Advertisements
Advertisements
प्रश्न
Represent the cell in which the following reaction takes place.The value of E˚ for the cell is 1.260 V. What is the value of Ecell?
\[\ce{2Al (s) + 3Cd^{2+} (0.1M) -> 3Cd (s) + 2Al^{3+} (0.01M)}\]
उत्तर
Al(s) /Cd2+ (0.1M) // Al3+ (0.01M) /Cd(s)
\[\ce{2Al(s) + 3Cd^{2+} (0.1M) -> 3Cd (s) + 2Al^{3+} (0.01M)}\]
Ecell = E°cell `(- 0.059)/n log [Al^(3+}]^2/([Cd^(2+)]^3`
Ecell = `1.26 - 0.059/6 log (0.01)^2/(0.1)^3`
= `1.26 - 0.059/6 (- 1)`
= 1.26 + 0.009
= 1.269 V
APPEARS IN
संबंधित प्रश्न
Arrange the following reducing agents in the order of increasing strength under standard state conditions. Justify the answer
|
Element |
Al(s) |
Cu(s) |
Cl(aq) |
Ni(s) |
|
Eo |
-1.66V |
0.34V |
1.36V |
-0.26V |
Can copper sulphate solution be stored in an iron vessel? Explain.
Calculate e.m.f of the following cell at 298 K:
2Cr(s) + 3Fe2+ (0.1M) → 2Cr3+ (0.01M) + 3 Fe(s)
Given: E°(Cr3+ | Cr) = – 0.74 VE° (Fe2+ | Fe) = – 0.44 V
Calculate emf of the following cell at 25 °C :
Fe|Fe2+(0.001 M)| |H+(0.01 M)|H2(g) (1 bar)|Pt (s)
E°(Fe2+| Fe)= −0.44 V E°(H+ | H2) = 0.00 V
Given the standard electrode potentials,
\[\ce{K+/K}\] = −2.93 V, \[\ce{Ag+/Ag}\] = 0.80 V,
\[\ce{Hg^{2+}/Hg}\] = 0.79 V
\[\ce{Mg^{2+}/Mg}\] = −2.37 V, \[\ce{Cr^{3+}/Cr}\] = −0.74 V
Arrange these metals in their increasing order of reducing power.
Depict the galvanic cell in which the reaction \[\ce{Zn(s) + 2Ag+(aq) → Zn^{2+}(aq) + 2Ag(s)}\] takes place. Further show:
- Which of the electrode is negatively charged?
- The carriers of the current in the cell.
- Individual reaction at each electrode.
Which cell will measure standard electrode potential of copper electrode?
Use the data given in below find out which of the following is the strongest oxidising agent.
`"E"_("Cr"_2"O"_7^(2-)//"Cr"^(3+))^⊖`= 1.33 V `"E"_("Cl"_2//"Cl"^-)^⊖` = 1.36 V
`"E"_("MnO"_4^-//"Mn"^(2+))^⊖` = 1.51 V `"E"_("Cr"^(3+)//"Cr")^⊖` = - 0.74 V
Consider the figure and answer the following question.
If cell ‘A’ has ECell = 0.5V and cell ‘B’ has ECell = 1.1V then what will be the reactions at anode and cathode?
The potential of a hydrogen electrode at PH = 10 is
