A) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g)...
One step in the manufacture of sulfuric acid is the oxidation of SO2 gas to SO3: 2SO2 (g) + O2 (g) 2SO3 (g) ΔH = ‒196 kJ mol–1 This reaction is usually performed at 698 K and 1-2 atmospheres of pressure. 2. Use Le Chatelier’s principle to explain why decreasing the temperature of the reaction vessel to 298 K should theoretically increase the yield of SO3 (g)
a. The oxidation of SO2(g): 2SO2(g) + O2(g) → 2SO3(g) is too slow at 298 K to be useful in the manufacture of sulfuric acid. To overcome this low rate, the process is conducted at an elevated temperature. i. Calculate K, the equilibrium constant, at 298 K and at 973 K. ∆G298o = -141.6 kJmol-1 for the reaction as written; (3) ii. Calculate K using ∆Ho and ∆So values at 973 K, ∆G973o = -12.12 kJmol-1 for the reaction as...
Enter your answer in the provided box. The formation of SO3 from SO2 and O2 is an intermediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. The equilibrium constant KP for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 0.13 at 803°C. In one experiment, 2.00 mol SO2 and 2.00 mol O2 were initially present in a flask. What must be the total pressure at equilibrium in order to have an...
An engineer examining the oxidation of SO2 in the production of sulfuric acid determines that Kc = 1.7 × 108 at 600 K: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) At equilibrium, the partial pressure of SO3 = 200 atm and the partial pressure of O2 = 160 atm. Calculate the partial pressure of SO2.
SO3(g) decomposes to produce SO2(g) and O2(g), as represented by 2SO3(g)⇄2SO2(g)+O2(g) ΔH°=180kJ/molrxn Under what temperature conditions will the reaction be thermodynamically favored: high temperatures, low temperatures, all temperatures, or no temperatures? Justify your answer in terms of the change in enthalpy and the change in entropy during the reaction.
A 2.0 L flask is filled with 0.30 mol SO3 , 0.40 mol of SO2 and 0.50 mol of O2 and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.34. Predict the effect on the concentration of SO3 as the equilibrium is achieved by using Q, the reaction quotient. 2SO3(g) —> 2SO2(g) + O2(g)
5) For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), if initially P(SO2) = 1.2 atm, P(O2) = 1.8 atm, and P(SO3) = 2.1 atm, calculate AG for this reaction at 25°C. The following data is valid at 25°C: AG° (kJ/mol) SO 300.4 SO3 370.4 A) -140.0 kJ/mol B)-141.3 kJ/mol C)-138.7 kJ/mol D) 1,174.7 kJ/mol E) -137.6 kJ/mol
A reaction vessel contains an equilibrium mixture of SO2, O2,, and SO3. The reaction proceeds such that: 2SO2 (g) + O2 (g) ----> <---- 2SO3 (g) The partial pressures at equilibrium are Pso2=0.001111 atm PO2 = 0.002728 atm PSO3 =0.0166 Calculate the Kp for the reaction.
2 SO2 (g) + O2 (g) = 2 SO3 (g) + Energy Predict the effect of each of the following changes on the number of moles of S03 present in the mixture at equilibrium Decreasing the volume of the system Adding oxygen to the equilibrium mixture Raising the temperature of the system Decreasing the pressure of the system Adding a catalyst 2 SO2 (g) + O2 (g) = 2 SO3 (g) + Energy Predict the effect of each of the...
SO2(g) + 0.5 O2(g) -> SO3(9) a) What quantity of heat is needed to raise 7219 mol of SO2(g) and a stoichiometric quantity of O2(g) in the rigid reaction tank from 25°C to the reaction temperature of 400°C?