(a) The table below shows the standard reduction potentials for four half cells Study it and answer the questions that follow. Number Half-reaction Evolts I Ag_((aq))^++2e^-leftharpoons Ag_((s)) +0.80 II Cu^2+_((aq))+2e^-=Cu_((s)) +0.34 III Pb^2+_((aq))+2e^-leftharpoons Pb_((s)) -0.13 N Zn^2+_(aq))+2e^2+Zn_((s)) -0.76 (i) - Identify the strongest reducing agent (1 mark) Predict whether or not a solution of copper (II) nitrate can be stored d in a container made of lead (2 marks) In the space provided draw a labeled diagram of the electrochemical cell that would give the hest emf. (3 marks) (iv) Calculate the E'' of the electrochemical cell constructed in (iii) above (1 mark)

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(a) The table below shows the standard reduction potentials for four half cells Study it and answer the questions that follow. Number Half-reaction Evolts I Ag_((aq))^++2e^-leftharpoons Ag_((s)) +0.80 II Cu^2+_((aq))+2e^-=Cu_((s)) +0.34 III Pb^2+_((aq))+2e^-leftharpoons Pb_((s)) -0.13 N Zn^2+_(aq))+2e^2+Zn_((s)) -0.76 (i) - Identify the strongest reducing agent (1 mark) Predict whether or not a solution of copper (II) nitrate can be stored d in a container made of lead (2 marks) In the space provided draw a labeled diagram of the electrochemical cell that would give the hest emf. (3 marks) (iv) Calculate the E'' of the electrochemical cell constructed in (iii) above (1 mark)

Answer 1

(i) The strongest reducing agent is the one with the most negative reduction potential. From the table, the half-reaction with the most negative reduction potential is the one for zinc (Zn), which is -0.76 V. Therefore, Zn is the strongest reducing agent. (ii) To predict whether a solution of copper (II) nitrate can be stored in a container made of lead, we need to compare the standard reduction potentials of the two metals. The standard reduction potential of lead (Pb) is -0.13 V, while the standard reduction potential of copper (Cu) is +0.34 V. Since the standard reduction potential of copper is more positive than that of lead, copper is more reactive than lead. Therefore, a solution of copper (II) nitrate can be stored in a container made of lead without any reaction occurring. (iii) To draw a labeled diagram of the electrochemical cell that would give the highest emf, we need to connect the half-reactions with the most positive and most negative reduction potentials. In this case, the half-reaction with the most positive reduction potential is copper (Cu), and the half-reaction with the most negative reduction potential is zinc (Zn). Therefore, we would connect the copper half-reaction to the cathode and the zinc half-reaction to the anode. (iv) To calculate the emf of the electrochemical cell, we need to sum up the standard reduction potentials of the two half-reactions. The standard reduction potential of the copper half-reaction is +0.34 V, and the standard reduction potential of the zinc half-reaction is -0.76 V. Therefore, the emf of the electrochemical cell is +0.34 V - 0.76 V = -0.42 V.

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