Enter your answer in the provided box. The formation of SO3 from SO2 and O2 is...
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 71.0% yield of SO3?
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Enter your answer in the provided box. The formation of SO3 from
SO2 and O2 is...
One step in the manufacture of sulfuric acid is the oxidation of SO2 gas to SO3:...
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)
. One mole of SO2 gas and 1.00 mol of O2 gas were confined at 1000...
. One mole of SO2 gas and 1.00 mol of O2 gas were confined at 1000 K in a 5.00 L flask. The gases reacted, and at equilibrium, 0.840 mol of SO3 gas had formed. Calculate the value of Kc and Kp. 2SO2 (g) + O2 (g) ↔ 2SO3 (g)
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...
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)
A reaction vessel contains an equilibrium mixture of SO2, O2,, and SO3. The reaction proceeds such...
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.
A) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g)...
a) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g): 2. 2SO2(g) O2(g)SO3(g) dGo, ΔΗο, and ASo values for the reaction are-141 .6kJ/mol,-1984kJ/mol and -187.9J/Kmol, respectively. Evaluate whether or not the reaction is spontaneous under standard conditions at 298K, predict the effect of increasing temperature on spontaneity and calculate the value of T at which the reaction becomes nonspontaneous. b) The reaction described in part (a) is too slow at room temperature to...
Enter your answer in the provided box. When coal is burned, the sulfur present in coal...
Enter your answer in the provided box. When coal is burned, the sulfur present in coal is converted to sulfur dioxide (SO2), which is responsible for the acid rain phenomenon: Ss) + O2(g) → SO2(9) If 3.15 kg of S reacts with oxygen, calculate the volume of So, gas (in mL) formed at 30.5°C and 1.04 atm.
Enter your answer in the provided box. The SO2 present in air is mainly responsible for...
Enter your answer in the provided box. The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 58O2 + 2MnO4 + 2H20 - 55042- + 2Mn2+ + 4H Calculate the number of grams of So, in a sample of air if 3.50 mL of 0.00700 M KMnO4 solution are required for the titration.
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at...
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at 625 oC What is Kc at this temperature? Kp = Kc[RT]Δn R = 0.08206 L-atm/mol K
2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625...
2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = Kc[RT]An R = 0.08206 L-atm/mol K
a. The oxidation of SO2(g): 2SO2(g) + O2(g) → 2SO3(g) is too slow at 298 K...
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...
a) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g): 2. 2SO2(g) O2(g)SO3(g) dGo, ΔΗο, and ASo values for the reaction are-141 .6kJ/mol,-1984kJ/mol and -187.9J/Kmol, respectively. Evaluate whether or not the reaction is spontaneous under standard conditions at 298K, predict the effect of increasing temperature on spontaneity and calculate the value of T at which the reaction becomes nonspontaneous. b) The reaction described in part (a) is too slow at room temperature to...
Enter your answer in the provided box. When coal is burned, the sulfur present in coal is converted to sulfur dioxide (SO2), which is responsible for the acid rain phenomenon: Ss) + O2(g) → SO2(9) If 3.15 kg of S reacts with oxygen, calculate the volume of So, gas (in mL) formed at 30.5°C and 1.04 atm.
Enter your answer in the provided box. The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 58O2 + 2MnO4 + 2H20 - 55042- + 2Mn2+ + 4H Calculate the number of grams of So, in a sample of air if 3.50 mL of 0.00700 M KMnO4 solution are required for the titration.
2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = Kc[RT]An R = 0.08206 L-atm/mol K
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