How do you write the equation that represents the formation of HF(g)?
Answer:
\(\frac{1}{2} H_{2}(g)+\frac{1}{2} F_{2}(g) \rightarrow H F(g) ; \Delta H_{\mathrm{rxn}}=\Delta H_{f}^{\circ}\)
Explanation:
The standard enthalpy of formation is defined as the enthalpy associated with the formation of one mole of substance from it elements in their standard states, under standard conditions.
Given this definition, \(\Delta H_{f}^{\circ} H F\) is the enthalpy associated with the following reaction:
\(\frac{1}{2} H_{2}(g)+\frac{1}{2} F_{2}(g) \rightarrow H F(g) ; \Delta H_{\mathrm{rxn}}=\Delta H_{f}^{\circ}\)