Advertisements
Advertisements
प्रश्न
Can copper sulphate solution be stored in an iron vessel? Explain.
Advertisements
उत्तर
Higher the standard reduction potential (Eº) value, greater the tendency of the species to accept electrons and undergo reduction.
Cu2++2e-→Cu, Eº = + 0.337 V ; Fe2+ + 2e- → Fe, Eº = - 0.440 V
Therefore, Cu2+ has a greater tendency to undergo reduction than Fe2+ or Fe can reduce (or displace) Cu2+ ions from its salt solution.
Fe(s) +Cu2(aq) → Fe2(aq) + Cu(s)
Hence, copper sulphate solution cannot be stored in an iron vessel as the iron vessel dissolves forming Fe2+ ions and Cu2+ ions from copper sulphate solution forms Cu.
APPEARS IN
संबंधित प्रश्न
Draw a neat and well labelled diagram of primary reference electrode.
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 |
Calculate E°cell for the following reaction at 298 K:
2Al(s) + 3Cu+2(0.01M) → 2Al+3(0.01M) + 3Cu(s)
Given: Ecell = 1.98V
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
Calculate e.m.f. and ∆G for the following cell:
Mg (s) |Mg2+ (0.001M) || Cu2+ (0.0001M) | Cu (s)
`"Given :" E_((Mg^(2+)"/"Mg))^0=−2.37 V, E_((Cu^(2+)"/"Cu))^0=+0.34 V.`
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.
In the representation of the galvanic cell, the ions in the same phase are separated by a _______.
Calculate the emf of the following cell at 25°C :
Standard electrode potential is measured taking the concentrations of all the species involved in a half-cell is ____________.
Standard hydrogen electrode operated under standard conditions of 1 atm H2 pressure, 298 K, and pH = 0 has a cell potential of ____________.
Which cell will measure standard electrode potential of copper electrode?
The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ______.
Using the data given below find out the strongest reducing 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
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
Which reference electrode is used to measure the electrode potential of other electrodes?
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?
Which is the correct order of second ionization potential of C, N, O and F in the following?
Standard electrode potential of three metals X, Y and Z are –1.2 V, +0.5 V and –3.0 V, respectively. The reducing power of these metals will be ______.
The potential of a hydrogen electrode at PH = 10 is
Standard reduction potentials (E°) of Cd2+, respectively which is the strongest reducing agent
