For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35...
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2 HCl(g), the
equilibrium constant K at 800oC is 4.35 x
104. |
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Homework Answers
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For the reaction H2(g) +
Cl2(g) 2 HCl(g), the
equilibrium constant K at 800oC is 4.35...
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35...
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35 x 10^4. Hydrogen at a partial pressure of 0.700 bar and chlorine at a partial pressure of 0.500 bar are placed in a vessel at 800oC and allowed to equilibrate. Find the final partial pressures of all three gases in this reaction in bar
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(g)+Cl2(g)?PCl5(g). A 7.5-L gas...
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas:PCl3(g)+Cl2(g)→PCl5(g).A 7.5-L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.123atm , PCl2 = 0.158atm , and PPCl5 = 1.20atm .Calculate Kc for this reaction at 450 K.
At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) <=> 2BrCl...
At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) <=> 2BrCl (g) is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). What is the equilibrium pressure of Br2? A. 0.86 atm B. The equilibrium partial pressures of Br2 will be the same as the initial value. C. The equilibrium partial pressure of Br2 will be...
The equilibrium constant, K. for the following reaction is 1.80X10-2 at 698 K: 2HI(g) P H2(g)...
The equilibrium constant, K. for the following reaction is 1.80X10-2 at 698 K: 2HI(g) P H2(g) +1,2) Calculate the equilibrium partial pressures of all species when HI(g) is introduced into an evacuated flask at a pressure of 1.83 atm at 698 K PH The equilibrium constant, K, for the following reaction is 1.04x10-2 at 548 K: NHCI() NH3(g) + HCl(g) Calculate the equilibrium partial pressure of HCl when 0.579 moles of NH CI(s) is introduced into a 1.00 L vessel...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.70 atm, are introduced into an evacuated vessel at 600 K. PCO = atm PCl2 = atm PCOCl2 = atm B. The equilibrium constant, Kc, for the following reaction is 2.90×10-2 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) Calculate Kc at this temperature for...
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g)...
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
At 400 K, the equilibrium constant for the reaction Br 2 (g) + Cl 2 (g) 2BrCl...
At 400 K, the equilibrium constant for the reaction Br 2 (g) + Cl 2 (g) 2BrCl (g) is K p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br 2 (g), 1.00 atm of Cl 2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true. The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. The reaction will...
23) At 400 K, the equilibrium constant for the reaction Br2(g) + Cl2 (9) 2BrCl (9)...
23) At 400 K, the equilibrium constant for the reaction Br2(g) + Cl2 (9) 2BrCl (9) is Kp = 70. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) 1.00 atm of Cl2 (g), and 2.00 alm of BrCl (g). Use Q to determine which of the statements below is true. A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br2....
For the reaction PCl5(g) ↔ PCl3(g) + Cl2(g) the value of K = 15.4 at 497.0...
For the reaction PCl5(g) ↔ PCl3(g) + Cl2(g) the value of K = 15.4 at 497.0 K. Calculate the equilibrium partial pressures (in bar) of all species at 497.0 K if the initial pressures were P(PCl5(g)) = 0.700 bar, P(PCl3(g)) = 0.320 bar, and P(Cl2(g)) = 0.000 bar.
The equilibrium constant, Ky, for the following reaction is 55.6 at 698 K: H2(g) +12(g) =2HI(g)...
The equilibrium constant, Ky, for the following reaction is 55.6 at 698 K: H2(g) +12(g) =2HI(g) Calculate the equilibrium partial pressures of all species when H, and 13, each at an intitial partial pressure of 1.24 atm, are introduced into an evacuated vessel at 698 K. atm atm P1 PHI atm
The equilibrium constant, K. for the following reaction is 1.80X10-2 at 698 K: 2HI(g) P H2(g) +1,2) Calculate the equilibrium partial pressures of all species when HI(g) is introduced into an evacuated flask at a pressure of 1.83 atm at 698 K PH The equilibrium constant, K, for the following reaction is 1.04x10-2 at 548 K: NHCI() NH3(g) + HCl(g) Calculate the equilibrium partial pressure of HCl when 0.579 moles of NH CI(s) is introduced into a 1.00 L vessel...
23) At 400 K, the equilibrium constant for the reaction Br2(g) + Cl2 (9) 2BrCl (9) is Kp = 70. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) 1.00 atm of Cl2 (g), and 2.00 alm of BrCl (g). Use Q to determine which of the statements below is true. A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br2....
The equilibrium constant, Ky, for the following reaction is 55.6 at 698 K: H2(g) +12(g) =2HI(g) Calculate the equilibrium partial pressures of all species when H, and 13, each at an intitial partial pressure of 1.24 atm, are introduced into an evacuated vessel at 698 K. atm atm P1 PHI atm
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