Solution Found!
Calculate ?H0 for the reaction using (a) Equation (9.3)
Chapter 9, Problem 104P(choose chapter or problem)
Calculate \(\Delta H^{\circ}\) for the reaction
\(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{HI}(g)\)
using (a) Equation (9.3) and (b) Equation (6.18), given that \(\Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{I}_{2}(g)\) is 61.0 kJ/mol.
Questions & Answers
QUESTION:
Calculate \(\Delta H^{\circ}\) for the reaction
\(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{HI}(g)\)
using (a) Equation (9.3) and (b) Equation (6.18), given that \(\Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{I}_{2}(g)\) is 61.0 kJ/mol.
ANSWER:Step 1 of 4
Here we are going to find out the bond enthalpy () for the given chemical reaction:
Bond enthalpy:
It is the enthalpy change required to break a particular bond in 1 mole of gaseous atoms.
The enthalpy of gas reaction in the gas phase is given by
………………………..(1)
If the total energy input is greater than the total energy released, () is positive and the reaction is endothermic.
If the total energy input is lesser than the total energy released, () is negative and the reaction is exothermic.