Use the following data to calculate `Delta_("lattice") H^(@)` for NaBr. `Delta_("sub")H^(@)` for sodium metal `=108.4 kJ mol^(-1)`, ionization enthalpy of sodium `=496 kJ mol^(-1)`., electron gain enthalpy of bromine `=-325 kJ mol^(-1)` bond dissociation enthalpy of bromine `=192 kJ mol^(-1) , Delta _f H^(@)` for `NaBr(s) - 360 kJ mol^(-1)`.

Explanation

To calculate the lattice enthalpy (Δ_lattice H^(@)) for NaBr using the Born-Haber cycle, we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Sublimation enthalpy of sodium (Δ_sub H^(@)) = 108.4 kJ/mol
- Ionization enthalpy of sodium (IE) = 496 kJ/mol
- Electron gain enthalpy of bromine (EGE) = -325 kJ/mol
...