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b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq Keq = [1.00 M12 [1.75 M] [2.10 M]² = 0.130 M-¹ (NOTE: "M-¹" is another way to write "1/M")

b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq Keq = [1.00 M12 [1.75 M] [2.10 M]² = 0.130 M-¹ (NOTE: "M-¹" is another way to write "1/M")

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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I need help with number 4 questions part b and show the work step by step?

4. For the reaction below: 2 NO2 (g) + O2 (g) 2 NO3 (g) a. Write the law of mass action (the equilibrium expression for Keq) Keq [NO312 [0₂] [NO₂]² Keq b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq = 0.130 M-¹ (NOTE: "M-¹" is another way to write "1/M") [1.00 M12 [1.75 M ] [2.10 M]² c. Based on the Keq value that you calculated in part b, are the reactants or products predominant (predominant means that there is a greater amount present)? REACTANTS: Keq is much less than 1
Transcribed Image Text:4. For the reaction below: 2 NO2 (g) + O2 (g) 2 NO3 (g) a. Write the law of mass action (the equilibrium expression for Keq) Keq [NO312 [0₂] [NO₂]² Keq b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq = 0.130 M-¹ (NOTE: "M-¹" is another way to write "1/M") [1.00 M12 [1.75 M ] [2.10 M]² c. Based on the Keq value that you calculated in part b, are the reactants or products predominant (predominant means that there is a greater amount present)? REACTANTS: Keq is much less than 1
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