A constant pressure calorimeter consists of an insulated beaker of mass `92g` made up of glass with heat capacity `0.75 J K^(-1) g^(-1)`. The beaker contains `100 mL` of `1M HCI` at `22.6^(@)C` to which `100 mL` of `1M NaOH` at `23.4^(@)C` is added. The final temperature after the reactions is complete is `29.3^(@)C`, What is `DeltaH` per mole for this neutralization reaction? Assume that the heat capacities of all solutions are equal that of same volumes of water.

Explanation

To find the ΔH per mole for the neutralization reaction between HCl and NaOH, we will follow these steps:

### Step 1: Calculate the moles of H⁺ and OH⁻ ions
- **Moles of H⁺ from HCl**:
\[ \text{Moles of H⁺} = \frac{100 \, \text{mL}}{1000} \times 1 \, \text{mol/L} = 0.1 \, \text{mol} \]

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