The reaction 2SO2 (g) + O2 (g) ↔ 2SO3 (g) is exothermic and at equilibrium. Which...
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
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The reaction 2SO2 (g) + O2 (g) ↔ 2SO3 (g) is exothermic and at
equilibrium. Which...
The reaction 2502 (g) + 02 (g) - 2503 (g) is exothermic and at equilibrium. Which...
The reaction 2502 (g) + 02 (g) - 2503 (g) is exothermic and at equilibrium. Which of the following action will shift equilibrium left? Lower environment temperature B Add 02 to the system Add a catalyst to slow down the reaction D Add Ne gas to the equilibrium Increase the volume of the reaction chamber
2SO2 (g) + O2 (g) <---> 2SO3 (g) The reaction is exothermic. How does the equilibrium...
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?
For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes...
For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes that will shift the equilibrium position to the right. (Select all that apply.) Add Ne(g) Add SO2(g) Remove SO3(g) Decrease temperature Add a catalyst Increase temperature Decrease volume
For the equilibrium reaction 2SO2(g) + O2(g) 2SO3(g), delta Hrxn = -198 kJ/mol. Which one of...
For the equilibrium reaction 2SO2(g) + O2(g) 2SO3(g), delta Hrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constent to increases? Decrease the temperature. Add SO2 gas Remove O2 gas Add a catalyst. None of these Consider this reaction at equilibrium If the volume of the system is compressed at constent temperature, what change will occure in the position of the equilibrium?
This equilibrium reaction is exothermic: 2SO2 (g) + O2 (g) <-> 2SO3 (g) (where <-> indicates equilibrium,...
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
1) The reaction below is exothermic 2SO2 (g) + O2(g) = 2803(g) + heat Le Châtelier's...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
Consider this reaction at equilibrium 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−198kJ Which of these changes would cause PSO2 to increase? Decreasing...
Consider this reaction at equilibrium 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−198kJ Which of these changes would cause PSO2 to increase? Decreasing the temperature Increasing the volume of the container Increasing the total pressure Adding O2(g)
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at...
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?
5. Consider the reaction, 2SO2 (g) + O2 (g) 2SO3 (g), at T-525°C with ΔΗ -197 kJ. This reaction has an equilibrium...
5. Consider the reaction, 2SO2 (g) + O2 (g) 2SO3 (g), at T-525°C with ΔΗ -197 kJ. This reaction has an equilibrium constant K = 781 at this temperature, which condition(s) listed below will cause a shift in the reaction equilibrium to RIGHT? I. If Psos -0.400 atm, Pso2-0.050 atm, and P02 0.050 atm II. If at equilibrium, Psos is suddenly decreased by removing SO III. If at equilibrium, the volume of the vessel is decreased IV. If at equilibrium,...
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the...
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)
The reaction 2502 (g) + 02 (g) - 2503 (g) is exothermic and at equilibrium. Which of the following action will shift equilibrium left? Lower environment temperature B Add 02 to the system Add a catalyst to slow down the reaction D Add Ne gas to the equilibrium Increase the volume of the reaction chamber
For the equilibrium reaction 2SO2(g) + O2(g) 2SO3(g), delta Hrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constent to increases? Decrease the temperature. Add SO2 gas Remove O2 gas Add a catalyst. None of these Consider this reaction at equilibrium If the volume of the system is compressed at constent temperature, what change will occure in the position of the equilibrium?
5. Consider the reaction, 2SO2 (g) + O2 (g) 2SO3 (g), at T-525°C with ΔΗ -197 kJ. This reaction has an equilibrium constant K = 781 at this temperature, which condition(s) listed below will cause a shift in the reaction equilibrium to RIGHT? I. If Psos -0.400 atm, Pso2-0.050 atm, and P02 0.050 atm II. If at equilibrium, Psos is suddenly decreased by removing SO III. If at equilibrium, the volume of the vessel is decreased IV. If at equilibrium,...
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