O KINETICS AND EQUILIBRIUMCalculating equilibrium composition from an equilibrium constantO3/5Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible:N2(g) +O,(g) – 2NO(g)The equilibrium constant K for this reaction is 5.01 at the temperature of the flask.Calculate the equilibrium molarity of O,. Round your answer to two decimal places.MII O ACIDS AND BASESO 3/5Predicting the qualitative acid-base properties of saltsConsider the following data on some weak acids and weak bases:acidbaseK.K,nameformulanameformula-8hypochlorous acidHCIO3.0 x 10ethylamine C2H5NH, 6.4 × 10hydrocyanic acidHCN4.9 x 10 10methylamine CH;NH, 4.4 × 10™Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next tothe solution that will have the next lowest pH, and so on.solutionpH0.1 M KCIchoose one v0.1 M CH3NH3CIchoose one v0.1 M NaCNchoose one v0.1 M C2H5NH3B.choose one vII

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Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +O,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places.

Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +O,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 62QRT

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