How much heat is released if 35.0 g of ethanol (C2H5OH) burns in excess oxygen? C2H5OH()...
Ethanol, C2H5OH, burns in oxygen gas by the following reaction. C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g); ΔH = -1235 kJ How many grams of ethanol would be needed to provide 293 kJ of heat?
Ethanol burns in oxygen to form CO2 and water: C2H5OH + 3O2 --> 2CO2 + 3H2O What is the amount of H2O produced from 0.55 mol C2H5OH? What is the amount of H2O produced from 0.55 mol C2H5OH Please show all work.
Heat Capacity and Calorimetry A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25C to 33.73C. If the heat capacity of the calorimeter and contents is 9.63kJ/C, what is the value of q for burning 1.00 lol of ethanol at constant volume and 25.00C. Is q equal to U or H? 214e Questions and Problems the enthalpy change when 0.710 mol of calcium...
Gasohol is a mixture of gasoline and ethanol (grain alcohol), C2H5OH. Calculate the maximum work that could be obtained at 25 ºC and 1 atm by burning 1 mol of C2H5OH. C2H5OH(l ) + 3O2(g)-------> 2CO2(g) + 3H2O(g) Review Problem 18.089 Incorrect. Gasohol is a mixture of gasoline and ethanol (grain alcohol), C2H5OH. Calculate the maximum work that could be obtained at 25 °C and 1 atm by burning 1 mol of C2H5OH. C2H5OH(1) + 302(g) 2C02(g) + 3H2O(g) -3976...
A 2.50 g sample of ethanol, C2H5OH, was combusted in the presence of excess oxygen in a bomb calorimeter containing 2.00 kg of water. The temperature of the water increased from 22.500oC to 27.845oC. The heat capacity of the calorimeter is 2520 J/oC and the specific heat capacity of water is 4.184 J/goC. Calculate the molar enthalpy of the combustion reaction in kJ/mol
With a good explanation please. An amount of 3.355 g ethanol C2H5OH(1) is burned completely in a calorimeter at 298.15 K. The heat produced is 99.472 kJ. It can be assumed that the measurement takes place under constant pressure of 1 bar. C2H5OH(1) + 302(g) + 2CO2(g) + 3H2O(1) 3a. (10 points) Calculate the standard enthalpy of reaction AHR based on the calorimeter mea- surement.
When wine goes bad, the ethanol (C2H5OH) is converted to acetic acid (HC2H3O2) in the following reaction: C2H5OH(l)+O2(g)→HC2H3O2(l)+H2O(l) However, this is usually a slow reaction, and when doing it in a calorimeter, the reaction goes to complete oxidation, giving the heats of reaction listed below: C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l),HC2H3O2(l)+2O2(g)→2CO2(g)+2H2O(l),ΔH∘=1410 kJ/molΔH∘=874 kJ/mol Part B Determine the heat of the reaction (ΔH) for the conversion of ethanol to acetic acid.
4) Ethanol, C2H5OH, is mixed with gasoline and is sold as gasohol at many gas stations. C2H5OH (l) + 3O2(g) → 2CO2(g) +3H2O (g) ∆H = –1235 kJ a. Determine the mass of ethanol that could produce 358 kJ of energy. b. This reaction was found to be 71.0 % efficient. Calculate the mass of oxygen required to produce 56.0 g CO2 if it were present in 10.0 % excess. c. Calculate the volume of O2 produced in question b...
The heat of combustion of ethanol, C2H5OH(l), is -1367 kJ/mol. A batch of sauvignon blanc wine contains 11.2 % ethanol by mass. Assuming the density of the wine to be 1.0 g/mL, what is the caloric content due to the alcohol (ethanol) in a 6-oz glass of wine (177 mL)?
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...