Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Co3? (aq) + e? ? Co2? (aq) EĀ° = +1.82 V Cl?(g) + 2e? ? 2Cl?(aq) EĀ° = +1.36 V Ce?? (aq) + e? ? Ce3? (aq) EĀ° = +1.61 V Sn2? (aq) + 2e? ? Sn(s) EĀ° = -0.14 V 2H?(aq) + 2e? ? H?(g) EĀ° = +0.00 V Cu2? (aq) + e? ? Cu?(aq) EĀ° = +0.15 V Ag?(aq) + e? ? Ag(s) EĀ° = +0.80 V Fe3? (aq) + e? ? Fe2? (aq) EĀ° = +0.77 V Sn?? (aq) + 2e? ? Sn2? (aq) EĀ° = +0.13 V Pb2? (aq) + 2e? ? Pb(s) EĀ° = -0.13 V Standard Cell Potential 1.36 V Anode Compartment Cathode Compartment
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Anode (oxidation): Pb(s) -> Pb2+ (aq) + 2e- Cathode (reduction): Cl2 (g) + 2e- -> 2Cl- (aq) ** Show moreā¦
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Use the half-reactions below to produce a voltaic cell with the given standard cell potential: Standard Cell Potential 2H+(aq) + 2e- -> H2(g) EĀ° = +0.00 V Ag+(aq) + e- -> Ag(s) EĀ° = +0.80 V Sn4+(aq) + 2e- -> Sn2+(aq) EĀ° = +0.13 V Cu2+(aq) + e- -> Cu+(aq) EĀ° = +0.15 V Fe3+(aq) + e- -> Fe2+(aq) EĀ° = +0.77 V Cl2(g) + 2e- -> 2Cl-(aq) EĀ° = +1.36 V Sn2+(aq) + 2e- -> Sn(s) EĀ° = -0.14 V Pb2+(aq) + 2e- -> Pb(s) EĀ° = -0.13 V Zn2+(aq) + 2e- -> Zn(s) EĀ° = -0.76 V Co3+(aq) + e- -> Co2+(aq) EĀ° = +1.82 V Anode Compartment Cathode Compartment
Ivan K.
Given the following two half-reactions, write the overall reaction in the direction in which it is spontaneous (a working Voltaic cell) and calculate the standard cell potential. (Note: only one answer and no partial credit) Fe3+(aq) + e- ā Fe2+(aq) EĀŗ = + 0.771 V Pb2+(aq) + 2 e- ā Pb(s) EĀŗ = ā 0.126 V Pb(s) + 2 Fe3+(aq) ā Pb2+(aq) + 2 Fe2+(aq) EĀŗcell = + 0.897 V Pb2+(aq) + Fe2+(aq) ā Pb(s) + Fe3+(aq) EĀŗcell = + 0.645 V Pb(s) + 2 Fe3+(aq) ā Pb2+(aq) + 2 Fe2+(aq) EĀŗcell = + 1.416 V Pb2+(aq) + 2 Fe2+(aq) ā Pb(s) + 2 Fe3+(aq) EĀŗcell = + 0.897 V Pb(s) + Fe3+(aq) āPb2+(aq) + Fe2+(aq) EĀŗcell = + 0.645 V None of the above
Suman K.
Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. 2 Ag+(aq) + Pb(s)-2 Ag(s) + Pb2+(aq) b. 2 ClO2(g) + 2 I-(aq)-2 ClO2-(aq) + I2(s) c. O2(g) + 4 H+(aq) + 2 Zn(s)-2 H2O(l) + 2 Zn2+(aq)
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