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2:12 AM Tue Dec 3 18% c30_m7_105_assignment 2 Done Lesson 5: Equilibrium Calculation 1. When acetic acid reacts with water, these equilibrium concentrations are found. [CH, COOH] = 0.20mol/L, [CH, COO ] = 0.0019mol/L, [H,O'] = 0.0019mol/L. The equation for the reaction is CH, COOH (aq) + H,O (0) - CH COO (aq) + HO (aq) What is the equilibrium constant expression for this reaction and what is the value of the equilibrium constant? (3 marks) Answer2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done NO, (8) - NO, (8) + _NO(g) K = 1.0 x 10 If 0.050 mol/L of NO, (g) exists at equilibrium, what is the concentration of N,O, (g) at equilibrium, assuming the reaction began with no products present?? (3 marks) Answer 3. Write the equilibrium expression and calculate the K for H, (g) + CS, (g) - CH (g) + 2 H,S (g) Concentrations at equilibrium: [CH ] = [H,S] = 1.3 x 10* mol/L [H,] = 4.4 x 10" mol/L [CS,] = 1.1 x 10 mol/L2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done 4. Calculate the [NO,] for 2 NO (g) + 0, (8) - NO, (8) If [NO] = 4.00 x 10" mol/L and [O,] = 2.00 x 10" mol/L at equilibrium, and the equilibrium constant is 2.34 x 10" at 500 C. (3 marks) Answer2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done ICE Table 5. 1.0 mole of hydrogen gas and 1.0 mole of fluorine gas are sealed in a 1.0 L flask and allowed to react at 450 C. At equilibrium 1.56 moles of hydrogen fluoride gas are present. Calculate the K for the reaction. H, (8) + F, (g) - 2HF (g) Answer (4 marks) H2 (8 )+ F2 (8)f 2HF (8) H2(g) mol/L F2(g) mol/L HF(g) mol/L - C F2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done 6. At certain temperatures, a mixture of hydrogen gas and chlorine gas was prepared by placing 0.200 moles of hydrogen gas and 0.200 moles of chlorine gas into a 2.00 L flask. After a period of time the equilibrium was established. 2HCL (g) - H, (g) + Ce, (8) It was determined that, at equilibrium, the chlorine gas concentration had dropped to 0.020 mol/L. What is K for this reaction? Answer (4 marks) H2 (g )+ Cl2 (8)f 2HCI(g) H2mol/L C12(g) mol/L HCI(g) mol/L C F2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done 7. Calculate the concentration of product gases at equilibrium when 0.240 mol/L COF, (g) decomposes into carbon monoxide and fluorine gas. The K for this reaction is 1.60 X 10". COF, (g) = CO (8) + F, (g) Answer (4 marks) COF2 (8) f co(g) + F2 (8) COF2(g)mol/L|CO(g) mol/L F2(g) mol/L2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done 8. Given the reaction below, what was the initial mass of HI (g) placed in a sealed 1.50 L flask which resulted in 0.025 mol of each of H, (g) and I, (g) being found in the flask at equilibrium? H2 (9) + 12 (9) - 2 HI (9) K = 50.5 Answer (4 marks) H2 (8 )+ 12(8)f 2 HI(8) K = 50.5 HI(g)mol/L H2(g) mol/L 12(g) mol/L C E2:18 AM Tue Dec 3 17% c30_m7_105_assignment 2 Done 9. If 0.100 mol/L of CO, (g) and H, (g) are injected into a sealed system, what are the concentrations of H, (g) and HO (g) at equilibrium given that K = 0.64 at 900K? CO, (g)+ H, (g) - CO (g) + HO (g) Answer (4 marks) CO2 (g )+ H2(g) f co(g)+ H20(8) CO2(g)mol/L H2(g)mol/L CO(g)mol/L H20(g)mol/L C