b. If we assume that the specific heat of the solution is 1.0 cal/g · °C, calculate the ΔHsol for this compound in kcal/g and in kcal/mol. Show your work.

1. Break Down the Problem

To calculate the enthalpy change of solution (ΔHsol) for the compound, we need to consider the following:

1. The specific heat of the solution: $1.0 \, \text{cal/g} \cdot \degree \text{C}$
2. Conversion from calories to kilocalories.
3. The mass of the solution and the temperature change during the dissolution (assuming these values are given or will be specified).

2. Relevant Concepts

The formula to calculate ΔHsol when you have a temperature change is: $\Delta H_{\text{sol}} = \frac{q}{n}$ Where:

• $q$ is the heat absorbed or released (in calories).
• $n$ is the number of moles of the solute.

The relationship to convert calories to kilocalories is: $1 \, \text{kcal} = 1000 \, \text{cal}$

3. Analysis and Detail

Assuming we have a given mass $m$ of the solution and a temperature change $\Delta T$:

• Calculate $q$ using specific heat: $q = m \cdot c \cdot \Delta T$ Where:

• $c = 1.0 \, \text{cal/g} \cdot \degree \text{C}$

• Convert $q$ from calories to kilocalories: $q_{\text{kcal}} = \frac{q}{1000}$

• If $M$ is the molar mass of the solute and $m$ is the mass of the solute: $n = \frac{m}{M}$

• Finally, calculate $\Delta Hsol$ in kcal/g and in kcal/mol. $\Delta H_{\text{sol (kcal/g)}} = \frac{q_{\text{kcal}}}{m}$ $\Delta H_{\text{sol (kcal/mol)}} = \frac{q_{\text{kcal}}}{n}$

4. Verify and Summarize

Confirm that all values are in the correct units and that no steps were skipped in converting values. Summarize the results as follows:

Final Answer

• $\Delta H_{\text{sol (kcal/g)}} = \text{(calculated value in kcal/g)}$
• $\Delta H_{\text{sol (kcal/mol)}} = \text{(calculated value in kcal/mol)}$

(Note: Specific values of mass, temperature change, and molar mass were not provided in the question, so the final numerical values cannot be calculated without those inputs.)