Chemistry Forum

So, here's the problem:

Remember that enthalpy goes with the balanced reaction and can be treated like a product; therefore, stoichiometry applies to enthalpy. The following balanced equation goes with the given -1367.1 kJ. Any change in the amount of the reactants and products would change the amount of heat (kJ) released by the reaction.

1. Consider the following reaction:
C₂H₅OH(l) + 3 O₂(g) 2CO₂(g) + 3H₂O(l)
ΔHo = -1367.1 kJ

Calculate the heat released when each of the following amounts of ethanol (C₂H₅OH(l)) is burned.
a. 1.0 g of C₂H₅OH(l)
b. 1.0 mol of C₂H₅OH(l)
c. 1.00x102 mol C₂H₅OH(l)
d. A mixture of 10.0g C₂H₅OH(l) and 10.0g of O₂

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My teacher gives us these problems before we even start that section so I'm pretty lost.

amaatreb wrote:So, here's the problem:

Remember that enthalpy goes with the balanced reaction and can be treated like a product; therefore, stoichiometry applies to enthalpy. The following balanced equation goes with the given -1367.1 kJ. Any change in the amount of the reactants and products would change the amount of heat (kJ) released by the reaction.

1. Consider the following reaction:
C₂H₅OH(l) + 3 O₂(g) 2CO₂(g) + 3H₂O(l)
ΔHo = -1367.1 kJ

Calculate the heat released when each of the following amounts of ethanol (C₂H₅OH(l)) is burned.
a. 1.0 g of C₂H₅OH(l)
b. 1.0 mol of C₂H₅OH(l)
c. 1.00x102 mol C₂H₅OH(l)
d. A mixture of 10.0g C₂H₅OH(l) and 10.0g of O₂

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My teacher gives us these problems before we even start that section so I'm pretty lost.

First calculate how much heat is released when 1 mol of C₂H₅OH(l) is burned.
In this particular case since C₂H₅OH(l) participates in reaction with coefficient 1: Q = -ΔHo = 1367.1 kJ
For the a. and c. just multiply this number to the number of moles.
For d. take into account which one is the limiting reagent.