Titanium(IV) chloride can be made from titanium(IV) oxide as shown in the equation. TiO₂(s) + 2C(s) + 2Cl₂(g) → 2CO(g) + TiCl₄(l) ΔH° = -60.0 kJ mol⁻¹ Some entropy data are shown in Table 3. | Substance | S° / J K⁻¹ mol⁻¹ | | ----------- | ----------------- | | TiO₂(s) | 50.2 | | Cl₂(g) | 5.70 | | CO(g) | 223 | | TiCl₄(l) | 253 | Use the equation and the data in Table 3 to calculate the Gibbs free-energy change for this reaction at 989 °C. Give your answer to the appropriate number of significant figures. Use your answer to explain whether this reaction is feasible. [6 marks]

A-Level AQA Chemistry Fundamentals of Acids & Bases: Titanium(IV) chloride can be mad

Titanium(IV) chloride can be made from titanium(IV) oxide as shown in the equation - AQA - A-Level Chemistry - Question 5 - 2017 - Paper 1

Question 5

Titanium(IV) chloride can be made from titanium(IV) oxide as shown in the equation. TiO₂(s) + 2C(s) + 2Cl₂(g) → 2CO(g) + TiCl₄(l) ΔH° = -60.0 kJ mol⁻¹ Some entropy... show full transcript

Worked Solution & Example Answer:Titanium(IV) chloride can be made from titanium(IV) oxide as shown in the equation - AQA - A-Level Chemistry - Question 5 - 2017 - Paper 1

Step 1

Calculate ΔS°

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Answer

To calculate the change in entropy (ΔS°), we use the equation:

$ΔS° = S°_{products} - S°_{reactants}$

Calculating:

$ΔS° = (2 imes 223 ext{ J K}^{-1} ext{ mol}^{-1}) + (253 ext{ J K}^{-1} ext{ mol}^{-1}) - ((50.2 ext{ J K}^{-1} ext{ mol}^{-1}) + (2 imes 5.70 ext{ J K}^{-1} ext{ mol}^{-1}))$

Solving this gives:

$ΔS° = 649 - 507.6 = 141.4 ext{ J K}^{-1} ext{ mol}^{-1}$

Step 2

Calculate Gibbs free energy change (ΔG°)

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Answer

To calculate the Gibbs free energy change (ΔG°), we use the equation:

$ΔG° = ΔH° - TΔS°$

Convert the temperature from Celsius to Kelvin:

$T = 989 + 273.15 = 1262.15 ext{ K}$

Now substituting the values:

$ΔG° = -60.0 ext{ kJ mol}^{-1} - (1262.15 ext{ K} imes (141.4 ext{ J K}^{-1} ext{ mol}^{-1} / 1000))$

Calculating this results in:

$ΔG° = -60.0 - (1262.15 imes 0.1414) ext{ kJ mol}^{-1}$

Calculating yields:

$ΔG° = -60.0 - 178.07 = -238.07 ext{ kJ mol}^{-1}$

Step 3

Explain feasibility of the reaction

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Answer

The Gibbs free-energy change (ΔG°) is negative, which indicates that the reaction is feasible under the specified conditions. A negative ΔG° suggests that the process can occur spontaneously, thus supporting the feasibility of the production of titanium(IV) chloride from titanium(IV) oxide.

Titanium(IV) chloride can be made from titanium(IV) oxide as shown in the equation - AQA - A-Level Chemistry - Question 5 - 2017 - Paper 1

Worked Solution & Example Answer:Titanium(IV) chloride can be made from titanium(IV) oxide as shown in the equation - AQA - A-Level Chemistry - Question 5 - 2017 - Paper 1

Calculate ΔS°

Calculate Gibbs free energy change (ΔG°)

Explain feasibility of the reaction

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