 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
1. The equilibrium constant, Kc, for the reaction PC13(g) + Cl2(g) = Pcl3(g) equals 49 at 230°C. If 0.400 mol each of phosphorus trichloride and chlorine are added to a 4.0-L reaction vessel, what is the equilibrium composition of the mixture at 230°C?
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500K. PCl5(g) to PCl3(g) + Cl2(g) If an equilibrium mixture of the three gases in a 15.2 L container at 500K contains 0.214 mol of PCl5(g) and 0.202 mol of PCl3, the equilibrium concentration of Cl2 is ___M.
For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 2.0 × 101 at 240°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl3(g) is 0.27 M, what is the equilibrium concentration of PCl5(g)?
9b. 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 0.560 moles of PCl3 and 0.560 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = M [Cl2] = M [PCl5] = M
For the reaction, PCl5 (g) <--> PCl3 (g) + Cl2 (g), Kc=33.3 at 760.0 C. In a container at equilibrium, there are 1.29 x 10-3 mol/L of PCl5 and 1.87 x 10-1 mol/L of Cl2. Calculate the [PCl3] in the container.
Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react. PCl3(g) + Cl2(g) ⇌ PCl5(g) The equilibrium constant for the reaction is KC = 38.0 at 233 °C. If 0.510 mol of phosphorus trichloride is added to 0.238 mol of chlorine in a 1.11-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride? Report your answer to THREE significant figures.