Part A - Daniell Cell Select the best description of reactions that occur in the
ID: 1021289 • Letter: P
Question
Part A - Daniell Cell
Select the best description of reactions that occur in the Daniell Cell.
D. Zinc ions (Zn2+) are reduced to Zn metal at electrode a and Cu metal is oxidized to Copper ions (Cu2+) ions at electrode b.
Part B Galvanic Cells
The right-hand half-cell contains a dissolved salt MX. M(s) is oxidized to M+(aq) during the oxidation reaction that occurs in this half-cell. In what direction do the electrons move through the external circuit, and what kind of reaction occurs in the left-hand half-cell.
A. Electrons move from right to left through the external circuit, and a reduction reaction occurs in the left-hand half-cell.
B. Electrons move from left to right through the external circuit, and a oxidation reaction occurs in the left-hand half-cell.
C. Electrons move from right to left through the external circuit, and an oxidation reaction occurs in the left-hand half-cell.
D. Electrons move from left to right through the external circuit, and a reduction reaction occurs in the left-hand half-cell.
Part C Hydrogen Fuel Cell
The following reaction occurs in a hydrogen fuel cell (see above):
2H2(g) + O2(g) ? 2H2O(l)
What is oxidized, and what is reduced during this reaction?
The following reaction occurs in a hydrogen fuel cell (see above):
2H2(g) + O2(g) ? 2H2O(l)
What is oxidized, and what is reduced during this reaction?
A. H2 is reduced and O2 is oxidized.
B. H2O is reduced.
C. H2 is oxidized and O2 is reduced.
D. This is not and oxidation-reduction reaction.
E. H2 is oxidized, but nothing is reduced.
Part D
Based upon the half-cell potentials given above which of the following reactions will be spontaneous?
Based upon the half-cell potentials given above which of the following reactions will be spontaneous?
A. Fe(s) + Cu2+(aq) ? Fe2+(aq) + Cu(s)
B. Fe(s) + Cu(s) ? Cu2+(aq) + Fe2+(aq)
C. Cu2+(aq) + Fe2+(aq) ? Cu(s) + Fe(s)
D. Fe2+(aq) + Cu(s) ? Fe(s) + Cu2+(aq)
A. Zn metal is oxidized to Zinc ions (Zn2+) at electrode a and Cu metal is oxidized to Copper ions (Cu2+) ions at electrode b. B. Zinc ions (Zn2+) are oxidized to Zn metal at electrode a and Cu metal is reduced to Copper ions (Cu2+) ions at electrode b. C. Zn metal is oxidized to Zinc ions (Zn2+) at electrode a and Copper ions (Cu2+) ions are reduced to Cu metal at electrode b.D. Zinc ions (Zn2+) are reduced to Zn metal at electrode a and Cu metal is oxidized to Copper ions (Cu2+) ions at electrode b.
Part B Galvanic Cells
The right-hand half-cell contains a dissolved salt MX. M(s) is oxidized to M+(aq) during the oxidation reaction that occurs in this half-cell. In what direction do the electrons move through the external circuit, and what kind of reaction occurs in the left-hand half-cell.
A. Electrons move from right to left through the external circuit, and a reduction reaction occurs in the left-hand half-cell.
B. Electrons move from left to right through the external circuit, and a oxidation reaction occurs in the left-hand half-cell.
C. Electrons move from right to left through the external circuit, and an oxidation reaction occurs in the left-hand half-cell.
D. Electrons move from left to right through the external circuit, and a reduction reaction occurs in the left-hand half-cell.
Part C Hydrogen Fuel Cell
The following reaction occurs in a hydrogen fuel cell (see above):
2H2(g) + O2(g) ? 2H2O(l)
What is oxidized, and what is reduced during this reaction?
The following reaction occurs in a hydrogen fuel cell (see above):
2H2(g) + O2(g) ? 2H2O(l)
What is oxidized, and what is reduced during this reaction?
A. H2 is reduced and O2 is oxidized.
B. H2O is reduced.
C. H2 is oxidized and O2 is reduced.
D. This is not and oxidation-reduction reaction.
E. H2 is oxidized, but nothing is reduced.
Part D
Based upon the half-cell potentials given above which of the following reactions will be spontaneous?
Based upon the half-cell potentials given above which of the following reactions will be spontaneous?
A. Fe(s) + Cu2+(aq) ? Fe2+(aq) + Cu(s)
B. Fe(s) + Cu(s) ? Cu2+(aq) + Fe2+(aq)
C. Cu2+(aq) + Fe2+(aq) ? Cu(s) + Fe(s)
D. Fe2+(aq) + Cu(s) ? Fe(s) + Cu2+(aq)
2e Zn2+ Cu+Explanation / Answer
Part A: C, Zn metal is oxidized to Zinc ions (Zn2+) at electrode a and Copper ions (Cu2+) ions are reduced to Cu metal at electrode b.
Part B: A, Electrons move from right to left through the external circuit, and a reduction reaction occurs in the left-hand half-cell. (Since it is clearly given that on right side oxidation is taking place which means electrons is being released there)
Part C: C, H2 is oxidized and O2 is reduced (Since H2 is releasing electron to become H+ and O2 is receiving to become O2- and combining with H+ to form water.
Part D: A, Fe(s) + Cu2+(aq) Fe2+(aq) + Cu(s) (Reduction potential chart shows that Cu2+ will be readily reduced compared to Fe2+ therefore this reaction would be spontaneous)