At a particular temperature, K = 4.9 × 10- 2NO2(g) → 2NO(g) + O₂(g) In an experiment in which 1.0 mol of NO2 is placed in a 4.0-L vessel, what are the equilibrium concentrations of all gases? [NO₂] = 0.25 M [NO] = 4.94x10^-5 M [0₂] = 2.47x10^-5 M for the following balanced reaction:

At a particular temperature, K = 4.9 × 10- 2NO2(g) → 2NO(g) + O₂(g) In an experiment in which 1.0 mol of NO2 is placed in a 4.0-L vessel, what are the equilibrium concentrations of all gases? [NO₂] = 0.25 M [NO] = 4.94x10^-5 M [0₂] = 2.47x10^-5 M for the following balanced reaction:

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 60QRT

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can u help me somethings wrong with the answer

At a particular temperature, K = 4.9 × 10-7 for the following balanced reaction:
2NO₂(g) → 2NO(g) + O₂(g)
In an experiment in which 1.0 mol of NO2 is placed in a 4.0-L vessel, what are the
equilibrium concentrations of all gases?
[NO₂] = 0.25
M
[NO] = 4.94x10^-5 M
[0₂] = 2.47x10^-5 M
An error has been detected in your answer. Check for typos,
miscalculations etc. before submitting your answer.
Submit Answer
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