What is the DeltaG of the following reaction in kJ/mol of ethanol? C2H5OH(g) + 3 O2(g)...
What is the DeltaG of the following reaction in kJ/mol of ethanol?
C2H5OH(g) + 3 O2(g) ? 2 CO2(g) + 3 H2O(g) E°cell = 1.13 V
The answer is -1310 kj/mol. Please explain how you got the answer.
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What is the DeltaG of the following reaction
in kJ/mol of ethanol?
C2H5OH(g) + 3
O2(g)...
Ethanol (C2H5OH) is used as an additive in many fuels today. What is AHørxn (kJ) for...
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
A 2.11 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C-5.65 kJ/"C. C2H5OH() + 3 O2...
A 2.11 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C-5.65 kJ/"C. C2H5OH() + 3 O2(g) + 2 CO2(g) + 3 H2O(g) AH'rxn=-1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in "C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q=m's'AT, heat capacity is equivalent to Cum's, giving Heat capacity is extensive whereas specific heat is intensive. -CAT.
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
The thermochemical equation for the combustion of ethanol is: C2H5OH (l) + 3 O2 (g) ->...
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?
Calculate DG0rxn for the combustion of ethanol C2H5OH(g), at 750°C using the following data: ...
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 experimentally determined heat of combustion of ethanol is 1233 kJ/mol. Calculate the heat of combustion...
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
2.21 g of ethanol C2H5OH and 3.55 of oxygen O2 are reacted. Molar mass of C2H5Oh...
2.21 g of ethanol C2H5OH and 3.55 of oxygen O2 are reacted. Molar mass of C2H5Oh 46.08 g/mol. O2 32.00 g/mol. Co2 44.01 g/mol. H20 18.02 g/mol a)What is the limiting reactant? b) what is the theoretical yield of carbon dioxide in grams will be obtained in the combustion reaction. starting with the amount of reagents given in part (a). assuming the reaction goes in 100% yield. c) If 0.951 f of CO2 is obtained from the reaction above, what...
termine AHo for the combustion of ethanol. Given: AHof (in kJ mol-1): C2H5OH(): -277.69 CO2(g): -393.51 H2O(l): -28...
termine AHo for the combustion of ethanol. Given: AHof (in kJ mol-1): C2H5OH(): -277.69 CO2(g): -393.51 H2O(l): -285.83 • 13. Calculate AHO, 298K for the following reaction: CO(g) + 1/2 02(g) 2 CO2(g) Given: A Hof,298K (in kJ mol-1): CO(g): -110.53 CO2(g): -393.51
For the unbalanced combustion reaction shown below, 1 mol of ethanol, C2H5OH, releases 327 kcal (1370...
For the unbalanced combustion reaction shown below, 1 mol of ethanol, C2H5OH, releases 327 kcal (1370 kJ). C2H5OH+O2→CO2+H2O How much heat (in kilocalories) is released from the combustion of 7.38 g of ethanol? How many grams of C2H5OH must be burned to raise the temperature of 360.0 mL of water from 20.0 ∘C to 100.0 ∘C? (The specific heat of water is 1.00 cal/g⋅∘C or 4.184 J/(g⋅∘C). Assume the density of water at 20.0∘C is 1.00 g/mL.
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
A 2.11 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C-5.65 kJ/"C. C2H5OH() + 3 O2(g) + 2 CO2(g) + 3 H2O(g) AH'rxn=-1235 kJ If the initial temperature is 25.0°C, what is the final temperature (in "C) of the calorimeter? The molar mass of ethanol is 46.07 g/mol. Remember, in the heat equation, q=m's'AT, heat capacity is equivalent to Cum's, giving Heat capacity is extensive whereas specific heat is intensive. -CAT.
termine AHo for the combustion of ethanol. Given: AHof (in kJ mol-1): C2H5OH(): -277.69 CO2(g): -393.51 H2O(l): -285.83 • 13. Calculate AHO, 298K for the following reaction: CO(g) + 1/2 02(g) 2 CO2(g) Given: A Hof,298K (in kJ mol-1): CO(g): -110.53 CO2(g): -393.51
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