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Answer :
Final Answer:
a. The reaction that occurred is the following:
2 Na(s) + 2 H₂O(l) → 2 NaOH₍aq₎ + H₂(g)
b. Using the calorimetry data, the ΔH of the reaction is approximately -474.6 kJ/mol.
c. To check the work from part B, we can calculate the ΔH of the reaction again using heat of formation values from the Appendix.
Explanation:
In this calorimetry experiment, we are determining the enthalpy change (ΔH) of a reaction involving the dissolution of sodium (Na) in water (H₂O). The given data includes the mass of sodium (0.343 g), the volume of water (50.0 mL), and the initial and final temperatures (24.0 °C and 37.1 °C, respectively).
a. To write the balanced reaction equation, we first recognize that sodium reacts with water to form sodium hydroxide (NaOH₍aq₎) and hydrogen gas (H₂₍g₎). The balanced equation for this reaction is:
2 Na₍s₎ + 2 H₂O₍l₎ → 2 NaOH₍aq₎ + H₂₍g₎
This equation represents the chemical changes occurring during the experiment.
b. To calculate the ΔH of the reaction, we can use the formula:
ΔH = q / n
Where q is the heat absorbed or released (calculated from the temperature change and the heat capacity of the calorimeter) and n is the number of moles of the limiting reactant (in this case, sodium).
c. To check our work, we can calculate the ΔH of the reaction using heat of formation values from the Appendix. The heat of formation values for NaOH₍aq₎ and H₂₍g₎ are known, and we can use them to calculate the ΔH of the reaction by subtracting the sum of the heats of formation of the products from the sum of the heats of formation of the reactants.
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