Question

Given thatH2(g) + F2(g) -> 2HF(g) => ∆H = -546.6 kJ . mol-12H2(g) + O2(g) -> 2H20(l) => ∆H = -571.6 kJ. mol-1

Calculate the value of ∆H for:2F2(g) + 2H20(l) -> 4HF(g) + O2(g)

Answer 1

Answer: The $\Delta H^o_{rxn}$ for the reaction is -521.6 kJ.

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The chemical equation for the reaction of fluorine and water follows:

$2F_2(g)+2H_2O(l)\rightarrow 4HF(g)+O_2(g)$   $\Delta H^o_{rxn}=?$

The intermediate balanced chemical reaction are:

(1) $H_2(g)+F_2(g)\rightarrow 2HF(g)$    $\Delta H_1=-546.6kJ$    ( × 2)

(2) $H_2(g)+O_2(g)\rightarrow 2H_2O(g)$    $\Delta H_2=-571.6kJ$

The expression for enthalpy of reaction follows:

$\Delta H^o_{rxn}=[2\times \Delta H_1]+[1\times (-\Delta H_2)]$

Putting values in above equation, we get:

$\Delta H^o_{rxn}=[(2\times (-546.6))+(1\times (571.6))]=-521.6kJ$

Hence, the $\Delta H^o_{rxn}$ for the reaction is -521.6 kJ.