The equilibrium constant, Kc, at 25 °C for the monomer-dimer equilibrium 2CHCO,H=(CH3CO,H)2 has been determined to be 3.2 x 104. Assume that acetic acid is present initially at a concentration of 4.0 x 10 mol/L at 25 °C and that no dimer is present initially. a what percentage of the acetic acid is converted to dimer? Percentage = % b As the temperature increases, in which direction does the equilibrium shift? (Recall that hydrogen-bond formation is an exothermic process.) O Increasing the temperature will shift the equilibrium to the right. Increasing the temperature will shift the equilibrium to the left. No shift will occur.

Kc=?

A 1.00-L flask was filled with 2.14 mol gaseous SO2 and 2.14 mol gaseous NO2 and heated. After equilibrium was reached, it was found that 1.55 mol gaseous NO was present. Assume that the reaction SO2 (g) + NO, (g) = SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. HOW DO WE GET THERE? What are the equilibrium concentrations of SO2, NO2, and SO3? [SO2] = [NO2] = M [SO3] = M

Consider the following equilibria at a given temperature: ½Nalg) + J½O>(g) = NO(g) K= 6.45 x 10°, NO (g) + 1½Brz(g) = NOB((g) K= 1.40 Determine the value of the equilibrium constant for the following reaction at the same temperature: %N(g) + ½Ozlg) + ½Br2(g) = NOBr(g) OA 583 x 107 O B.3.36 x 10-18 OC4.17x 107 OD.6.45 x 10 OE 9.03 x 10

The equilibrium constant for the synthesis of ammonia N2(g) + 3 H2(g) --> 2 NH3(g) has the value K = 3.19 × 10^-4 at  400°C. Calculate the equilibrium partial pressures of N2(g), H2(g), and NH3(g) if the total pressure is 1.00 atm and the H:N atomratio in the system is 3;1. (Hint: Try the approximationthat PN2  and PH2  > PNH3  and see if the resulting equationsare simpliied.)

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N, (g) + 3 H, (g) = 2 NH3 (g) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.

At 454 K, Al,Cl6(g) reacts to form Al;Cl,(g) according to the equation 3 Al,Cl,(g) = 2 Al;Cl,(g) In an experiment at this temperature, the equilibrium par- tial pressure of Al,Cl(g) is 1.00 atm and the equilibrium partial pressure of Al;Cl,(g) is 1.02 × 10-2 atm. Compute the equilibrium constant of the preceding reaction at 454 K.