7. Ammonia can be synthesized according to the equation: 1/2 N₂(g) + 3/2 H₂(g) → NH3(g). The equilibrium constant is 1.69 x 10-4 at 673 K and AH° is -106.5 kJ mol-¹. Calculate the equilibrium constant at 773 K.

You have two 250 mL beakers placed side by side under a bell jar, each filled with 100. mL of water, one containing 0.100 moles of NaCl, and the other containing 0.100 moles of CaCl2. After some time, equilibrium is established between the two beakers. What are the final volumes in the two beakers? (Assume ideal behavior, and that the sum of the two volumes remains 200. mL.)

1. Given the equilibrium constant values N₂ (g) + ¹/2O₂(g) → N₂O (g) N₂O4 (g) → 2 NO₂ (g) ½ N₂(g) + O₂(g) → NO₂ (g) Kel=2.7 x 10-18 K₂=4.6 x 10-³ K3 = 4.1 x 10⁹ Determine the value of K. for the reaction below: 2 N₂O(g) + 30₂ (g) → 2 N₂O4 (g)

The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋  CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.

Suppose the following reaction is at equilibrium: PCl3 + Cl2 ⇋ PCl5; (a) Are the equilibrium concentrations of PCl3, Cl2, and PCl5 necessarily equal? Explain. (b) Is the equilibrium concentration of PCl3 necessarily equal to that of Cl2? Explain.

3. The reaction of bromine gas with chlorine gas, has a Ke value of 7.20 at 200°C. If a closed 2.50 L vessel were charged with the two reactants, with the former weighing 9.65 g while the latter is 5-70 g, what would be the equilibrium concentration of the two reactants and BrCl(g)? Determine whether the forward or the reverse reaction will be favored. Explain your answer.

Write the equilibrium constant expression for this reaction: 2 CH;COO (aq)+C,H,O2(aq) → C¿H1,Og(aq)+2OH (aq)

Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 25.0 L tank with 8.8 mol of methane gas and 2.8 mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 2.0 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 x10 X

COz (g) + Hz (g) = CO(g)+Hz0(g) Keq = 0.64 If we start with 0.100 mol/L of carbon dioxide and hydrogen gas, what is the equilibrium concentrations of all species?

The following reaction is in equilibrium: NO2 (aq) + H20 (1) = HNO, (aq) + OH (aq). Kh (NO, ) = 2.2 x 1011. which of the following statement is correct if we pump HCI (g) into the above solution? Note that the solution volume stays the same after HCI (g) is pumped into the above solution. O a. The reaction will shift to left to re-establish equilibrium and the pH of the solution will increase. O b. The reaction will shift to right to re-establish equilibrium and the pH of the solution will increase. O C. There is no effect to pump HCI (g) into the solution. O d. The reaction will shift to right to re-establish equilibrium and the pH of the solution will decrease. O e. The reaction will shift to left to re-establish equilibrium and the pH of the solution will decrease.