Consider the following equilibrium: 2NOCI(g) 2NO(g) + Ch(g) with K = 1.6 × 10 1.00 mole of pure NOC1 and 0.981 mole of pure Cl are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g). Select one: O a. 9.81 × 10-!M O b. 1.02 M O c.4.04 x 10³M O d. 2.02 x 103 M O e.5.71 x 10 M search
Consider the following equilibrium: 2NOCI(g) 2NO(g) + Ch(g) with K = 1.6 × 10 1.00 mole of pure NOC1 and 0.981 mole of pure Cl are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g). Select one: O a. 9.81 × 10-!M O b. 1.02 M O c.4.04 x 10³M O d. 2.02 x 103 M O e.5.71 x 10 M search
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 13QAP: Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant...
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Step 1
For the equilibrium Reaction -
2NOCl <-----> 2NO + Cl2
The , Equilibrium constant can be written as -
Kc = concentration of Products/concentration of Reactants
Kc = [NO]2[Cl2]/[NOCl]2
Here,
Kc = 1.6×10-5
[NO] = moles of NO = ?
[Cl2] = moles of Cl2 = 0.981 mole
[NOCl] = moles of NOCl = 1 mole
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