4.4 CHAPTER 4. ELECTROCHEMICAL REACTIONS
Exercise 4 - 4
- In your own words, explain what is meant bythe ’electrode potential’of a metal.
- Give the standard electrode potential for eachof the following metals:
(a) magnesium
(b) lead
(c) nickel- Refer to the electrodepotentials in table ??.
(a) Which of the metalsis most likely to be oxidised?
(b) Which metal is most likely to be reduced?
(c) Which metal is the strongest reducing agent?
(d) In the copper half-reaction, does the equilibrium position for the reaction
lie to the left or to the right? Explain your answer.
(e) In the mercury half-reaction, does the equilibrium position for the reaction
lie to the left or to the right? Explain your answer.
(f) If silver was added toa solution of copper sulphate, would it displacethe
copper from the coppersulphate solution? Explain your answer.- Use the table of standard electrode potentials to put the following inorder from
the strongest oxidising agent to the weakest oxidising agent.- Cu2+
- MnO− 4
- Br 2
- Zn2+
- Look at the followinghalf-reactions.
- Ca2++ 2e−→ Ca
- Cl 2 + 2e−→ 2Cl
- Fe3++ 3e−→ Fe
- I 2 + 2e−→ 2I−
(a) Which substance isthe strongest oxidising agent?
(b) Which substance isthe strongest reducing agent?- Which one of the substances listed below acts as the oxidising agent in the fol-
lowing reaction?
3SO 2 + Cr 2 O^27 −+ 2H+→ 3SO^24 −+ 2Cr3++ H 2 O(a) H+
(b) Cr3+
(c) SO 2