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17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on...
please answer 17a,b,c 17. Using values for the standard enthalpies of formation (AHY) and standard molar entropy (AS 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 AG° at 298K Formula SU/(K-mol 160 TABLE 16.1 Standard Molar Entropies for Some Common Substances at 25...
Brazilains are quite familiar with fueling their automobiles with ethanol, a fermentation product from sugarcane. Calculate the standard molar enthalpy for the complete combustion of liquid ethanol (C2H5OH) using the standard enthalpies of formation of the reactants and the products. C2H5OH (l) + 3O2 (g) --> 2CO2 (g) + 3H2O (g)
5. The standard molar entropy of liquid ethanol (C2H5OH) is 160.7 J K mol and the standard enthalpy of combustion is - 1368 kJ mol at 298 K, how much is the standard Gibbs energy (A,Gº) of formation of liquid ethanol at 298 K? (20 pts) The formation reaction of ethanol is 2C (graphite) + O2(g) + 3H2 (g) → C2H5OH() The combustion reaction of ethanol is CH5OH (1) + 302 (9) ► 200, (g) + 3H20 (1) CO; (g)...
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
question 15 please, thanks! (15 points) Ethanol is being promoted as renewable biofuel. Use the standard enthalpies of formation below to determine the standard enthalpy of combustion of ethanol shown below. 15 CH3CH2OH + 302-2CO2 +3H20 AHP-? Af of 02 0 AH in kJ/mol -277 Substance CH,CH2OHD CO(g) H-OD -394 -286
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found in Appendix B of the textbook to calculate the enthalpy change of the reaction. The standard enthalpy of formation of BsH, (I) is 73.2 kl/mol. 5 B2Os (s) +9 H2O (I) (b) Predict the sign of the entropy change and provide the two reasons likely to have made the biggest impact on the entropy change (and upon which you based your prediction). (c) Based...
TC05ЕОЗ Use the enthalpies of formation given in the table below to calculate the standard molar enthalpy change for this reaction at 298K: 2ZnS(s) 302(g) 2ZnO(s) + 2SO2(g) Att / kJ mol at 298K, standard state 1 bar, Substance ZnO(s) -350 SO2(g) -297 ZnS(s) -206 Select one: a. -441 kJ mor1 b. -853 kJ mol1 c. +882 kJ mol 1 d. +441 kJ molr1 e. -882 kJ mol1 TСОЗЕОЗ A chemical reaction carried out at an ambient pressure of 1.02...
answer should be in sig figs. LReterences] TUTOR Calculating Enthalpy Change Using the standard formation enthalpies that follow, calculate the standard enthalpy change for this reaction. 2CO(g)+2NO(g)2CO2(g)+ N2(g) AH kJ Species AHo (kJ/mol) -110.5 CO(g) NO(g) CO2(g) 90.3 -393.5
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]
3. Using standard enthalpies of formation, calculate AH° for the reaction 2H2S@+3026 2SO2(+2H2O 4. The first step in the preparation of lead from its ore (PbS) consists of roasting the ore. 2P6S+302® 2SO20 2P6O) Use the standard enthalpies of formation from Appendix II in your text to calculate the AH for the reaction above.