Consider the following half cell reactions Zn 2 aq 2 e Zns E o 076 V Cu2 aq 2 e

Consider the following half cell reactions zn 2 aq 2

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4.Consider the following half-cell reactions:Zn2+(aq)+ 2 e-Zn(s);Eo= -0.76 VCu2+(aq)+ 2 e-Cu(s);Eo= 0.34 V 2
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Chem 1B Chapter 18 Exercises (a) Sketch a voltaic cell consisting of Zn(s)|ZnSO4(aq)and Cu(s)|CuSO4(aq)half-cells using Na2SO4as salt-bridge. Label the following: (i) the anode and cathode half-cells; (ii) the positive and negative electrodes; (iii) the direction electron flows in the circuit and ions flow in the salt bridge.(b) Write the cell notation for the voltaic cell. (c) Write net ionic equation for: (i) anode half-cell reaction; (ii) cathode half-cell reaction, and (iii) the overall cell reaction. (d) Calculate standard cell potential (Ecell) at 25oC and the Ecellwhen the concentrations are [Zn2+] = 1.0 Mand [Cu2+] = 0.0010 (e) What is the value of Gofor the overall reaction at 25 oC? (f) Calculate the maximum free energy available for work if 5.0 g of zinc is reacted at an average cell potential of 1.00 V? o M Answer : o 5.Consider the following standard reduction (half-cell) potentials:Al3+(aq)+ 3e-Al(s);Eo= -1.66 VCu2+(aq)+ 2e-Cu(s);Eo= +0.34 V(a) Sketch a voltaic cell consisting of the above half-cells using KNO3as salt-bridge. Label the following: (i) the anode and cathode half-cells; (ii) the positive and negative electrodes; (iii) the direction electron flows in the circuit and ions flow in the salt bridge. (b) Write the net equation for the overall cell reaction and calculate the standard cell potential (Eocell) at 25oC. (c) Calculate Gofor the overall reaction at 25 oC. (d) How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum at an average cell potential of 2.00 V? E o G
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