Reaction: PCl5 D PCl3 + Cl2 Kc = 0.47
2.5 moles of PCl5 are placed in a 5.0 L flask and allowed to come to...
If 0.696 mol PCl5 is placed in a
1.78 L flask and allowed to reach equilibrium at a
given temperature, what is the final concentration of
Cl2 in the flask?
PCl5(g) PCl3(aq)
+ Cl2(g)
Kc = 0.47
a. 0.429 M
b. 0.243 M
c. 0.254 M
d. 0.275 M
e. 0.724 M
1.Initially, 0.64 mol of PCl5 is placed in a 1.0 L flask. At equilibrium, there is 0.12 mol of PCl3 in the flask. What is the equilibrium concentration of PCl5? 2.What is the equilibrium concentration of Cl2? 3.What is the numerical value of the equilibrium constant, Kc, for the reaction?
Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5(g)↽−−⇀PCl3(g)+Cl2(g) A 13.5 g13.5 g sample of PCl5PCl5 is added to a sealed 1.50 L1.50 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 34.8%34.8% of the PCl5PCl5 remains. What is the equilibrium constant, ?cKc , for the reaction? ?c=Kc=
Consider the following reaction: PCl5(g)⇌PCl3(g)+Cl2(g) a. Initially, 0.62 mol of PCl5 is placed in a 1.0 L flask. At equilibrium, there is 0.20 mol of PCl3 in the flask. What is the equilibrium concentration of PCl5? Express your answer to two significant figures and include the appropriate units. b. What is the equilibrium concentration of Cl2? Express your answer to two significant figures and include the appropriate units. c. What is the numerical value of the equilibrium constant, Kc, for...
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)?
Consider the following equilibrium system: PCl5(g) -->PCl3(g) + Cl2(g) A 10.00 L evacuated flask is filled with 0.4334 mol PCl5(g) at 297.3 K. The temperature is then raised to 510.0 K, where the decomposition of PCl5 gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 2.665 atm. What is the value of the equilbrium constant in terms of concentrations, Kc, at 510.0 K?
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.287 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [ PCl5] = M [PCl3] = M [Cl2] = M
When 1.000 mol of PCl5 is introduced into a 5.000 L container at 500 K, 78.50 % of the PCl5dissociates to give an equilibrium mixture of PCl5, PCl3, and Cl2: PCl5(g)⇌PCl3(g)+Cl2(g) Part A Calculate the values of Kc and Kp. Part B KP = Part C If the initial concentrations in a particular mixture of reactants and products are = 0.504 , = 0.129 , and = 0.594 , in which direction does the reaction proceed to reach equilibrium? In the direction of formation of PCl3...
An analysis of a chemical reaction system at 340 °C shows that PCl5, PCl3, and Cl2 are present at equal concentrations of 0.120 mol/L. Determine the equilibrium concentrations (in M) of PCl5, PCl3 and Cl2 at 340 °C, given that Kc = 0.800. Show all calculations and report your answer to the correct number of sig figs. PCl5(g) ⟺ PCl3(g) + Cl2(g)
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)