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b) In another experiment, the following equilibrium was established: 2 NO(g) + Cl₂(g) = 2 NOCI(g) 2.6 moles of NO(g) and 1.8 moles of Cl₂(g) were put in a sealed container and allowed to reach equilibrium. At equilibrium, there were 1.8 moles of NO(g) and the total pressure was 125 kPa. By constructing an ICE table (or other method) to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units.

b) In another experiment, the following equilibrium was established: 2 NO(g) + Cl₂(g) = 2 NOCI(g) 2.6 moles of NO(g) and 1.8 moles of Cl₂(g) were put in a sealed container and allowed to reach equilibrium. At equilibrium, there were 1.8 moles of NO(g) and the total pressure was 125 kPa. By constructing an ICE table (or other method) to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section12.2: The Equilibrium Constant
Problem 12.3CE: After a mixture of cis-2-butene and trans-2-butene has reached equilibrium at 600 K, where Kc =...
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Could you help me answer "part b" of this question please. Thank You 

Question 2 a) In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6 H₂O(g) State and explain the effect of an increase in pressure on the equilibrium position. State and explain the effect of an increase in temperature on this equilibrium position. i) ii) b) In another experiment, the following equilibrium was established: 2 NO(g) + Cl₂(g) = 2 NOCI(g) 2.6 moles of NO(g) and 1.8 moles of Cl₂(g) were put in a sealed container and allowed to reach equilibrium. At equilibrium, there were 1.8 moles of NO(g) and the total pressure was 125 kPa. By constructing an ICE table (or other method) to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units.
Transcribed Image Text:Question 2 a) In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6 H₂O(g) State and explain the effect of an increase in pressure on the equilibrium position. State and explain the effect of an increase in temperature on this equilibrium position. i) ii) b) In another experiment, the following equilibrium was established: 2 NO(g) + Cl₂(g) = 2 NOCI(g) 2.6 moles of NO(g) and 1.8 moles of Cl₂(g) were put in a sealed container and allowed to reach equilibrium. At equilibrium, there were 1.8 moles of NO(g) and the total pressure was 125 kPa. By constructing an ICE table (or other method) to find mole fractions and partial pressures at equilibrium, determine the equilibrium constant Kp for this reaction and give its units.
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