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Enthalpy changes

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Question 1

A student plans to determine the enthalpy change of reaction 1 shown below:

Na2O(s)+2HCl(aq)→2NaCl(aq)+H2O(l)reaction 1 \text{Na}_2\text{O(s)} + 2\text{HCl(aq)} \rightarrow 2\text{NaCl(aq)} + \text{H}_2\text{O(l)} \quad \text{\textbf{reaction 1}} Na2​O(s)+2HCl(aq)→2NaCl(aq)+H2​O(l)reaction 1

This enthalpy change can be determined indirectly using Hess' Law from the enthalpy changes of reaction 2 and reaction 3 shown below:

Na2O(s)+H2O(l)→2NaOH(aq)reaction 2 \text{Na}_2\text{O(s)} + \text{H}_2\text{O(l)} \rightarrow 2\text{NaOH(aq)} \quad \text{\textbf{reaction 2}} Na2​O(s)+H2​O(l)→2NaOH(aq)reaction 2 HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)ΔrH=−57.6 kJ mol−1reaction 3 \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \quad \Delta_r H = -57.6 \text{ kJ mol}^{-1} \quad \text{\textbf{reaction 3}} HCl(aq)+NaOH(aq)→NaCl(aq)+H2​O(l)Δr​H=−57.6 kJ mol−1reaction 3

The student determines the enthalpy change of reaction 2 using a polystyrene cup calorimeter as outlined below:

  • Weigh a bottle containing Na2O(s)\text{Na}_2\text{O(s)}Na2​O(s) and weigh a polystyrene cup.
  • Add about 30 cm330\text{ cm}^330 cm3 of water to the polystyrene cup and measure its temperature.
  • Add the Na2O(s)\text{Na}_2\text{O(s)}Na2​O(s), stir the mixture, and measure the maximum temperature reached.
  • Weigh the empty bottle and weigh the polystyrene cup with the final solution.

Mass readings

  • Mass of bottle + Na2O(s)\text{Na}_2\text{O(s)}Na2​O(s) = 18.45 g18.45\text{ g}18.45 g
  • Mass of empty bottle = 16.90 g16.90\text{ g}16.90 g
  • Mass of empty polystyrene cup = 23.40 g23.40\text{ g}23.40 g
  • Mass of polystyrene cup + final solution = 54.40 g54.40\text{ g}54.40 g

Temperature readings

  • Initial temperature of water = 21.0 ∘C21.0\text{ }^{\circ}\text{C}21.0 ∘C
  • Maximum temperature of final solution = 58.5 ∘C58.5\text{ }^{\circ}\text{C}58.5 ∘C

The density and specific heat capacity, ccc, of the solution are the same as for water (c=4.18 J g−1 K−1c = 4.18\text{ J g}^{-1}\text{ K}^{-1}c=4.18 J g−1 K−1).

a.

Calculate the enthalpy change of reaction 2 (in kJ mol−1\text{kJ mol}^{-1}kJ mol−1) and the enthalpy change of reaction 1 (in kJ mol−1\text{kJ mol}^{-1}kJ mol−1). Show your working.

[6]
b.

The uncertainty in each temperature reading is ±0.1 ∘C\pm 0.1\text{ }^{\circ}\text{C}±0.1 ∘C. The uncertainty in each mass reading is ±0.005 g\pm 0.005\text{ g}±0.005 g. Determine whether the mass of Na2O\text{Na}_2\text{O}Na2​O or the temperature change has the greater percentage uncertainty. Show your working.

[3]
c.

Suggest a modification to this experiment, using the same apparatus, which would reduce the percentage errors in the measurements. Explain your reasoning.

[2]
d.

Sodium oxide, Na2O\text{Na}_2\text{O}Na2​O, can be prepared by the redox reaction of NaNO3\text{NaNO}_3NaNO3​ and sodium metal. Nitrogen gas is also formed. (i) What is the systematic name for NaNO3\text{NaNO}_3NaNO3​?

[1]
e.

(ii) Using oxidation numbers, with signs, show the element that is oxidised and the element that is reduced in this reaction.

[2]
f.

(iii) Construct the balanced chemical equation for this reaction.

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Enthalpy changes Questions

  1. A Level
  2. /Chemistry
  3. /Enthalpy changes