POST) question 12please answer B and show work thank you Consider the following reaction:2SO2(g) + O2(g) = 2SO3(g)KcKcSubmitO Kc ==Part B=Kc =LUJ[0₂] [SO₂]²[0₂] [2SO2][2SO3][2SO3][0₂] [2SO2]Previous AnswersCorrectIn the equilibrium-constant expression, the product concentrations are in the numerator, and the reactant concentrations are in thedenominator. The concentrations are multiplicative, so the coefficients from the balanced chemical equation become exponents forthe respective concentrations.Now, use this expression to calculate the equilibrium constant using the equilibrium concentrations of the reactants and product.What is the numerical value of K for the reaction if the concentrations at equilibrium are [SO₂] = 0.15 M, [O₂] = 0.15 M, and [SO3] = 0.57M?Express your answer using two significant figures.Review | Constants | Periodic TableIVE ΑΣΦ@] ?

Answered: Image /qna-images/answer/b2f1b070-4dba-4bcb-8069-eff826e21c0f.jpg

▾ Part B What is the numerical value of K, for the reaction if the concentrations at equilibrium are [SO₂] = 0.15 M. [0₂] = 0.15 M, and [SO3] = 0.57 M? Express your answer using two significant figures. K₂= ΨΕΙ ΑΣΦ ?

▾ Part B What is the numerical value of K, for the reaction if the concentrations at equilibrium are [SO₂] = 0.15 M. [0₂] = 0.15 M, and [SO3] = 0.57 M? Express your answer using two significant figures. K₂= ΨΕΙ ΑΣΦ ?

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

Section: Chapter Questions

Problem 51QRT: At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 ×...

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Question

POST) question 12

please answer B and show work thank you

Consider the following reaction:
2SO2(g) + O2(g) = 2SO3(g)
Kc
Kc
Submit
O Kc =
=
Part B
=
Kc =
LUJ
[0₂] [SO₂]²
[0₂] [2SO2]
[2SO3]
[2SO3]
[0₂] [2SO2]
Previous Answers
Correct
In the equilibrium-constant expression, the product concentrations are in the numerator, and the reactant concentrations are in the
denominator. The concentrations are multiplicative, so the coefficients from the balanced chemical equation become exponents for
the respective concentrations.
Now, use this expression to calculate the equilibrium constant using the equilibrium concentrations of the reactants and product.
What is the numerical value of K for the reaction if the concentrations at equilibrium are [SO₂] = 0.15 M, [O₂] = 0.15 M, and [SO3] = 0.57
M?
Express your answer using two significant figures.
Review | Constants | Periodic Table
IVE ΑΣΦ
@] ?

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