Homework Answers
The heat required to heat SO2 is calculated:
q SO2 = n * cp * ΔT = 7219 mol * 0.0384 kJ / mol * K * (400 - 25) = 103 954 kJ
The heat required to heat the O2 is calculated:
q O2 = 7219 * 0.5 * 0.0352 * (400 - 25) = 47645 kJ
total q = 151599 kJ
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SO2(g) + 0.5 O2(g) -> SO3(9) a) What quantity of heat is needed to raise 7219...
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
Consider the reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (9) If 278.2 mL...
Consider the reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (9) If 278.2 mL of SO2 is allowed to react with 168.1 mL of Oz (both measured at STP), what is the theoretical yield o SO3? V AUD S moo? A W Theoretical Yield mol If 180.7 mL of SO3 is collected (measured at STP), what is the percent yield for the reaction? 190 AM OO ? Percent Yield =
5) For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), if initially P(SO2) = 1.2...
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
1).From the following enthalpy changes, S (s) +3/2 O2 (g) 2 SO2 (g) SO3 (g) O2...
1).From the following enthalpy changes, S (s) +3/2 O2 (g) 2 SO2 (g) SO3 (g) O2 (g)2 SO3 (g) AH =-395.2 kJ AHo 198.2 kJ Calculate the value of AHo for the reaction by using Hess's law of Heat Summation S(s) O2 (g) SO2 (g) 2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2. 4 CO2 (g) +2 H20 (g) 2 C2H2 + 5 O2 (g) If the enthalpy change for the reaction is -2511.14 kJ/mol, a) How...
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above...
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above reaction is allowed to reach equilibrium prior to the following changes. Answer the following questions by writing increase, decrease or remain the same on the line. **please also explain why** If the reaction mixture is heated up , the value of the equilibrium constant will _______________________ If SO2 (g) is added to the reaction vessel the concentration of O2(g) will____________________________. If SO3 (g) is...
3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x...
3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x = -197.6 kJ a. If 285.3 g of SO2 is allowed to react with 158.9 g of O2, what is the limiting reactant and theoretical yield of SO3 in liters if the reaction is performed at 315 K and 50.0 mmHg? How much of each reactant remains at the end of the reaction? [10] LR: SO TY: SO2 remaining: O2 remaining: Imol soa 64.000log...
1). From the following enthalpy changes, S (s) + 3/2 O2 (g) → SO3 (9) 2...
1). From the following enthalpy changes, S (s) + 3/2 O2 (g) → SO3 (9) 2 SO2 (g) + O2(g) → 2 SO3 (9) AH° = -395.2 kJ AH° = -198.2 kJ Calculate the value of AH° for the reaction by using Hess's law of Heat Summation S (s) + O2 (g) → SO2 (g).
1. Calculate A Gº for the reaction at 25°C 2 SO2(g) + O2(g) → 2 SO3...
1. Calculate A Gº for the reaction at 25°C 2 SO2(g) + O2(g) → 2 SO3 (g), given that AHº is -197.7 kJ mol- and A.Sº is -188 JK' mol!
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given...
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given the thermochemical equations below. 2 S(s) + 3 O2(g) =2 SO3(g) AH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) AH° = -197 9 kJ Show all work and calculate to the correct number of sig figs.
Consider the reaction of NO(g) from its elements. 2 502(g) + O2(g) → 2 SO3(9) Use...
Consider the reaction of NO(g) from its elements. 2 502(g) + O2(g) → 2 SO3(9) Use the thermodynamic data given to determine the following for this reaction: AH°, equal O kJ/mol Asº, equals O J/molk Calculate the AG, at 500 °c with all gases at standard pressure and equilibrium constant K at 500 °C. AG, at 500 °c equals O kJ/mol K at 500 equals tance (kJ/mol) (J/mol-K) O2(g) 205.2 SO2(g) -296.8 248.2 SO3(9) -395.7 240.0 AHO so
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
Consider the reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (9) If 278.2 mL of SO2 is allowed to react with 168.1 mL of Oz (both measured at STP), what is the theoretical yield o SO3? V AUD S moo? A W Theoretical Yield mol If 180.7 mL of SO3 is collected (measured at STP), what is the percent yield for the reaction? 190 AM OO ? Percent Yield =
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
1).From the following enthalpy changes, S (s) +3/2 O2 (g) 2 SO2 (g) SO3 (g) O2 (g)2 SO3 (g) AH =-395.2 kJ AHo 198.2 kJ Calculate the value of AHo for the reaction by using Hess's law of Heat Summation S(s) O2 (g) SO2 (g) 2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2. 4 CO2 (g) +2 H20 (g) 2 C2H2 + 5 O2 (g) If the enthalpy change for the reaction is -2511.14 kJ/mol, a) How...
3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x = -197.6 kJ a. If 285.3 g of SO2 is allowed to react with 158.9 g of O2, what is the limiting reactant and theoretical yield of SO3 in liters if the reaction is performed at 315 K and 50.0 mmHg? How much of each reactant remains at the end of the reaction? [10] LR: SO TY: SO2 remaining: O2 remaining: Imol soa 64.000log...
1). From the following enthalpy changes, S (s) + 3/2 O2 (g) → SO3 (9) 2 SO2 (g) + O2(g) → 2 SO3 (9) AH° = -395.2 kJ AH° = -198.2 kJ Calculate the value of AH° for the reaction by using Hess's law of Heat Summation S (s) + O2 (g) → SO2 (g).
1. Calculate A Gº for the reaction at 25°C 2 SO2(g) + O2(g) → 2 SO3 (g), given that AHº is -197.7 kJ mol- and A.Sº is -188 JK' mol!
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given the thermochemical equations below. 2 S(s) + 3 O2(g) =2 SO3(g) AH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) AH° = -197 9 kJ Show all work and calculate to the correct number of sig figs.
Consider the reaction of NO(g) from its elements. 2 502(g) + O2(g) → 2 SO3(9) Use the thermodynamic data given to determine the following for this reaction: AH°, equal O kJ/mol Asº, equals O J/molk Calculate the AG, at 500 °c with all gases at standard pressure and equilibrium constant K at 500 °C. AG, at 500 °c equals O kJ/mol K at 500 equals tance (kJ/mol) (J/mol-K) O2(g) 205.2 SO2(g) -296.8 248.2 SO3(9) -395.7 240.0 AHO so
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