termine AHo for the combustion of ethanol. Given: AHof (in kJ mol-1): C2H5OH(): -277.69 CO2(g): -393.51 H2O(l): -28...
13 Calculate AHo, 298K for the following reaction: CO(g)1/2 O2(g) CO2(g) Given: AHof,298K (in kJ mol-1): CO(g): -110.53 CO2(g): -393.51
AGfº (kJ mol-4) -174.89 -394.36 -228.59 Using the data: AH” (kJ mol-1) . S°(JK-7 mol-1) C2H5OH (1) - 277.69 160.7 02 (9) 0 205.03 CO2(g) -393.51 213.63 H2O(g) -241.82 188.72 Calculate AG° at 25 °C for C2H5OH (g) + 3 O2(g) → 2 CO2(g) + 3 H2O(g). O A. 1325.4 kJ mol-1 O B. -1325.4 kJ mol-1 O C. -1649.4 kJ mol-1 O D. -1299.6 kJ mol-1 O E. 448.1 kJ mol-1
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)...
The experimentally determined heat of combustion of ethanol is 1233 kJ/mol. Calculate the heat of combustion of ethanol in kJ/g. Molar mass of ethanol C2H5OH = 46 g/mol C2H5OH(g) + 3 O2(g) → 2 CO2 (g) + 3 H2O(l) LaTeX: \DeltaΔH = -1233 kJ/mol
Calculate DG0rxn for the combustion of ethanol C2H5OH(g), at 750°C using the following data: C2H5OH(g) + O2(g) → CO2(g) + H2O(g) ∆G0f (C2H5OH(g)) = -167.9 kJ/mol, ∆G0f (02(g)) = 0 kJ/mol, ∆G0f (CO2(g)) = -394.4 kJ/mol, ∆G0f (H2O(g)) = -228
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...
For the combustion of cyclopropane at 25 ºC C3H6(g) + (9/2) O2(g) → 3 CO2(g) + 3 H2O(liq) ΔHºc(C3H6,g) = -2091 kJ / mol. What is the standard molar enthalpy of formation of cyclopropane(g) at 25 ºC if the standard molar enthalpies of formation of CO2(g) and H2O(liq) at that temperature are, respectively, -393.51 kJ / mol and -285.83 kJ / mol?
Ethanol (C2H5OH) is used as an additive in many fuels today. What is AHørxn (kJ) for the combustion of 2 moles of liquid ethanol? C2H5OH (1) + 3 O2() + 2 CO2(g) + 3 H20 (1) Formula Hºf (kJ/mol) @ 298K C2H5OH-277.6 CO2(g) -393.5 H2O () -241.8 H20 -285.8 A. -401.7 kJ B. +401.7 kJ C. -2469 kJ D. +2734 kJ E. -2734 kJ О Е ОА oc OB
The thermochemical equation for the combustion of ethanol is: C2H5OH (l) + 3 O2 (g) -> 2 CO2 (g) + 3 H2O (g) ΔHrxn = -1360 kJ What is the enthalpy change when 3.50 kg of ethanol react with excess oxygen?
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid para-benzoquinone, C6H4O2(s), is determined to be -2767.0 kJ mol-1. What is the Hf° of C6H4O2(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1 kJ mol-1