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TC05ЕОЗ Use the enthalpies of formation given in the table below to calculate the standard molar...
TC05E04 Use the enthalpies of formation given in the table below to calculate the standard molar enthalpy change for...
TC05E04 Use the enthalpies of formation given in the table below to calculate the standard molar enthalpy change for this reaction at 298K: 2CuS(s) 302(g)2CuO(s)+ 2SO2(g) AfH / kJ mol at 298K, standard Substance state 1 bar. CuO(s) -157 SO2(g) -297 CuS(s) -53 Select one: a. -802 kJ mol1 b. +401 kJ mol1 c. +802 kJ mol1 d. -507 kJ mol1 e. -401 kJ mol1
Chemistry
The "roasting" of 48.7 g of ZnS at constant pressure gives off 220. kJ of heat. Calculate the DH for this reaction.2ZnS(s) + 3O2(g) ® 2ZnO(s) + 2SO2(g)A.) -110 kJ/mol rxnB.) -293 kJ/mol rxnC.) -440. kJ/mol rxnD.) -881 kJ/mol rxnE.) +440. kJ/mol rxn
4. Use a standard enthalpies of formation values below to determine the change in enthalpy for...
4. Use a standard enthalpies of formation values below to determine the change in enthalpy for each of these reactions. Reaction: NaOH(s) + HCl(g) → NaCl(s) + H2O(g) Compound NaOH(s) HCl(g) NaCl(s) H2O(g) AHF (kJ/mol) -426.7 -92.3 -411.0 -241.8
Use a standard enthalpies of formation values below to determine the change in enthalpy for each...
Use a standard enthalpies of formation values below to determine the change in enthalpy for each of these reactions. SHOW WORK PLEASE. Reaction: NaOH(s) + HCl(g) →NaCl(s) + H2O(g) Compound ∆Hf (kJ/mol) NaOH(s) -426.7 HCl(g) -92.3 NaCl(s) -411.0 H2O(g) -241.8
TC04M01 Use the enthalpy changes given in the data below to calculate the enthalpy change for...
TC04M01 Use the enthalpy changes given in the data below to calculate the enthalpy change for this reaction: Cus(s) + O2(g) → Cu(s) + SO2(9) Data: Reaction no. Reaction A.HⓇ/kJ morat 298K standard state = 1 bar. +314 2 2 CuO(s) – 2Cu(s) + O2(g) S(s) + O2(g) - S02(9) 2CuO(s) + 2S(s) - 2CuS(s) + O2(9) -297 +208 Select one: a. +225 kJ/mol b.-85 kJ/mol O C. -244 kJ/mol d. -191 kJ/mol e. -225 kJ/mol
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous...
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
Heat of Formation Calculations: 32) Use a standard enthalpies of formation (Ho) table to determine the...
Heat of Formation Calculations: 32) Use a standard enthalpies of formation (Ho) table to determine the change in enthalpy for each of these reactions Hrxn [n. Ho(products) - n. Ho(products)] CO (g): -110.5 kJ/mol; CO2 (g): -393.5 kJ/mol CH4 (g): -890.4 kJ/mol H2O (l): -285.8 kJ/mol; H2O (g): -241.8 kJ/mol H2S (g): -20.6 kJ/mol; NO: -90.2 kJ/mol NO2: +33.9 kJ/mol; HCl (g): -92.3 kJ/mol NaOH (s): -426.7 kJ/mol; SO2 (g): -296.8 kJ/mol a) CH4(g) + 2 O2(g) ---> CO2(g) +...
Use the References to access important values if needed for this question. Given the standard enthalpy...
Use the References to access important values if needed for this question. Given the standard enthalpy changes for the following two reactions: (1) 2Fe(s) + O2(g) →2FeO(s) AH° = -544.0 kJ (2) 2Zn(s) + O2(g)—2ZnO(5) AH° = 696.6 kJ what is the standard enthalpy change for the reaction: (3) FeO(s) + Zn(s)—>Fe(s) + ZnO(s) AH° = ?
Use the information given here, data from Appendix D, and equation (7.22) to calculate the standard...
Use the information given here, data from Appendix D, and equation (7.22) to calculate the standard enthalpy of formation per mole of ZnS(s). 2 ZnS(s) + 302(g) —2 ZnO(s) + 2 SO2(g) A Hº = -878.2 kJ mol-1 (Reference to Equation 7.22):
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on...
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on the Appendix, calculate the following thermodynamic values for the complete combustion of ethanol: (10 points) C2H5OH(g) + 302(g) → 2CO2(g) + 3H2O(g) a) The standard enthalpy change (AHº) b) The standard entropy change (AS) c) Use values from a) and b) above to calculate AGO at 298K d) Is this reaction spontaneous at 298K under standard conditions?
TC05E04 Use the enthalpies of formation given in the table below to calculate the standard molar enthalpy change for this reaction at 298K: 2CuS(s) 302(g)2CuO(s)+ 2SO2(g) AfH / kJ mol at 298K, standard Substance state 1 bar. CuO(s) -157 SO2(g) -297 CuS(s) -53 Select one: a. -802 kJ mol1 b. +401 kJ mol1 c. +802 kJ mol1 d. -507 kJ mol1 e. -401 kJ mol1
4. Use a standard enthalpies of formation values below to determine the change in enthalpy for each of these reactions. Reaction: NaOH(s) + HCl(g) → NaCl(s) + H2O(g) Compound NaOH(s) HCl(g) NaCl(s) H2O(g) AHF (kJ/mol) -426.7 -92.3 -411.0 -241.8
TC04M01 Use the enthalpy changes given in the data below to calculate the enthalpy change for this reaction: Cus(s) + O2(g) → Cu(s) + SO2(9) Data: Reaction no. Reaction A.HⓇ/kJ morat 298K standard state = 1 bar. +314 2 2 CuO(s) – 2Cu(s) + O2(g) S(s) + O2(g) - S02(9) 2CuO(s) + 2S(s) - 2CuS(s) + O2(9) -297 +208 Select one: a. +225 kJ/mol b.-85 kJ/mol O C. -244 kJ/mol d. -191 kJ/mol e. -225 kJ/mol
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
Use the References to access important values if needed for this question. Given the standard enthalpy changes for the following two reactions: (1) 2Fe(s) + O2(g) →2FeO(s) AH° = -544.0 kJ (2) 2Zn(s) + O2(g)—2ZnO(5) AH° = 696.6 kJ what is the standard enthalpy change for the reaction: (3) FeO(s) + Zn(s)—>Fe(s) + ZnO(s) AH° = ?
Use the information given here, data from Appendix D, and equation (7.22) to calculate the standard enthalpy of formation per mole of ZnS(s). 2 ZnS(s) + 302(g) —2 ZnO(s) + 2 SO2(g) A Hº = -878.2 kJ mol-1 (Reference to Equation 7.22):
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on the Appendix, calculate the following thermodynamic values for the complete combustion of ethanol: (10 points) C2H5OH(g) + 302(g) → 2CO2(g) + 3H2O(g) a) The standard enthalpy change (AHº) b) The standard entropy change (AS) c) Use values from a) and b) above to calculate AGO at 298K d) Is this reaction spontaneous at 298K under standard conditions?
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