Chapter 9, Problem 81E

Interpretation Introduction

Interpretation:

The standard enthalpy of formation of triflurochlorine needs to be deduced using the following reaction

  ${\text{2ClF}}_{\text{3}}{\text{(g) + 2NH}}_3\text{(g) }\to {\text{ N}}_2{\text{(g) + 6HF(g) + Cl}}_{\text{2}}\text{(g) }\Delta {\text{H}}^0=-1196\text{ kJ}$

Concept Introduction:

The standard enthalpy change for a reaction ${\text{ΔH}}_{\text{R}}^{\text{0}}$ measured at 298 K and 1 atm is given in terms of the difference in the standard enthalpy of formation of the products and that of reactants.

i.e. ${\text{ΔH}}_{\text{R}}^{\text{0}}\text{ = }{\displaystyle \sum {\text{n}}_{\text{p}}{\text{ΔH}}_{\text{f}}^{\text{0}}}\text{(products) - }{\displaystyle \sum {\text{n}}_{\text{r}}{\text{ΔH}}_{\text{f}}^{\text{0}}}\text{(reactants) ------(1)}$

Here,

n_p and n_r are the number of moles of the products and reactants