A piece of copper metal is placed in a test tube containing a solution of silver

Question

A piece of copper metal is placed in a test tube containing a solution of silver nitrate and left overnight ure a). The next day, a white precipitate appeared, and the solution is now light blue (Figure b). Highlight the correct component in each of the boxes that will best explain what happened in this spontaneous oxidation-reduction reaction. Cu(s) or Ag(s) reacts with Ag(aq) or Cu(aq) ions to produce Cu(s) or Ag(s) and Ag(aq) or Cu(aq) ions. As the silver gets | oxidized or reduced . it accumulates on the copper piece. The solution turns a blue color due to the oxidation or reduction of the copper. To highlight the correct answer, click on each box, and click and drag on the correct answer (should turn blue color) To erase, select clear from the highlight options, then click and drag on what you want to erase.

Explanation / Answer

1. Ag(s) reacts with Cu2+ ions to produce Cu(s) and Ag+(aq) ions. As the silver gets reduced, it accumulates on the copper piece. The solution turns a blue color due to the oxidation of the copper.

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2.a. Data.

2 Ag(s) + H2S(g) ==> Ag2S(s) + H2(g)

This redox reaction can be reversed adding Al in presence of water, as follows;

3 Ag2S + 2 Al + 6 H2O ==> 6 Ag + 2 Al(OH)3 + 3 H2S

2.b. Data

Standard potentials of reduction:

Ag+ + 1e- => Ag ; +0.80 v

Al3+ + 3e- => Al ; -1.66 v

E° = E°cat - E°ano = 0.80 - (-1.66)

E° = 2.46 V

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