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.

The standard enthalpy of formation is defined as the enthalpy change for creating one mole of a compound from elements in their standard states.

The enthalpy of formation (ΔHf) of [tex]Br_2[/tex] (g) at 1.00 atm and 298 K is 0 kJ/mol.

It is because the enthalpy of formation of the molecule is only 0 in its standard state and for bromine, the standard state at 298K is the liquid state.

Hence, option A is correct.

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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.

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What does ΔHf mean?

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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.