4.) Consider the following equilibrium: Fe3+(aq) + SCN"(aq) = FESCN2+(aq) Initial concentrations: [Fe3+] = 0.390; [SCN"] = 0.819; [FeSCN2+] = 0 The equilibrium concentration of [FESCN2+]eg = 0.300 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =

Cl3] ² [Hz] ² [A] [AC] Consider the chemical equation and equilibrium constant for the synthesis of ammonia at 25 °C: N₂ (g) + 3 H₂ (g) = 2 NH3 (g) K = 5.6 x 105 Calculate the equilibrium constant for the following reaction at 25 °C: NH3 (g) 1/2 N₂ (g) + 3/2 H₂ (g) K' = ? Kc = [NH3 ]² [₂] [H₂]] Kc- [~₂] ¹/2 [H NH3

C and D

The equilibrium constant for the reaction                         2 KAl(OH)4(aq) + 4 H2SO4(aq)  ⇆ 2 KAl(SO4)2(s) + 8 H2O(l) at room temperature is 84.5. At equilibrium, the concentration of sulfuric acid (H2SO4) is 0.258M. What is the concentration of KAl(OH)4 (in moles/L)?

A student ran the following reaction in the laboratory at 544 K: COC12(g) → CO(g) + Cl₂ (9) When she introduced 0.930 moles of COCl2 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0369 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

At room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold.  HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).

C6-6

4. The formation of glucose from water and carbon dioxide is an extremely important reaction for life to exist. Plants perform this reaction through the process of photosynthesis, creating the base of the food chain. The UNBALANCED equation is: H₂O (9) CO2 (g) C6H12O6 (s) + O2 (g) At a particular temperature the equilibrium concentrations were found to be: [H₂0] = 7.90x10-2M, [CO₂] = 0.930M, [0₂] =2.40x10-³M. a. Balance the equation. b. Write an expression for Kc- c. Calculate the value of Kc for the reaction at equilibrium.

Consider the reaction;  N2(g) + O2(g)⇆ 2 NO(g)  where K = 0.10.      Starting with initial concentrations of [N2] = 0.04 M and [O2] = 0.40 M,      the equilibrium concentration of NO is

Chapter 12 part 1 #12