Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of nitrogen monoxide. [N2] [02] 2NO(g) ? N2(g) + O2(g) K = = 2.78×10-2 at 287 K [NO]² A flask originally contains 0.378 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = = [N2] [02] = Σ Σ Σ M Check & Submit Answer Show Approach

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Use K and initial concentrations to calculate equilibrium concentrations.
Consider the equilibrium system involving the decomposition of nitrogen monoxide.
[N2] [02]
2NO(g)
?
N2(g) + O2(g)
K =
=
2.78×10-2 at 287 K
[NO]²
A flask originally contains 0.378 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases.
[NO] =
=
[N2]
[02]
=
Σ Σ Σ
M
Check & Submit Answer
Show Approach
Transcribed Image Text:Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of nitrogen monoxide. [N2] [02] 2NO(g) ? N2(g) + O2(g) K = = 2.78×10-2 at 287 K [NO]² A flask originally contains 0.378 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = = [N2] [02] = Σ Σ Σ M Check & Submit Answer Show Approach
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