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Electrolysis - Check your Understanding, Exercises of Chemistry

Chemistry

Exercise to check understanding of material introduced at IB Higher Level for Electrolysis

Typology: Exercises

2021/2022

Uploaded on 11/09/2022

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Chemistry IBH2 Name: …………………………………………………………....
Electrolysis - Check your understanding
1. If an electrolyte conducts electricity, why is a metal not an electrolyte?
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2. Sodium chloride cannot act as an electrolyte when it is in the solid state. Why not?
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3. W and X are metals. Y and Z are non-metals. Which of the following compounds would be expected to act as an
electrolyte? WX2W2Y YZ XZ
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4. Which of the following substances could act as electrolytes? Ethanol (C2H5OH); sodium hydroxide (NaOH);
potassium bromide (KBr); sulphur chloride (SCl2); water (H2O); sugar C6H1206). Explain your answer.
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Chemistry IBH2 Name: …………………………………………………………....

Electrolysis - Check your understanding

  1. If an electrolyte conducts electricity, why is a metal not an electrolyte? ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………...
  2. Sodium chloride cannot act as an electrolyte when it is in the solid state. Why not? ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………...
  3. W and X are metals. Y and Z are non-metals. Which of the following compounds would be expected to act as an electrolyte? WX 2 W 2 Y YZ XZ ………………………………………………………………………………………………………………………...
  4. Which of the following substances could act as electrolytes? Ethanol (C 2 H 5 OH); sodium hydroxide (NaOH); potassium bromide (KBr); sulphur chloride (SCl 2 ); water (H 2 O); sugar C 6 H 1206 ). Explain your answer. ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………...
  1. Draw an electrolytic cell for the electrolysis of copper (II) chloride. Label the anode and cathode. State what is deposited at each electrode and give the half-equations for the reactions occuring.
  2. Write the appropriate half-equations for the reactions that occur at each electrode when the following molten compounds are electrolysed: a. Lead chloride Anode: ………………………………………………………………………………………………………. Cathode: …………………………………………………………………………………………………….. b. Sodium bromide Anode: ………………………………………………………………………………………………………. Cathode: …………………………………………………………………………………………………….. c. Magnesium oxide Anode: ………………………………………………………………………………………………………. Cathode: ……………………………………………………………………………………………………..

b. Sodium bromide with copper electrodes Anode: ………………………………………………………………………………………………………. Cathode: …………………………………………………………………………………………………….. c. Copper sulphate with copper electrode Anode: ………………………………………………………………………………………………………. Cathode: ……………………………………………………………………………………………………..

  1. Two methods can be used to protect iron from rusting, electroplating with a less reactive metal or attaching a more reactive metal. Compare the two methods and evaluate which would be better to prevent a ship’s hull from rusting. ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………... ………………………………………………………………………………………………………………………...
  2. An electrolytic cell produces 235 g of Al(l) according to the equation below. 2Al 2 O 3 (l) + 3C(s) → 4Al(l) + 3CO 2 (g) a. Calculate the number of moles of electrons that must be transferred in the cell to produce the 235 g of Al(l). ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. ………………………………………………………………………………………………………………..

b. Calculate the volume of CO 2 (g), measured at 301 K and 99.7 kPa, that is produced in the process. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. c. For the electrolytic cell to operate, the Al 2 O 3 must be in the liquid state rather than in the solid state. Explain. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. ……………………………………………………………………………………………………………….. When Al(s) is placed in a concentrated solution of KOH at 25°C, the reaction represented below occurs. 2Al(s) + 2OH-(aq) + 6 H 2 O(l) → 2[Al(OH) 4 ]-(aq) + 3H 2 (g) d. The standard reduction potentials for the reaction are shown below. Half-reaction E° (V) [Al(OH) 4 ]-(aq) + 3e-^ ⇌ Al(s) + 4OH-(aq) 2. 2H 2 O(l) + 2e-^ ⇌ H 2 (g) + 2OH-(aq) 0. i. Calculate E°, in volts, for the formation of [Al(OH) 4 ]-(aq) and H 2 (g) at 25°C ………………………………………………………………………………………………………. ………………………………………………………………………………………………………. ………………………………………………………………………………………………………. ………………………………………………………………………………………………………. ii. ΔG°, in kJ/molrxn , for the formation of [Al(OH) 4 ]-(aq) and H 2 (g) at 25°C ………………………………………………………………………………………………………. ………………………………………………………………………………………………………. ………………………………………………………………………………………………………. ……………………………………………………………………………………………………….