ΔH°rxn (Enthalpy) Is -277.4 kJ/mol.
Enthalpy, a characteristic of a thermodynamic system, is the result of adding the internal energy of the system and the product of its pressure and volume. It is a state function that is frequently employed in measurements of chemical, biological, and physical systems at constant pressure, which the sizable surrounding environment conveniently provides.
The amount of heat released or absorbed during a reaction that takes place under constant pressure is referred to as the enthalpy change. The sign for it is H, which can be read as "ΔH."
CH4(g) + 4Cl2(g) → CCl4(l) + 4HCl(g)
ΔH = ∑(n × ΔH [tex]_{products}[/tex])- ∑(n × ΔH [tex]x_{reactants}[/tex])
n = number of moles
ΔH = ((1−139 kJ/mol) + [1 x (−92.31 kJ/mol)] - [(1 × (−74.87 kJ/mol)] + (1 × 121.0 kJ/mol))
ΔH = -277.4 kJ/mol.
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