1. | \(2 \mathrm{CuSO}_{4}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s}) \rightarrow 2 \mathrm{Cu}(\mathrm{s})+\mathrm{Ag}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \) |
2. | \(\mathrm{CuSO}_{4}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \) \(\rightarrow \mathrm{ZnSO}_{4}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s}) \) |
3. | \(\mathrm{CuSO}_{4}(\mathrm{aq})+\mathrm{Fe}(\mathrm{s}) \) \(\rightarrow \mathrm{FeSO}_{4}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s}) \) |
4. | \(\mathrm{FeSO}_{4}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \) \(\rightarrow \mathrm{ZnSO}_{4}(\mathrm{aq})+\mathrm{Fe}(\mathrm{s}) \) |
The standard electrode potential (E°) values of Al3+/ Al, Ag+ / Ag, K+ / K, and Cr3+ / Cr are –1.66 V, 0.80 V, –2.93 V, & –0.79 V respectively. The correct decreasing order of the reducing power of the metal is:
1. | Ag > Cr > Al > K | 2. | K > Al > Cr > Ag |
3. | K > Al > Ag > Cr | 4. | Al > K > Ag > Cr |
Standard reduction potentials of the half-reactions are given below:
The strongest oxidizing and reducing agents, respectively, are:
1. and
2. and
3. and
4. and
A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+/Fe2+ is +0.77 V and E° for I2/2I– = 0.536 V.
The favourable redox reaction is:
1. Fe2+ will be oxidized to Fe3+.
2. I2 will be reduced to I–.
3. There will be no redox reaction.
4. I– will be oxidized to I2.
The strongest oxidizing agent in the above equation is:
1.
2.
3.
4.
Standard electrode potentials are:
,
Choose the correct observation if , and Fe block are kept together:
1. increases
2. decreases
3. remains unchanged
4. decreases