Assignment 22 Chap 15: Applications of Equilibrium Constants
At 900 K the following reaction has Kp=0.345:
2SO2(g)+O2(g)⇌2SO3(g)
In an equilibrium mixture, the partial pressures of SO2 and O2 are 0.120 atm and 0.440 atm , respectively.
What is the equilibrium partial pressure of SO3 in the mixture?
Assignment 22 Chap 15: Applications of Equilibrium Constants At 900 K the following reaction has Kp=0.345:...
At 900 K the following reaction has Kp=0.345: 2SO2(g)+O2(g)???2SO3(g) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.150atm and 0.465atm , respectively. What is the equilibrium partial pressure of SO3 in the mixture?
QUESTION 10 [CLO-6] At 900 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2502 + O2(g) ==== 2503 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is atm 4.21 x 10-3 6.20 x 10-4 82.0 40.2 192
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =
A reaction vessel contains an equilibrium mixture of SO2, O2,, and SO3. The reaction proceeds such that: 2SO2 (g) + O2 (g) ----> <---- 2SO3 (g) The partial pressures at equilibrium are Pso2=0.001111 atm PO2 = 0.002728 atm PSO3 =0.0166 Calculate the Kp for the reaction.
The equilibrium constant, Kp, for the following reaction is 2.74 at 1.15x103K. 2803(g) 22502(g) + O2(g) + If an equilibrium mixture of the three gases in a 10.9 L container at 1.15*10²K contains SO3 at a pressure of 1.77 atm and SO2 at a pressure of 0.926 atm, the equilibrium partial pressure of O2 is atm.
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...
1- 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 products when 0.395 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M 2- student ran the following reaction in the laboratory at 1090 K: 2SO3(g) ----------> 2SO2(g) + O2(g) When he introduced SO3(g) at a pressure of 1.05 atm into a 1.00...
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2and O2to form SO3is 0.365 at 1.15×103K: 2 SO2( g ) + O2( g ) --> 2 SO3( g ) A sample of SO3is introduced into an evacuated container at 1150 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.879atm. Calculate the equilibrium partial pressures of SO2and O2in the container.
If the equilibrium constant for reaction X is K. What is the equilibrium constant for reaction Y is? Reaction X: SO2 (g) + (1/2) O2 (g) ⇌ SO3 (g) Reaction Y: 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) a. 2K b. K2 c. 1/K2 d. 0.5 x K e. -K2
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1270 K? Kp =