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Consider the following equilibria: SO2(g) + 1/2O2(g) = SO3(g) NO3(g) = NO2(g) + ½/2O2(g) Kej = 2.1 x 10-³ Ke₂ = 3.7 x 10-² SO₂(g) + NO3(g) = SO3(g) + NO2(g). Calculate the equilibrium constant for the reaction: a) 7.8 x 10-5 b) 3.9 x 10² c) 1.6 x 10-4 d) 1.3 x 10³

Consider the following equilibria: SO2(g) + 1/2O2(g) = SO3(g) NO3(g) = NO2(g) + ½/2O2(g) Kej = 2.1 x 10-³ Ke₂ = 3.7 x 10-² SO₂(g) + NO3(g) = SO3(g) + NO2(g). Calculate the equilibrium constant for the reaction: a) 7.8 x 10-5 b) 3.9 x 10² c) 1.6 x 10-4 d) 1.3 x 10³

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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7. Consider the following equilibria: SO2(g) + 1/2O2(g) = SO3(g) NO3(g) = NO2(g) + 1/2O2(g) Calculate the equilibrium constant for the reaction: a) 7.8 x 10-5 b) 3.9 x 10² c) 1.6 x 104 d) 1.3 x 10³ e) None of the above 3 Ke₁ = 2.1 x 10-³ Ke₂ = 3.7 x 10-² SO2(g) + NO3(g) = SO3(g) + NO2(g).
Transcribed Image Text:7. Consider the following equilibria: SO2(g) + 1/2O2(g) = SO3(g) NO3(g) = NO2(g) + 1/2O2(g) Calculate the equilibrium constant for the reaction: a) 7.8 x 10-5 b) 3.9 x 10² c) 1.6 x 104 d) 1.3 x 10³ e) None of the above 3 Ke₁ = 2.1 x 10-³ Ke₂ = 3.7 x 10-² SO2(g) + NO3(g) = SO3(g) + NO2(g).
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Step 1: Explanation

When we add two equilibrium equations then we multiply the equilibrium constant (Kc1) and the equilibrium constant(Kc2) to get equilibrium constant for the overall equations.

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