| -2816 kJ/mol | |
| -5336 kJ/mol | |
| -1939 kJ/mol | |
| 580.7 kJ/mol |
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Heres the question, show work please! Calculate the enthalpy of combustion per mole for C6H12O6. Assume that the comb...
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into...
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol ______kJ/mol
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into...
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, Δ H o f CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol
1. Calculate the standard enthalpy of combustion for the following reaction: C6H12O6 (s) + 6 O2...
1. Calculate the standard enthalpy of combustion for the following reaction: C6H12O6 (s) + 6 O2 (g) ---> 6 CO2 (g) + 6 H2O (l) To solve this problem, we must know the following ΔH°f values: C6H12O6 (s) -1275.0 O2 (g) zero CO2 (g) -393.5 H2O (l) -285.8 5. 2. Using the reaction and ΔH from #1, calculate how many liters of oxygen gas will be used to produce 11,000 kJ of energy at 745 mmHg and 90°C.
Calculate the molar enthalpy of combustion of cinnamaldehyde (AH comb) (in kilojoules per mole of cinnamaldehyde)....
Calculate the molar enthalpy of combustion of cinnamaldehyde (AH comb) (in kilojoules per mole of cinnamaldehyde). kJ/mol 45
Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not...
Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not balanced. Round to the nearest whole number. C3H8(g) + O2 --> CO2(g) + H2O(l) kJ/mol Compound Hf (kJ/mole) C3H8(g) -105 CO2(g) -394 H2O(l) -284
Calculate the approximate enthalpy change, ?Hrxn, for the combustion of one mole of methane a shown...
Calculate the approximate enthalpy change, ?Hrxn, for the combustion of one mole of methane a shown in the balanced chemical equation: CH4+2O2?2H2O+CO2 Use the values you calculated in Parts A, B, C, and D, keeping in mind the stoichiometric coefficients. delta H CH4=1656 kJ/mol delta H O2=498 kJ/mol delta H H2O=-928 kJ/mol delta H CO2=-1598 kJ/mol
The standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. CzH3(g)...
The standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. CzH3(g) + 5 O2(g) + 3 CO2(g) + 4H2O(g) Calculate 4, Hº for propane based on the following standard molar enthalpies of formation. molecule CO2(g) H2O(g) 4,Hº (kJ/mol-rxn) -393.5 -241.8
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
7. Calculate the maximum non-expansion work per mole that may be obtained from the combustion of...
7. Calculate the maximum non-expansion work per mole that may be obtained from the combustion of methanol at 298 K. (10 pts) 2CH,OH (g) + O2 (g) 2002 (g) + 4H20 (1) CH,OH (g) 0:(8) CO2(g) H20 (1) A, Gº (kJ mol) -161.96 0 -394.36 -273.13
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some...
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some of the following data to calculate the molar enthalpy of formation of C2H6(g) at 298.15 K 2. Calculate the molar enthalpy of combustion of ethane at 500K Table provided gives values of standard enthalpy of formation values at 298.15 K Substance deltafH (kJ*mol^-1) Cpm (J*K^-1*mol^-1) CO2 (aq) -413.8 N/A CO2 (g) -393.51 37.11 H2O (l) -285.83 75.291 H2O(g) -241.82 33.58 C2H6(g) to be determined...
Calculate the molar enthalpy of combustion of cinnamaldehyde (AH comb) (in kilojoules per mole of cinnamaldehyde). kJ/mol 45
The standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. CzH3(g) + 5 O2(g) + 3 CO2(g) + 4H2O(g) Calculate 4, Hº for propane based on the following standard molar enthalpies of formation. molecule CO2(g) H2O(g) 4,Hº (kJ/mol-rxn) -393.5 -241.8
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
7. Calculate the maximum non-expansion work per mole that may be obtained from the combustion of methanol at 298 K. (10 pts) 2CH,OH (g) + O2 (g) 2002 (g) + 4H20 (1) CH,OH (g) 0:(8) CO2(g) H20 (1) A, Gº (kJ mol) -161.96 0 -394.36 -273.13
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