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Question 2 In the second stage of the industrial production of nitric acid, nitrogen monoxide combines with oxygen to produce nitrogen dioxide in a reversible, exothermic reaction: 2 NO(g) + O2(g) = 2 NO2(g) a) State and explain the effect of an increase in pressure on the equilibrium. b) State and explain the effect of a decrease in temperature on the equilibrium. c) An industrial chemist used this reaction to produce a batch of nitrogen dioxide. He mixed 4.8 moles of NO(g) and 2.4 moles of O2(g) in a sealed container at 305K and allowed the reaction to reach equilibrium. At equilibrium, there were 0.8 moles of NO(g) and the total pressure was 225 kPa. By constructing an ICE table to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units. You should show all working in your answer. d) When the system had reached equilibrium, the chemist added more oxygen to the reaction vessel at the same temperature of 305K. Explain the effect of this on the value of Kp [2 marks]

Question 2 In the second stage of the industrial production of nitric acid, nitrogen monoxide combines with oxygen to produce nitrogen dioxide in a reversible, exothermic reaction: 2 NO(g) + O2(g) = 2 NO2(g) a) State and explain the effect of an increase in pressure on the equilibrium. b) State and explain the effect of a decrease in temperature on the equilibrium. c) An industrial chemist used this reaction to produce a batch of nitrogen dioxide. He mixed 4.8 moles of NO(g) and 2.4 moles of O2(g) in a sealed container at 305K and allowed the reaction to reach equilibrium. At equilibrium, there were 0.8 moles of NO(g) and the total pressure was 225 kPa. By constructing an ICE table to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units. You should show all working in your answer. d) When the system had reached equilibrium, the chemist added more oxygen to the reaction vessel at the same temperature of 305K. Explain the effect of this on the value of Kp [2 marks]

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Question 2 In the second stage of the industrial production of nitric acid, nitrogen monoxide combines with oxygen to produce nitrogen dioxide in a reversible, exothermic reaction: 2 NO(g) + O2(g) = 2 NO2(g) a) State and explain the effect of an increase in pressure on the equilibrium. b) State and explain the effect of a decrease in temperature on the equilibrium. c) An industrial chemist used this reaction to produce a batch of nitrogen dioxide. He mixed 4.8 moles of NO(g) and 2.4 moles of O2(g) in a sealed container at 305K and allowed the reaction to reach equilibrium. At equilibrium, there were 0.8 moles of NO(g) and the total pressure was 225 kPa. By constructing an ICE table to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units. You should show all working in your answer. d) When the system had reached equilibrium, the chemist added more oxygen to the reaction vessel at the same temperature of 305K. Explain the effect of this on the value of Kp [2 marks]
Transcribed Image Text:Question 2 In the second stage of the industrial production of nitric acid, nitrogen monoxide combines with oxygen to produce nitrogen dioxide in a reversible, exothermic reaction: 2 NO(g) + O2(g) = 2 NO2(g) a) State and explain the effect of an increase in pressure on the equilibrium. b) State and explain the effect of a decrease in temperature on the equilibrium. c) An industrial chemist used this reaction to produce a batch of nitrogen dioxide. He mixed 4.8 moles of NO(g) and 2.4 moles of O2(g) in a sealed container at 305K and allowed the reaction to reach equilibrium. At equilibrium, there were 0.8 moles of NO(g) and the total pressure was 225 kPa. By constructing an ICE table to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units. You should show all working in your answer. d) When the system had reached equilibrium, the chemist added more oxygen to the reaction vessel at the same temperature of 305K. Explain the effect of this on the value of Kp [2 marks]
Expert Solution
Step 1

The balanced chemical reaction in equilibrium is:

2NO(g) + O2(g) ⇌ 2NO2(g) + Heat(Exothermic); Kp = ?? (To be calculated) 

Number of gaseous moles of the reactant side = 2+1 = 3

Number of gaseous moles of the product side = 2 

 

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