30. For a reaction: A (g) + B (g) ↔ C (g) + D (s), 6.0 atm of A and 5.0 atm of B are initially added to a container. When equilibrium is reached, there are 4.0 atm of C. What is the Kp for the reaction?
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
1) The Keq for the reaction: A + B ↔ A B is 36 What is the Keq for A B ↔ A + B ? 2) The Keq for the reaction: A+B ↔ ABA+B ↔ AB is 8 What is the Keq for 3 AB↔ 3 A +3 B3 AB↔ 3 A +3 B ? 3)Consider the reaction below. 1.3 mol of A and 7.5 mol of B are added to a 2 L container. At equilibrium, the concentration of...
For the following hypothetical reaction, 2 C(g) ↔ D(g) + E(g) determine what the system will do given P(C) = 1.58 atm, P(D) =0.15 atm, P(E) = 0.050 atm and Kp = 3×10-3.
The equilibrium partial pressures for the reaction Cl2 (g) + PCl3 (g) ↔ PCl5 (g) at 300 K are PCl2 = 0.75 atm, PPCl3 = 0.45 atm, and PPCl5 = 0.73 atm. The value of Kp is __________. A. 0.15 B. 0.048 C. 4.7 D. 2.16
For the reaction 2 A(g) + 3 B(g) ↔ 2 C(g) + 2 D(g), the equilibrium constant at 298 K is 1.409×10-11. If the initial partial pressures of A, and B are 0.500 bar, and 0.718 bar, respectively, determine the partial pressure of D (in bar) once equilibrium has been reached at 298 K.
For the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) Kp = 8210 At 298 K in a 10.0 L vessel, the known equilibrium values are as follows: 0.087 atm of A, 0.22 mol of B, and 10.5 mol of C. What is the equilibrium partial pressure of D?
The reaction below was observed in a 4.0 L flask at 445 oC. H2 (g) + I2 (g) ↔ 2 HI (g) Initially, 0.20 atm of each gas (H2, I2 and HI) was placed in the flask. If the kp = 50.2 atm at 445oC, what is the equilibrium pressure (in atm) of HI (g)?
Consider the reaction below. 4.4 mol of A and 6.0 mol of B are added to a 9 L container. At equilibrium, the concentration of A is 0.23 M. What is the concentration of B at equilibrium? 1 A + 2 B ↔ 4 C
Consider the following reaction at equilibrium, CaCO3(s) ↔ CaO(s) + CO2(g). Which of the following statements are true regarding this equilibrium? Select all that are True. a) If CaO(s) is added from the equilibrium mixture the reaction will remain unchanged. b) If CaO(s) is removed from the equilibrium mixture the reaction will shift to the left. c) If CO2(g) is added to the equilibrium mixture the reaction will shift to the right. d) If CO2(g) is added to the equilibrium...
For the reaction in the previous problem, that is, 2HI(g) ↔ H2(g) + I2(g) Keq = 0.016 Initially a container contains 0.39 M HI and no product. What is the equilibrium concentration of H2?