A chemist does a reaction in which H and I react to form J The chemist used solutions that were 0.40M H and 0.25M I The chemist made a mixture of 25.0mL of 0.40M H, 20.0mL of 0.25M I, and 55.0mL H2O (such that the final volume is 100.0mL). After the solution reaches its equilibrium, the chemist determined that the solution contains 0.035M J. What is the equilibrium constant (Ke) of the reaction?

Consider the following reaction: 2NOBr(g) 2NO(g) + Br₂ (9) for this question. If 0.340 moles of NOBr(g), 0.327 moles of NO, and 0.499 moles of Br₂ are at equilibrium in a 12.3 L container at 445 K, the value of the equilibrium constant, Ke, is

Solid magnesium fluoride and solid magnesium carbonate are in equilibrium with a solution containing 7.82x103 M potassium carbonate. Calculate the concentration of fluoride ion present in this solution. [fluoride] = M

Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 75 L tank with 31. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 12. mol of nitrogen dioxide gas. The engineer then adds another 10. mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 Х G