HF(aq)+H2O(1)→F (aq)+H3O"(aq) At a certain temperature, a chemist finds that a 4.7 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 1.19 g H,O 846. g F 0.440 g H,0* 0.149 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 75 L tank with 22. mol of carbon monoxide gas and 26. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 13.5 mol of carbon monoxide gas, 17.5 mol of water vapor and 8.5 mol of hydrogen gas. The engineer then adds another 7.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. || mol x10

Suppose a 250. mL flask is filled with 1.0 mol of N, and 2.0 mol of NH,. This reaction becomes possible: N2 (g) + 3H,(g) – 2NH, (g) 2NH3 (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 H, NH, initial ? change equilibrium

Suppose a 250. mL flask is filled with 0.20 mol of N2 and 2.0 mol of NO. The following reaction becomes possible: N2(g) + O2(g) = 2NO(g) The equilibrium constant K for this reaction is 0.693 at the temperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to two decimal places. Шм

Suppose a 250. mL flask is filled with 0.60 mol of N, and 0.70 mol of NO. This reaction becomes possible: N2(g) +0,(g) = 2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N, NO initial change equilibrium 미미

Suppose a 250. mL flask is filled with 1.9 mol of O, and 1.5 mol of NO. The following reaction becomes possible: N2 (g) +0,(g) =2NO(g) The equilibrium constant K for this reaction is 8.51 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. OM

At a certain temperature, 0.4811 mol of N2 and 1.781mol of H2 are placed in a 4.00 L container.   N2(g)+3H2(g)↽−−⇀2NH3(g)   At equilibrium, 0.1801 mol of N2 is present. Calculate the equilibrium constant, Kc.

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase         The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled.        (c) The volume of the reaction vessel is reduced by 50%.

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

Suppose a 250. mL flask is filled with 0.10 mol of N, and 1.8 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) == 2NO (g) The equilibrium constant K for this reaction is 0.422 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places. IM ?