Redox Equilibrium

Laboratory Activity 1H (Purification of Metals by Electrolysis):Aim: To study the purification of copper by electrolysis. Materials: 1.0 mol dm−3 of copper(II) nitrate, Cu(NO3)2 solution, impure copper plate and pure copper plate. Apparatus: Beaker, battery, connecting wires with crocodile clips, ammeter and switch. Procedure:1. Pour 1.0 mol dm−3 of copper(II) nitrate, Cu(NO3)2 solution into a beaker … Read more

Laboratory Activity 1G (Electroplating of Metals by Electrolysis) :Aim: To study the electroplating of an iron spoon with copper. Materials: 1.0 mol dm−3 of copper(II) sulphate, CuSO4 solution, iron spoon, copper plate and sandpaper. Apparatus: Beaker, battery, connecting wires with crocodile clips, ammeter, switch and rheostat. Procedure:1. Clean the copper plate and iron spoon with … Read more

Activity 1J:Carry out the activity in groups. 1. Carefully study the electrolytic cell in Figure 1.31 (a) and Figure 1.31 (b). 2. Based on Figures 1.31 (a) and 1.31 (b), discuss:(a) the products formed on each electrode.(b) half equations for each electrode.(c) changes in the products if the concentrations of the electrolyte is changed to … Read more

Experiment 1C (The Effects of Type of Electrode on the Selection of Ions to be Discharged) :Aim: To study the effects of the type of electrode used on the selective discharge of ions at the electrodes. Problem statement: Does the type of electrode used affect the selective discharge of ions at the electrodes? Hypothesis: Construct … Read more

Experiment 1B (The Effects of Concentrations of Ions in Solutions on the Selective Discharge of Ions) :Aim: To study the effects of the concentrations of ions in hydrochloric acid, HCl on the selective discharge of ions at the electrode. Problem statement: Does the concentration of hydrochloric acid, HCl affect the selection of ions to be … Read more

Laboratory Activity 1F (Electrolysis of an Aqueous Solution Using Carbon Electrodes):Aim: To study the electrolysis of the aqueous solution of copper(II) sulphate, CuSO4 and dilute sulphuric acid, H2SO4 with carbon electrodes. Materials: 0.1 mol dm−3 of copper(II) sulphate, CuSO4 solution and 0.1 mol dm−3 of sulphuric acid, H2SO4 Apparatus: Electrolytic cell, battery, carbon electrodes, connecting … Read more

Activity 1l :1. Using a suitable thinking map, predict the observation and explain how the products of electrolysis are formed at the anode and cathode for:(a) molten zinc oxide, ZnO.(b) molten magnesium chloride, MgCl2. Answer: (a)(b)

Laboratory Activity 1E (Electrolysis of Molten Lead(II) bromide, PbBr2):Aim: To study the electrolysis of molten lead(II) bromide, PbBr2. Material: Lead(II) bromide powder, PbBr2. Apparatus: Beaker, crucible, light bulb, battery, carbon electrodes, connecting wire with crocodile clip, switch, tripod stand, pipe clay triangle and Bunsen burner. Procedure:1. Fill a crucible with lead(II) bromide powder, PbBr2 until … Read more

Activity 1H:Compounds can be classified into electrolytes and non-electrolytes. How do you prove a substance is an electrolyte or non-electrolyte? 1. Carry out this activity in pairs. 2. Each group will choose one substance X to be investigated. Substance X provided are as follows: (a) Solid copper(II) chloride, CuCl2(b) Solid glucose, C6H12O6(c) Solid oxalic acid, … Read more

Question 1:Write the cell notation for the following voltaic cells:$$ \begin{aligned} & \mathrm{Sn}^{2+} / \mathrm{Sn} \text { and } \mathrm{Mg}^{2+} / \mathrm{Mg} . \\ & \mathrm{Cl}_2 / \mathrm{Cl}^{-} \text {and } \mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+} . \end{aligned} $$ Answer:(a)$$ \operatorname{Mg}(\mathrm{s})\left|\mathrm{Mg}^{2+}(\mathrm{aq})\right|\left|\mathrm{Sn}^{2+}(\mathrm{aq})\right| \operatorname{Sn}(\mathrm{s}) $$ (b)$$ \operatorname{Pt}(\mathrm{s})\left|\mathrm{Cl}^{-}(\mathrm{aq}), \mathrm{Cl}_2(\mathrm{aq})\right|\left|\mathrm{MnO}_4^{-}(\mathrm{aq}), \mathrm{Mn}^{2+}(\mathrm{aq})\right| \operatorname{Pt}(\mathrm{s}) $$ Question 2:Calculate the voltage for the following cells:$$ … Read more