One step in the manufacture of sulfuric acid is the oxidation of SO2 gas to SO3:...
Homework Answers
According to Le Chatelier’s principle, the reaction tends to move in that direction which will undo the change.
Now, Since This is an exothermic reaction(Given ), their is an increase in Heat in forward direction.
Now, as temperature is decrease, we need to move in that direction where their is an increase in temperature (From Le Chatelier’s principle) which occurs in FORWARD DIRECTION.
Thus the yield of SO3(g) increases on decreasing temperature.
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One step in the manufacture of sulfuric acid is the oxidation
of SO2 gas to SO3:...
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...
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...
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...
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.
An engineer examining the oxidation of SO2 in the production of sulfuric acid determines that Kc...
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.
1) The reaction below is exothermic 2SO2 (g) + O2(g) = 2803(g) + heat Le Châtelier's...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
Using Le Chatelier's Principle, What will happen to the number of moles of SO3 in equilibrium...
Using Le Chatelier's Principle, What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the reaction? 2SO3(g) ⇌ 2SO2(g) + O2(g) in each of the following cases: 1. Oxygen is added to reaction container. 2. The pressure is increased by decreasing the volume of the reaction container. 3. In the rigid container (i.e. constant volume), the pressure is increased by adding argon gas. 4. The temperature of the reaction container is decreased (Note:...
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...
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.
. 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)
Calculate Δ G for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g)...
Calculate Δ G for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when P of SO2 = 0.500 atm, P of O2 = 0.0100 atm, and P of SO3 = 0.100 atm. The value for Δ G^o for this reaction at 298 K is -141.6 kJ. ΔG = ???? kJ I got -160.9 kj but it is incorrect.
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...
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