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]²Keqb.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]²c. 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

According to law of Mass Action, Equilibrium constant is the product of the molar concentrations of…

Answered: b. If gas concentrations are as…

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")

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 38A

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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

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