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
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Could you help me answer "part b" of this question please. Thank You
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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