For the reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) At 650K, Kc = 345 and Kp = 6.47. What is ΔGo ? a) −10.1 kJ b) +31.6 kJ c) −31.6 kJ d) −311 J e) −99.7 J
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
For the reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) At 650K, Kc = 345 and Kp =...
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 1260 K? Kp= ?
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 =
2. [8 Points). The value of Ko for the reaction: 2SO2(g) + O2(g) 2S0ig is 1.2 x 103 at 527 ℃ a) [12 Points]. Write the equilibrium constant (Kp) expression for the reaction. b) what is the value of Kp for: 2SO3(g) 2SO2(g) 021g) ? + c) What is the value of Kp for: 6S02)30)6SOse)? O2(g) # 2SO3(g). + d) Calculate the value of Kc for: 2SO2(g)
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
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?
2SO2 (g) + O2 (g) <---> 2SO3 (g) The reaction is exothermic. How does the equilibrium shift at: a) increase of [O2]? b) decrease of [SO3]? c) increase in pressure? d) increase in the volume of the container? e) increase in temperature? f) addition of catalyst?
Consider the following reaction where Kc = 34.5 at 1150 K: 2SO2(g) + O2(g) =2SO3(g) A reaction mixture was found to contain 4.39x10-2 moles of SO2(g), 4.28x10-2 moles of O2(g) and 4.23x10-2 moles of SO3(), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium SO3(g) must be consumed. 2. In order to reach equilibrium Kc must decrease. 3. In order to reach equilibrium SO2 must be consumed....
The reaction 2SO2 (g) + O2 (g) ↔ 2SO3 (g) is exothermic and at equilibrium. Which of the following action will shift equilibrium left? A Lower environment temperature B Add O2 to the system C Add a catalyst to slow down the reaction D Add Ne gas to the equilibrium E Increase the volume of the reaction chamber
A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g) When she introduced 8.07×10-2 moles of SO2(g) and 7.94×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 5.86×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
This equilibrium reaction is exothermic: 2SO2 (g) + O2 (g) <-> 2SO3 (g) (where <-> indicates equilibrium, or double headed arrows) Le Châtelier's principle predicts that __________ will result in an increase in the number of moles of SO3(g) in the reaction container. A) decreasing the liquid level B) removing some oxygen C) increasing the pressure D) increasing the volume of the container E) decreasing the pressure