Given that the ΔHf^∘ of 1 M H2 SO3 is -633 kJ, use the data in Appendix II, Table B to calculat

step 1 In this question we're going to be looking at the standard enthalpy change of a reaction and the

Given that the ΔHf^∘ of 1 M H2 SO3 is -633 kJ, use the data...

Given that the $\Delta H_{\mathrm{f}}^{\circ}$ of $1 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{3}$ is $-633 \mathrm{~kJ},$ use the data in Appendix II, Table B to calculate the $\Delta H^{\circ}$ for the formation of a $1 \mathrm{M}$ solution of $\mathrm{SO}_{2}$ in water from $\mathrm{SO}_{2}(g)$

Key Concepts

Solution Formation and Solvation Energy

When a gas dissolves in a solvent, additional energy changes occur due to interactions between the solute and solvent molecules, commonly referred to as solvation or hydration. This process is important when calculating the enthalpy of formation for a solution, as the dissolution step contributes to the overall enthalpy change.

Thermodynamic Data and Standard States

Using reliable thermodynamic data, such as tables of standard enthalpies of formation, is essential for accurate calculations. The concept of standard states (e.g., gases at 1 atm, solutes in a specific concentration) provides a consistent framework for these measurements, ensuring that comparisons and calculations are meaningful.

Standard Enthalpy of Formation

This is a measure of the heat change when one mole of a compound is formed from its constituent elements in their standard states. It provides a baseline value that can be used to calculate the overall enthalpy changes for other reactions by serving as a reference point.

Hess’s Law

Hess’s Law states that the total enthalpy change for a chemical reaction is the same regardless of the number of steps or the pathway between the initial and final states. This concept allows one to calculate the overall reaction enthalpy by summing the standard enthalpy of formation values of the products and subtracting those of the reactants.

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