Reference no: EM132409908
Ethanol, a fuel derived from fermentation of corn or other biomass, burns according to the thermochemical equation. 2C2H5OH (l) + 3O2 (g) -> 2CO2 + 3H2O + 1367 kJ
a. Write out all possible mole ratios for all reactants and products plus all possible ratios for the enthalpy term.
b. What mass of CO2 is released per mole of ethanol burned?
c. What mass of CO2 is produced from 200g of ethanol?
d. What mass of oxygen is required to burn 300g of ethanol completely?
e. How much energy is released if 400g of ethanol is burned?
Answer the following questions for the case where 250g of ethanol is burned in the presence of 150g of oxygen.
a. Is this a stoichiometric mixture of reactants? If not, which is the limiting reactant?
b. How many grams of CO2 and water are produced by this reaction? What mass of reactant (if any) remains unused?
c. How much energy is released by this reaction?
If you have 1.0 litre of ehanol and 1.5 litres of methanol (both liquids at room temperature). How much heat energy (expressed as kj) will each release if burned in an ample supply of oxygen. Which will release more heat? Hint you need to find several values for each chemical in order to answer this question. Be sure to state the values you found and where you found them?
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Fermentation of corn or other biomass
: Ethanol, a fuel derived from fermentation of corn or other biomass, burns according to the thermochemical equation. 2C2H5OH (l) + 3O2 (g) -> 2CO2 + 3H2O + 1367
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