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Redox Reaction

Q. Consider the following half-reactions: Cl2(g) + 2e^- → 2 Cl^-(aq) 1.360V Cu^2+(aq) + 2e^- → Cu(s) 0.337V Mg^2+(aq) + 2e^- →Mg(s) -2.370 V (6) Which species can be reduced by Cu(s)? If none leave blank.

Solved • Apr 1, 2020

Redox Reaction

Q. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Mn metal and I2(s), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.

Solved • Apr 1, 2020

Redox Reaction

Q. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Zn metal and Cl2(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.

Solved • Apr 1, 2020

Redox Reaction

Q. Consider the following half-reactions: Cl2(g) + 2e^- → 2 Cl^-(aq) 1.360V Cu^2+(aq) + 2e^- → Cu(s) 0.337V Mg^2+(aq) + 2e^- →Mg(s) -2.370 V (4) The strongest reducing agent is:

Solved • Apr 1, 2020

Redox Reaction

Q. Consider the following half-reactions: Cl2(g) + 2e^- → 2 Cl^-(aq) 1.360V Cu^2+(aq) + 2e^- → Cu(s) 0.337V Mg^2+(aq) + 2e^- →Mg(s) -2.370 V (3) The weakest reducing agent is:

Solved • Apr 1, 2020

Redox Reaction

Q. Consider the following half-reactions: Br2(l) + 2e^- → 2Br^- (aq) 1.080V 2H^+ (aq) + 2e^- → H2(g) 0.000V Fe^2+ (aq) + 2e^- → Fe(s) -0.440V (6) Which species can be reduced by H2(g)? If none, leave box blank.

Solved • Apr 1, 2020

Redox Reaction

Q. Consider the following half-reactions: (4) The weakest reducing agent is:

Solved • Apr 1, 2020