Suppose a 500. mL flask is filled with 1.3 mol of NO3 and 1.8 mol of NO₂. The following reaction becomes possible: NO₂(g) + NO(g) → 2NO₂(g) The equilibrium constant K for this reaction is 0.690 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. M X

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Chapter14: Chemical Equilibirum
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Problem 14.19QP: During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction...
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Suppose a 500. mL flask is filled with 1.3 mol of NO3 and 1.8 mol of NO₂. The following reaction becomes possible:
NO₂(g) + NO(g) 2NO₂(g)
The equilibrium constant K for this reaction is 0.690 at the temperature of the flask.
Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.3 mol of NO3 and 1.8 mol of NO₂. The following reaction becomes possible: NO₂(g) + NO(g) 2NO₂(g) The equilibrium constant K for this reaction is 0.690 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
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