Which of these statements are true? Select all that apply. The Delta.Hf for Br2(I) is 0 kJ/mol. The Delta.Hf for He(I) is 0 kJ/mol. The Delta.Hf for Hg(I) is 0 kJ/mol. The Delta.Hf for Cl2(g) is 0 kJ/mol. The Delta.Hf for N2(I) is 0 kJ/mol. CORRECT ANSWER IS A, C, AND D.

Enthalpy of formation is defined as the change in the enthalpy when 1 mole of a chemical substance is formed from its pure element at standard conditions. It is represented by the symbol [tex]\Delta H_{f}[/tex]

Enthalpy of formation for elemental atoms is always equal to 0.

We know:

Bromine (Br) exists in a liquid state.

Helium (He) exists in a gaseous state.

Mercury (Hg) exists in a liquid state.

Chlorine (Cl) exists in a gaseous state.

Nitrogen (N) exists in a gaseous state.

For the given options:

The [tex]\Delta H_{f}[/tex] for [tex]Br_2(l), Hg(l)\text{ and }Cl_2(g)[/tex] will be equal to 0 because they are formed by the natural states of their elemental atoms.

Hence, the correct options are A, C and D.

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-12-10T20:07:04+01:00

A substance in its standard state has an enthalpy of formation of 0 kJ/mol.

The enthalpy of formation of a substance in its standard state is 0 kJ/mol.

The standard state of a substance refers to its state at 1 atm and at a temperature of 298 K. Bearing this in mind, we can now identify the true and false statements.

So,

ΔHf for Br2(I) is 0 kJ/mol - True

ΔHf for He(I) is 0 kJ/mol - False

ΔHf for Hg(I) is 0 kJ/mol - True

ΔHf for Cl2(g) is 0 kJ/mol - True

ΔHf for N2(I) is 0 kJ/mol - False

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