contestada

Which statement about Delta.Hf is true?
It is zero for any compound in its standard state.
It is positive when the bonds of the product store more energy than those of the reactants.
It is negative when a compound forms from elements in their standard states.
It is zero for any element that is in the liquid state.

Respuesta :

Edufirst

Answer:

  • It is positive when the bonds of the product store more energy than those of the reactants. (the second statement)

Explanation:

ΔHf is the change of enthalpy during the reaction, which is equal to the sum of enthaply  changes of the products less the sum of the enthalpy changes of the reactants.

  • ΔHf = ∑ (ΔH products)  - ∑ (ΔH reactants)

  • ΔHf = ΔH rxn

Also, ΔHrxn, per definition, is the potential chemical energy stored in the bonds of the products less the chemical potential energy stored in the bonds of the reactants.

Then, when the potential chemical energy stored in the bonds of the products is greater than the chemical potential energy stored in the bonds of the reactants ΔHrxn is positive.

Hence, you conclude that ΔHf is positive when the bonds of the product store more energy than those of the reactants (second statement from the choices).

Some brief comments about the other statements:

  • The standard enthalpy of formation, ΔHf, is zero for an element in its standard state, not for a compound.

  • For a compound the enthalpy of formation at 25ºC and 1 atm (the standard state) may be positive or negative.

  • Also, note that the standard state for any element is not liquid: some are solids, some are gases, and some are liquids at 25ºC and 1 atm.

izzypalmisano

Answer:

B

Explanation:

answer on edg :)

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