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For the following reaction at equilibrium
2NOCl (g) = 2NO(g) + Cl2(g)
K = 1.6 x 10-5 M. 1.00 mole of NOCl and 1.00 mole of Cl2 are placedin a 1.00 L container. Calculate the equilibrium concentration ofNO(g).
A 0.50 M
B 6.2 x 10-4 M
C 1.6 x 10-5 M
D 1. 0 M
E 4.0 x 10-3 M

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At 35 C, K = 1.6 × 10-5 for the reaction

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Calculate the concentrations of all species at equilibrium, if 2.0 mol NOCl and 1.0 mol Cl2 are placed in a 1.0 L flask

lavenderalligator149

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At 298 K, the equilibrium constant,

KC, equals 0.12. What is the equilibrium concentration of

HCl, if the initial concentrations of methane and chlorine wereboth [CH4] = [Cl2] = 0.50 M.

CH4(g) + Cl2(g) <---->

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For the following reaction at equilibrium
2NOCl (g) = 2NO(g) + Cl2(g)
K = 1.6 x 10-5 M. 1.00 mole of NOCl and 1.00 mole of Cl2 are placedin a 1.00 L container. Calculate the equilibrium concentration ofNO(g).
A 0.50 M
B 6.2 x 10-4 M
C 1.6 x 10-5 M
D 1. 0 M
E 4.0 x 10-3 M

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For the following reaction at equilibrium2NOCl (g) = 2NO(g) + Cl2(g)K = 1.6 x 10-5 M. 1.00 mole of NOCl and 1.00 mole of Cl2 are placedin a 1.00 L container. Calculate the equilibrium concentration ofNO(g).A 0.50 MB 6.2 x 10-4 MC 1.6 x 10-5 MD 1. 0 ME 4.0 x 10-3 M

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard

For the following reaction at equilibrium
2NOCl (g) = 2NO(g) + Cl2(g)
K = 1.6 x 10-5 M. 1.00 mole of NOCl and 1.00 mole of Cl2 are placedin a 1.00 L container. Calculate the equilibrium concentration ofNO(g).
A 0.50 M
B 6.2 x 10-4 M
C 1.6 x 10-5 M
D 1. 0 M
E 4.0 x 10-3 M