Redox Equilibrium

Question 6:Figure 2 shows a set-up of apparatus for a voltaic cell. With reference to the half-cell standard electrode potential, E0:(a) identify the negative and positive terminals.(b) write the cell notation for the chemical cell.(c) write the equations for reduction, oxidation and the overall ionic equation.(d) calculate the voltage of the cell. Answer:(a) Negative terminal … Read more

Question 3:Figure 1 shows the set-up of apparatus and observation for the experiment to study displacement of a metal from its salt solution.(a) Suggest a suitable X(NO3)2 solution and name the brown solid at the bottom of the test tube.(b) Write the half equations for oxidation and reduction.(c) Write the ionic equation for the redox … Read more

Question 1:Identify whether a redox reaction occurs for each reaction below.Explain your answer based on the change in oxidation number. Answer:Reaction I is a redox reaction. – The oxidation number of iron before the reaction is +2 and after the reaction is 0.– The oxidation number of magnesium before the reaction is 0 and after … Read more

Question 1:Figure 1.43 shows the observation of two experiments to study the effects of metals P and Q on rusting of iron.(a) Suggest metals P and Q.(b) Explain and include the half equations for the reactions in experiment I and experiment II.(c) Arrange iron, metal P and metal Q in an ascending order of electropositivity. … Read more

Activity 1M:Conduct this activity in groups.1. Discuss and explain the following situation:(a) What is the difference between rusting of iron and metal corrosion?(b) Describe the mechanisms for rusting from the aspects of oxidation and reduction.(c) How can metals that are more electropositive than iron prevent rusting of iron? State examples of application in daily life … Read more

Experiment 1E (Effects of Other Metals on Rusting) :Aim: To study the effects of other metals on rusting.Problem statement: How do different metals in contact with iron affect rusting?Hypothesis: When a more electropositive metal comes into contact with an iron nail, the iron does not rust; when a less electropositive metal comes into contact with … Read more

Experiment 1D (Corrosion of Metal that Occurs on Copper and Iron):Aim: To study the corrosion of copper and iron.Problem statement: Do copper and iron undergo corrosion?Hypothesis: Corrosion of copper metal produces blue precipitate and corrosion of iron metal produces brown precipitate.Variables:(a) Manipulated variable : Copper and iron.(b) Responding variable : Presence of blue and brown … Read more

Question 1:Name a metal that exists as an element. Answer:Silver and aurum. Question 2:Explain why aluminium cannot be extracted through reduction reaction by carbon. Answer:– Aluminium is more reactive than carbon in the reactivity series of metals.– Reaction between aluminium oxide and carbon does not occur.– Carbon cannot reduce aluminium oxide. Question 3:Iron is extracted … Read more

Activity 1L (Discussion):Carry out this activity in groups.1. Scan the QR code to watch a video on aluminium extraction by electrolysis.2. Based on the information in the video, discuss:(a) the ionic equation for the reaction.(b) the overall chemical equation involved.(c) whether the extraction of aluminium is a redox reaction?Write your discussion in your notebook. Answer:(2)(a)During … Read more

Question 1:Table 1.11 shows electrodes, electrolytes and observations at the anode for three electrolytic cells.(a) Name the anions present in copper(II) chloride, CuCl2 solution.(b) State the name of the gases released at the anode in electrolytic cells I and II.Explain your answers.(c)(i) Write the half equation for the reaction that occurs at the anode of … Read more