Suppose a 250. mL flask is filled with 0.90 mol of N, and 0.50 mol of NO. The following reaction becomes possible: N2(g) +O,(g) - 2NO(g) The equilibrium constant K for this reaction is 0.212 at the temperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to two decimal places.

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Suppose a 250. mL flask is filled with 0.90 mol of \( \text{N}_2 \) and 0.50 mol of NO. The following reaction becomes possible:

\[
\text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g)
\]

The equilibrium constant \( K \) for this reaction is 0.212 at the temperature of the flask.

Calculate the equilibrium molarity of \( \text{N}_2 \). Round your answer to two decimal places.

[Text box for input] \( \boxed{M} \)

Options: clear (x), submit (↻), help (?)
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.90 mol of \( \text{N}_2 \) and 0.50 mol of NO. The following reaction becomes possible: \[ \text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g) \] The equilibrium constant \( K \) for this reaction is 0.212 at the temperature of the flask. Calculate the equilibrium molarity of \( \text{N}_2 \). Round your answer to two decimal places. [Text box for input] \( \boxed{M} \) Options: clear (x), submit (↻), help (?)
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