Use the information below to answer this question. $\text{NaHCO}_3(s) + \text{HCl}(aq) \rightarrow \text{NaCl}(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g)$, $\Delta H = -38.97\ \text{kJ mol}^{-1}$ $\text{Na}_2\text{CO}_3(s) + 2\text{HCl}(aq) \rightarrow 2\text{NaCl}(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g)$, $\Delta H = -96.59\ \text{kJ mol}^{-1}$ When heated, sodium hydrogencarbonate breaks down as follows. $2\text{NaHCO}_3(s) \rightarrow \text{Na}_2\text{CO}_3(s) + \text{H}_2\text{O}(l) + \text{CO}_2(g)$ Determine the enthalpy change for this decomposition?
- A$-57.62\ \text{kJ mol}^{-1}$
- B$-18.65\ \text{kJ mol}^{-1}$
- C$18.65\ \text{kJ mol}^{-1}$
- D$57.62\ \text{kJ mol}^{-1}$