Using the values that were recorded, answer the questions. A) Find the energy value for the single ethanol molecule. This is the enthalpy of formation (Δ H f). Double this energy to determine the energy of two isolated ethanol molecules. Substract this value from the energy value for the two ethanol molecules with hydrogen bonding. Convert this result to kilojoules per mole (see Hint).

Question

Barclay

Chemistry

10 April, 18:48

Using the values that were recorded, answer the questions. A) Find the energy value for the single ethanol molecule. This is the enthalpy of formation (Δ H f). Double this energy to determine the energy of two isolated ethanol molecules. Substract this value from the energy value for the two ethanol molecules with hydrogen bonding. Convert this result to kilojoules per mole (see Hint).

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Answers (1)

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Keyon Coleman · Answer 1

-5.318213 x 10

Negative, exothermic

Explanation:

If you did the Spartan assignment, you'll have energy values for one ethanol molecules and two. For the first ethanol, double it. This is what you're going to subtract from the energy found from two ethanol molecules. Your answer should be negative. Because the enthalpy of formation is negative, that means heat is lost (exerted) and therefore exothermic.