a) $2Cl^-_{(aq)} \rightarrow 2e^- + Cl_{2(g)}$
b) Products: Oxygen and water
When dilute sodium chloride is used, hydroxide ions are discharged and not chloride.
johnmulu answered the question on May 15, 2017 at 08:59
- The set-below was used by a student to investigate the products formed when aqueous copper (II) chloride was electrolyzed using carbon electrodes(Solved)
The set-below was used by a student to investigate the products formed when aqueous copper (II) chloride was electrolyzed using carbon electrodes
i) Write the equation for the reaction that takes place at the cathode.
ii) Name and describe a chemical test for the product initially formed at the anode when a highly concentrated solution of copper (II) chloride is electrolyzed.
iii) How would the mass of the anode change if the carbon anode was replaced with copper metal? Explain.
Date posted: May 15, 2017. Answers (1)
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The set-up below (Figure 2) was used to electrolyse a bromide of metal D, DBr2.
a) Write the equation for the reactions at the I. Cathode II. Anode
b) The electrodes used in the experiment were made of carbon and metal D. Which of the two electrodes was used as the anode? Give a reason
c) Give a reason why this experiment is carried out in a fume cupboard.
Date posted: May 15, 2017. Answers (1)
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The diagram below represents a set up that can be used to electrolyze aqueous copper (II) sulphate.
i) describe s how oxygen gas is produced during the electrolysis.
ii) Explain why copper electrodes are not suitable for this electrolysis.
Date posted: May 15, 2017. Answers (1)
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The diagram below represents an experiment that was set up to investigate movement of ions during electrolysis.
When the circuit was completed, it was noticed that a blue colour spread towards the right.
a) Explain this observation.
b) Write the equation for the reaction that occurred at the anode.
Date posted: May 15, 2017. Answers (1)
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The diagram below shows the apparatus that can be used to electrolyze acidified water obtain hydrogen and oxygen gases. Study it and answer the questions that follow.
i) Identify the electrode at which oxidation takes place.
ii) Give a reason why it is necessary to acidify the water.
iii) Explain why hydrochloric acid is not used to acidify the water.
Date posted: May 15, 2017. Answers (1)
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The diagram below represents a diagram cell used to electrolyse pure brine.
i) Name: I. Product at U
II. Another material that can be used instead of titanium
III. The impurity present in the product at U.
ii) State two functions of the diaphragm
iii) Give one industrial use of the product at U.
Date posted: April 27, 2017. Answers (1)
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The diagram below represents the set-up that was used tom study the effect of an electric current on pure water and dilute sulphuric (VI) acid.
State and explain the observation made when each experiment was started.
Date posted: April 27, 2017. Answers (1)
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The set-up below was used to electrolyse molten lead (II) iodine
i) State the observation that was made at the anode during the electrolysis. Give a reason for your answer.
ii) A current of 0.5 A was passed for two hours. Calculate the mass of lead that was deposited (pb = 2071F = 9, 500C)
Date posted: April 27, 2017. Answers (1)
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An electric current was passed through a concentrated solution of copper (II) chloride as shown in the diagram below.
i) Explain the observation that would be made on the electrolyte as the experiment progresses
ii) Which of the electrodes is the anode? Explain.
Date posted: April 27, 2017. Answers (1)
- The table below gives standard electrode potentials for the metals represented by the letters D, E, F and G. Study it and answer the questions that follow.(Solved)
The table below gives standard electrode potentials for the metals represented by the letters D, E, F and G. Study it and answer the questions that follow.
Which metal can be displaced from a solution of its salt by all the other metals in the table? Give a reason.
Date posted: April 27, 2017. Answers (1)
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Study the flow chart below and answer the questions that follow:
a) Identify substance:
i) A
ii) B
b) Name process C.
c) Give one use of PVC.
Date posted: April 27, 2017. Answers (1)
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The set-up below was used to electroplate a metallic spoon. Study it and answer the questions that follow.
a) Write an ionic equation for the reaction that occurred at the cathode
b) State and explain what happened to the anode.
Date posted: April 27, 2017. Answers (1)
- 100 cm3 of 2 M sulphuric (VI) acid was electrolyzed using the set-up represented by the diagram below(Solved)
100 cm3 of 2 M sulphuric (VI) acid was electrolyzed using the set-up represented by the diagram below
i) Write an equation for the reaction that produces gas L.
ii) Describe how gas K can be identified
iii) Explain the difference in:
I. The volume of the gases produced at the electrodes.
II. Brightness of the bulb if 100 cm3 of 2 M ethanoic acid was used in place of sulphuric (VI) acid.
Date posted: April 27, 2017. Answers (1)
- The diagram below represents a mercury cell that can be used in the industrial manufacture of sodium hydroxide. Study it and answer the questions that follow.(Solved)
The diagram below represents a mercury cell that can be used in the industrial manufacture of sodium hydroxide. Study it and answer the questions that follow.
i) Name
I. The raw material introduced at 2
II. another substance that can be used in the cell instead of graphite.
ii) Identify the by – product that comes out at 1
iii) Give
I. One use of sodium hydroxide
II. Two reasons why mercury is recycled.
Date posted: April 27, 2017. Answers (1)
- The set-up below was used during the electrolysis of aqueous magnesium sulphate using inert electrodes.(Solved)
The set-up below was used during the electrolysis of aqueous magnesium sulphate using inert electrodes.
a) Name a suitable pair of electrodes for this experiment.
b) Identify the anions and cations in the solution.
c) Explain the change that occurred to the concentration of magnesium sulphate solution during the experiment
Date posted: April 27, 2017. Answers (1)
- The set –up below was used to electrolyse aqueous copper (II) sulphate.(Solved)
The set –up below was used to electrolyse aqueous copper (II) sulphate.
a) Explain why the bulb light brightly at the beginning of the experiment and becomes dim after sometimes.
b) Write the ionic equation of the reaction that took place at the cathode.
Date posted: April 27, 2017. Answers (1)
- Study the diagram below and answer the questions that follow.(Solved)
Study the diagram below and answer the questions that follow.
When some hydrogen chloride gas is allowed into water and the mixture stirred, the bulb lights and gases X and Y are formed.
i) Name: gas X and gas Y
ii) Explain why the bulbs does not light before the hydrogen chloride gas is let into water
Date posted: April 27, 2017. Answers (1)
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A solution of hydrogen was allowed to decompose and the oxygen gas given off collected. After 5 minutes, substance G was added to the solution of hydrogen peroxide. The total volume of oxygen evolved was plotted against time as shown in the graph below
i) Describe the procedure of determining the rate of the reaction at minute 12.
ii) How does the production of oxygen in region AB compare with that in region BC? Explain.
Date posted: April 27, 2017. Answers (1)
- The curve below shows the variation of time against temperature for the reaction between sodium thiosulphate and hydrochloric acid(Solved)
The curve below shows the variation of time against temperature for the reaction between sodium thiosulphate and hydrochloric acid
Explain the shape of the curve.
Date posted: April 27, 2017. Answers (1)
- The curves below represents the change in mass when equal masses of powdered zinc and zinc granules were reacted with excess 2 M hydrochloric acid. Study them and answer the question below(Solved)
The curves below represents the change in mass when equal masses of powdered zinc and zinc granules were reacted with excess 2 M hydrochloric acid. Study them and answer the question below
Which curve represents the reaction with zinc granules? Explain answer.
Date posted: April 27, 2017. Answers (1)