Consider the following unbalanced reaction: HCl (g) ?H2 (g) + Cl2 (g)
a. If the equilibrium constant of this reaction is Kp = 4.17*10-34, determine the equilibrium constant for H2 (g) + Cl2 (g) ? HCl (g) at 25 oC.
b. If this were an endothermic reaction, how would increasing the temperature alter the equilibrium constant?
c. Given 1.00 atm Cl2, 0.567 atm H2 and 2.50 atm HCl, determine their equilibrium partial pressures at 25 oC
8. Consider the following unbalanced reaction: HCl (g)?H2 (g) +Cl2 (g) a. If the equilibrium constant of this reaction is Kp 4.17"10-34 determine the equilibrium constant for H2 (g) + Cl2 (g) ? HCl (g) at 25 °C b. If this were an endothermic reaction, how would increasing the temperature alter the equilibrium constant? c. Given 1.00 atm Cl2, 0.567 atm H2 and 2.50 atm HCJ, determine their equilibrium partial pressures at 25 °C
PCl5(g) has Kp = 0.0870 at 300 °C. A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2, and 0.20 atm PCl5 at this temperature. (a) Use the reaction quotient to determine the direction the reaction must proceed to reach equilibrium. (b) Calculate the equilibrium partial pressures of the gases. (c) What effect will increasing the volume of the system have on the mole fraction of Cl2 in the equilibrium mixture? (d) The reaction is exothermic. What effect will increasing the temperature of the system have on the mole fraction of Cl2 in the equilibrium mixture?