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N Molecule AH!" (kJ mor') CO (g) Sº (J K' mol') 197.67 -110.52 He(...
12. Using the data: CH«(9), AH; = +51.9 kJ mor', sº = 219.8 J mor' k'...
12. Using the data: CH«(9), AH; = +51.9 kJ mor', sº = 219.8 J mor' k' CO2(g), AH = -394.0 kJ mor', sº = 213.6 J mor' k' H2O(), AH = -286.0 kJ mor', sº = 69.96 J mor'' O2(g), AH = 0.00 kJ mor', sº = 205 J mor'' calculate the maximum amount of useful work that can be obtained, at 25.0 °C, from the process: C2H4(9) + 3 O2(g) → 2 CO2(g) + 2 H2O(1) a. 1332 kJ...
→ Fe(s) + CO2(g), AGº is - 5.8 kJ and AH° is -11 kJ. Sº (J...
→ Fe(s) + CO2(g), AGº is - 5.8 kJ and AH° is -11 kJ. Sº (J mol-? K-'); 4. For the reaction Fe(s) + CO(g) Fe (27.3), CO(197.5), CO (213.7) a) What is AS sur? [37 JK-'] b) Use AG to determine whether the reaction is spontaneous or nonspontaneous under standard conditions. Explain. c) Use AS univ to determine whether the reaction is spontaneous or nonspontaneous under standard conditions. Explain. d) What is Sº for FeO? [61 J mol-'K-']
For the reaction CO2(g) + H2(9)—-CO(g) +H30(9) AH° = 41.2 kJ and A Sº = 42.1...
For the reaction CO2(g) + H2(9)—-CO(g) +H30(9) AH° = 41.2 kJ and A Sº = 42.1 JK The equilibrium constant for this reaction at 252.0 K is Assume that AH and AS are independent of temperature. For the reaction N2(g) + 3H2(g) 2NH3(g) AH° = -92.2 kJ and AS™ = -198.7 J/K The equilibrium constant for this reaction at 347.0 K is Assume that AHⓇ and AS are independent of temperature.
2. Use the following rxn to answer the questions. CO(g) + 2 H2(9) = CH3OH(1) For...
2. Use the following rxn to answer the questions. CO(g) + 2 H2(9) = CH3OH(1) For this reaction, AH = -128.1 kilojoules Sº (J/mol.K) AH (kJ/mol) -110.5 AG, (kJ/mol) -137.3 197.9 CO(g) CH,OH(1) -238.6 - 166.2 126.8 The data in the table above were determined at 25°C. a) Calculate AGº for the reaction above at 25°C. b) Calculate Key for the reaction above at 25°C. c) Calculate AS for the reaction above at 25°C. d) In the table above, there...
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate...
The reaction below has an equilibrium constant of
Kp=2.26×104 at 298 K.
CO(g)+2H2(g)⇌CH3OH(g)
Part A Calculate Kp for the reaction below. CH3OH(g) CO(g)+2H2(g) Submit My Answers Give Up Part B Reactants will be favored at equilibrium. O Products will be favored at equilibrium. Submit My Answers Give Up Part C Calculate Kp for the reaction below. 를 CO (g) + H2 (g)- CH, OH (g) K=
What is the Kp for the reaction at 700 K? 35. For the reaction CO(g)+2H2(g) CH3OH(g...
What is the Kp for the reaction at 700 K?
35. For the reaction CO(g)+2H2(g) CH3OH(g ) AG 700K-13.464 kJ. What is Kp for this reaction at 700. K? a. 1.00 b. 1.54 c. 10.1 d. 2.31 e. none of these Copyright Cengage Leaming. Powered by Cognero. Pac
b Consider the reaction: Ca(s) +2 H2001) + Ca(OH)2(aq) +2H2(g) -285.83 -1002.82 AH" (kJ/mol) S°(J/K) mol...
b Consider the reaction: Ca(s) +2 H2001) + Ca(OH)2(aq) +2H2(g) -285.83 -1002.82 AH" (kJ/mol) S°(J/K) mol 41.59 69.95 -74.5 130.7 Is the reaction spontaneous at 298 K? AH° = -431.16 AS° = 5.41 AG° = -432.77 O Yes O No Submit Submit Answer Retry Entire Group 9 more group attempts remaining
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol...
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol K) 0 205.1 Oxygen 02 (g) O(g) 03 (g) 249.2 231.7 161.1 142.7 163.2 238.9 Phosphorus AH° (kJ/mol) AG°f(kJ/mol) sº (/mol K) Nitrogen AH°(kJ/mol) AG°f(kJ/mol) s° /mol K) N2 (8) 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 132.0 -79.0 113.0 90.3 86.6 210.8 51.7 66.1 261.8 NH4+ (aq) NO (g) NOCI (9) NO2 (g)...
10. For H2(g) + CO2(g) ←→CO(g) + H2O(g), AH 34.78 kJ/mol at 1000 K. If Kp...
10. For H2(g) + CO2(g) ←→CO(g) + H2O(g), AH 34.78 kJ/mol at 1000 K. If Kp = 0.236 at 800 K, calculate Kp at 1200 K, assuming that 4H' does not vary significantly with temperature.
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K,...
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
12. Using the data: CH«(9), AH; = +51.9 kJ mor', sº = 219.8 J mor' k' CO2(g), AH = -394.0 kJ mor', sº = 213.6 J mor' k' H2O(), AH = -286.0 kJ mor', sº = 69.96 J mor'' O2(g), AH = 0.00 kJ mor', sº = 205 J mor'' calculate the maximum amount of useful work that can be obtained, at 25.0 °C, from the process: C2H4(9) + 3 O2(g) → 2 CO2(g) + 2 H2O(1) a. 1332 kJ...
→ Fe(s) + CO2(g), AGº is - 5.8 kJ and AH° is -11 kJ. Sº (J mol-? K-'); 4. For the reaction Fe(s) + CO(g) Fe (27.3), CO(197.5), CO (213.7) a) What is AS sur? [37 JK-'] b) Use AG to determine whether the reaction is spontaneous or nonspontaneous under standard conditions. Explain. c) Use AS univ to determine whether the reaction is spontaneous or nonspontaneous under standard conditions. Explain. d) What is Sº for FeO? [61 J mol-'K-']
For the reaction CO2(g) + H2(9)—-CO(g) +H30(9) AH° = 41.2 kJ and A Sº = 42.1 JK The equilibrium constant for this reaction at 252.0 K is Assume that AH and AS are independent of temperature. For the reaction N2(g) + 3H2(g) 2NH3(g) AH° = -92.2 kJ and AS™ = -198.7 J/K The equilibrium constant for this reaction at 347.0 K is Assume that AHⓇ and AS are independent of temperature.
2. Use the following rxn to answer the questions. CO(g) + 2 H2(9) = CH3OH(1) For this reaction, AH = -128.1 kilojoules Sº (J/mol.K) AH (kJ/mol) -110.5 AG, (kJ/mol) -137.3 197.9 CO(g) CH,OH(1) -238.6 - 166.2 126.8 The data in the table above were determined at 25°C. a) Calculate AGº for the reaction above at 25°C. b) Calculate Key for the reaction above at 25°C. c) Calculate AS for the reaction above at 25°C. d) In the table above, there...
The reaction below has an equilibrium constant of
Kp=2.26×104 at 298 K.
CO(g)+2H2(g)⇌CH3OH(g)
Part A Calculate Kp for the reaction below. CH3OH(g) CO(g)+2H2(g) Submit My Answers Give Up Part B Reactants will be favored at equilibrium. O Products will be favored at equilibrium. Submit My Answers Give Up Part C Calculate Kp for the reaction below. 를 CO (g) + H2 (g)- CH, OH (g) K=
What is the Kp for the reaction at 700 K?
35. For the reaction CO(g)+2H2(g) CH3OH(g ) AG 700K-13.464 kJ. What is Kp for this reaction at 700. K? a. 1.00 b. 1.54 c. 10.1 d. 2.31 e. none of these Copyright Cengage Leaming. Powered by Cognero. Pac
b Consider the reaction: Ca(s) +2 H2001) + Ca(OH)2(aq) +2H2(g) -285.83 -1002.82 AH" (kJ/mol) S°(J/K) mol 41.59 69.95 -74.5 130.7 Is the reaction spontaneous at 298 K? AH° = -431.16 AS° = 5.41 AG° = -432.77 O Yes O No Submit Submit Answer Retry Entire Group 9 more group attempts remaining
*** ** -305.01 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 AHºf (kJ/mol) AG°f (kJ/mol) Sº (/mol K) 0 205.1 Oxygen 02 (g) O(g) 03 (g) 249.2 231.7 161.1 142.7 163.2 238.9 Phosphorus AH° (kJ/mol) AG°f(kJ/mol) sº (/mol K) Nitrogen AH°(kJ/mol) AG°f(kJ/mol) s° /mol K) N2 (8) 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 132.0 -79.0 113.0 90.3 86.6 210.8 51.7 66.1 261.8 NH4+ (aq) NO (g) NOCI (9) NO2 (g)...
10. For H2(g) + CO2(g) ←→CO(g) + H2O(g), AH 34.78 kJ/mol at 1000 K. If Kp = 0.236 at 800 K, calculate Kp at 1200 K, assuming that 4H' does not vary significantly with temperature.
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
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