ampere The reaction, PCls (g) 5 PC13(g) + Cl2(g), has Kc = 4.20 x 102. If...
Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K The reaction is allowed to reach equilibrium in a 15.2-L flask. At equilibrium, [PCIs]-9.75x102 M, [PCl,]-o.156 M and [C12] = 0.156 M. (a) The equilibrium mixture is transferred to a 7.60-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 7.60-L flask. [PCI5] [C12] =
For the equilibrium reaction: PCis(g) = PC13(g) + Cl2(g); Kc = 0.00183 a. Write the concentration equilibrium equation for the reaction. [1 mark] b. If 2.0 gram of PCis(g) is introduced into a 1.5 L flask what will be the equilibrium concentrations of PCls, PC13 and Cl2? [4marks]
Phosphorus pentachloride decomposes according to the chemical equation PC15(g) PC13(g) + Cl2 (g) Kc = 1.80 at 250° C A 0.475 mol sample of PCI, (g) is injected into an empty 4.90 L reaction vessel held at 250° C. Calculate the concentrations of PCI, (g) and PCI,(g) at equilibrium. [PCls] [PCl3]
Part B please
For the equilibrium reaction: PCI (g) =PC13(g) + Cl2(g); Kc = 0.00183 a. Write the concentration equilibrium equation for the reaction. [1 mark] b. If 2.0 gram of PCis(g) is introduced into a 1.5 L flask what will be the equilibrium concentrations of PCls, PClz and Cl ? [4marks]
Consider the reaction. PCl5(g)−⇀↽−PCl3(g)+Cl2(g)Kc=0.0420 The concentrations of the products at equilibrium are [PCl3]=0.180 M and [Cl2]=0.280 M. What is the concentration of the reactant, PCl5, at equilibrium?
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, 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
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) <---> PCl3(g) + Cl2(g) Kc= 1.80 at 250°C A 0.314 mol sample of PCl5(g) is injected into an empty 3.45 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. [PCl5]= ? M [PCl3]= ? M
The equilibrium constant, Kc, for the reaction below is 1.50. 2.00 mol of Cl2 are combined with 2.00 mol of PCl3 in a 1.00 L flask. What mass of PCl3 is present at equilibrium? (MW of PCl3 = 137.5 g/mol) PCl3 (1) + Cl2 (g) ⇌ PCl5 (g)