In this experiment you will determine the enthalpy change, $$\(\Delta H_{r}\)$$, for the reaction shown. $$\[ \mathrm{NaOH}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{~g}) \rightarrow \mathrm{NaHCO}_{3}(\mathrm{aq}) \quad \text { enthalpy change }=\Delta H_{\mathrm{r}} \]$$ You will react each of sodium hydroxide and sodium hydrogencarbonate with excess dilute sulfuric acid. You will determine the enthalpy change for each reaction, then use Hess's law to calculate $$\(\Delta H_{r}\)$$. Calculations (i) Calculate the energy change, in J , in your experiment. energy change $$\(=\)$$ .......................... $$\(J\)$$ (ii) Calculate the amount, in mol, of sulfuric acid that reacted with FA 1 in your experiment. $$\[ \text { amount of } \mathrm{H}_{2} \mathrm{SO}_{4}= \]$$ .......................... mol (iii) Calculate the enthalpy change of reaction, $$\(\Delta H_{1}\)$$, in $$\(\mathrm{kJ} \mathrm{mol}^{-1}\)$$ of sulfuric acid, for the neutralisation of $$\(\mathrm{NaOH}(\mathrm{aq})\)$$ with $$\(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\)$$. Show your working. $$\[ \Delta H_{1}=\underset{\text { sign }}{\ldots \ldots \ldots .} \underset{\text { value }}{\ldots \ldots \ldots \ldots \ldots \ldots . . . . . . \mathrm{kJ} \mathrm{mol}^{-1}} \text { of } \mathrm{H}_{2} \mathrm{SO}_{4} \]$$

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