Ethanol is used as an additive in many fuels today. What is the ΔHºrxn for the combustion of ethanol?
2C2H5OH(l) + 6O2(g) → 4CO2(g) + 6H2O(l)
a)401.7 kJ
b)-401.7 kJ
c)-2734 kJ
d)-2469 kJ
Ethanol is used as an additive in many fuels today. What is the ΔHºrxn for the...
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
QUESTION 3 The balanced equation for the combustion of ethanol is 2C2H5OH(g) + 702(g) -> 4CO2(g) + 6H2O(g) How many grams of oxygen gas are required to burn 3.69 g of C2H50H? (write your answer with 3 sig figs and no units) QUESTION 4
L 255-7.cozts) to 2) Ethanol, C2H5OH, is promoted as a clean fuel and is used as an additive in many gasoline mixtures. Calculate the AH rxn for the combustion of ethanol. Tail Substance Hºf(kJ/mol) og C2H5OH( -277.0 5 GHSCUli) + O2(9) -> CO2(g) +H2O() CO2(8) -393.5 737 H20(9) -241.8 A)-1235.4 kJ B-751.8 kJ C) -358.3 kJ D) 358.3 kJ E) 1235.4 Kj
Ethanol (C2H6O) is used as an additive in gasoline . Calculate the molality of an ethanol solution prepared by dissolving 78.6 g of ethanol in enough water to produce 225 g of solution . Select one: A. 11.67 m B. 7.59 m C. 349.33 m D. 0.349 m E. 0.537 m
8. Ethanol is a common biofuel additive for gasoline. Estimate AH (kJ mol) for the combustion reaction of ethanol. Potentially useful bond energies are: H-H = 436 kJ/mol, O=0 = 499 kJ/mol, O-H 463 kl/mol, C=O = 799 kl/mol, C-O 358 kJ/mol, C-H= 411 kJ/mol, C-C = 346 kJ/mol a) -6000 b) - 1601 c) -1250 d) o e) + 4700
Time Taken:0:33:09 Brandon Bates: Attempt 1 MULUI PUT Ethanol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. Standard enthalpy formation of [CO2(e)] = -393.5 kJ/mol and [H20(1)] = -285.8 kJ/mol, C,H,OH(1) = -277.6 kJ/mol, what is the standard enthalpy of combustion of ethanol? kJ C,H, OH(1) + 3 02(g) + 2 CO2(g) + 3 H2O(l); A Hex = AH, /mol AH° (ræn) = In A Hfº (products) - In AHF ° (reac tants) +2349 kJ/mol +1366.8...
Calculate the amount of energy released as heat at constant pressure when 1.00 g of glucose undergoes a combustion reaction according to the equation below: C6H12O6(s) + 6O2(g) ® 6CO2(g) + 6H2O(g) ∆rHϴ = –2806 kJ (A) 16.00 kJ (B) 156.0 kJ (C) 468.0 kJ (D) 2806 kJ (E) 505600 kJ
CO2 is produced in a 1.75 L container at 751 mmHg and 35oC by combustion ethanol (C2H6O), how many mL of ethanol was used in this combustion? (density of ethanol is 0.789 g/mL). a) 4.78 mL b) 0.399 mL c) 3.78 mL d) 4.00 mL e) 2.00 mL
Many power plants produce energy by burning carbon-based fuels, which also produces carbon dioxide. Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the number of moles of CO2(g) produced per megajoule of heat released from the combustion of each fuel under standard conditions (1 atm and 25 �C). Each must be in mol * MJ^-1 (a) coal, C(s, graphite) (b) natural gas, CH4(g); (c) propane, C3H8(g);...
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter.In the laboratory a student burns a 0.796-g sample of glutaric acid(C5H8O4) in a bomb calorimeter containing 1000. g of water. The temperature increases from 25.70 °C to28.30 °C....