One step in the manufacture of sulfuric acid is the oxidation of sulfur dioxide to sulfur trioxide. Consider performing this oxidation at a pressure of 1 bar with an excess of 100 mole % oxygen, using air as the oxygen source. For the optimal yield of SO3, it is desirable to maintain the reactor at a constant temperature of 700°C. You may assume ∆hrxn° is independent of temperature. What is the effect of increasing the pressure on the extent of reaction?
One step in the manufacture of sulfuric acid is the oxidation of sulfur dioxide to sulfur...
Sulfur trioxide is made from the oxidation of sulfur dioxide. 2 SO2 + O2 --> 2 SO3. A 16 g sample of SO2, reacted with excess oxygen, gives 18 g SO3. What is the percent yield?
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)
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 25.0L tank with 8.8 mol of sulfur dioxide gas and 2.4 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 0.48 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the...
Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2SO2(g)+O2(g)→2SO3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide has the following composition: Calculate the value of the equilibrium constant Kp for this reaction. Round your answer to 2 significant digits. compound pressure at equilibrium SO2 58.3 atm 02 84.7 atm SO3 66.3 atm
Suifur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fils a 125. L tank with 7.4 mol of sulfur dioxide gas and 56. mol of oxygen gas at 38. °C. He then raises the temperature, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 1.5 mol. Calculate the concentration equilibrium constant for the reaction of sulfur...
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...
Sulfur trioxide is formed from sulfur dioxide and oxygen according to the reaction formula 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) with the equilibrium constant 2.5 × 1010 at the temperature 5.0 × 102 K. A reaction vessel with a volume of 0.25 L contains from start 0.030 moles of SO2 (g) and 0.050 moles of O2 (g). a) Calculate the partial pressure SO3 (g) after equilibrium is reached at 5.0 × 102 K. b) Will more...
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 50, (g) + O2(g) 250, (g) The standard enthalpies of formation for SO2(g) and SO2(g) are AH (SO2(g)] = –296.8 kJ/mol AH (SO2(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 1.09 L of So, (g) is converted to 1.09 L of So, (g) according to this process at a constant pressure...
3.24 mol of surfer dioxide reacts with an excess of oxygen gas to phone sulfur trioxide assuming the reaction occurs as a temperature of 300 K and a pressure of 2.50 ATM what volume of sulfur trioxide want your list in L Table of Contents > Test 3 > Module 8 > After Class: Knewton HW and quiz > 8.4 Gas Laws: Ideal Gas Laws 18.4 Gas Laws: Ideal Gas Laws ---- Consider the reaction represented by the following chemical...
please help me solving this step by step... thank you :) 8.25 Sulfur dioxide is converted to sulfur trioxide by oxidation over a V20, catalyst at atmospheric pressure. In the reactor configuration shown in Figure P8.25, SO2 and O2 avalable at 300°C and 25°C, respectively, are preheated to 425°C and fed in stoichiometric ratio to the reactor. Conversion is 96% and, to keep the reactor temperature from rising too much, 10 kcal/g-mol of com bined feed is removed by external...