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प्रश्न
Answer the following in one or two sentences.
Write Nernst equation. What part of it represents the correction factor for nonstandard state conditions?
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उत्तर
1) For any general reaction, aA + bB → cC + dD
Nernst equation is given by
`"E"_"cell" = "E"_"cell"^circ - "RT"/"nF" "ln" (["C"]^"c" ["D"]^"d")/(["A"]^"a" ["B"]^"b")` OR
`"E"_"cell" = "E"_"cell"^circ - (2.303 "RT")/"nF" log_10 (["C"]^"c" ["D"]^"d")/(["A"]^"a" ["B"]^"b")`
where n = moles of electrons used in the reaction, F = Faraday = 96500 C,
T = temperature in kelvin,
R = gas constant = 8.314 J K-1 mol-1
2) The second term in the Nernst equation is the correction for nonstandard state conditions.
Correction factor is `(2.303 "RT")/"nF" log_10 (["C"]^"c" ["D"]^"d")/(["A"]^"a" ["B"]^"b")`
संबंधित प्रश्न
Choose the most correct option.
The standard potential of the cell in which the following reaction occurs:
H2 (g,1 atm) + Cu2+ (1M) → 2H+ (1M) + Cu(s),
`("E"_"Cu"^circ = 0.34 "V")` is
Consider the half reactions with standard potentials.
- \[\ce{Ag^{\oplus}_{ (aq)} + e^{\ominus} -> Ag_{(s)}E^\circ = 0.8 V}\]
- \[\ce{I2_{(s)} + 2e^\ominus -> 2I^{\ominus}_{(aq)} E^\circ = 0.53V}\]
- \[\ce{Pb^{2\oplus}_{(aq)} + 2e^{\ominus} -> Pb_{(s)} E^\circ = -0.13 V}\]
- \[\ce{Fe^{2\oplus} + 2e^{\ominus} -> Fe_{(s)} E^\circ = -0.44 V}\]
The strongest oxidising and reducing agents respectively are ______.
Answer the following in one or two sentences.
Under what conditions the cell potential is called standard cell potential?
Answer the following in brief.
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Answer the following:
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Calculate `"E"_"cell"^circ` of the following galvanic cell:
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`"E"_("Fe"^(2+)//"Fe")^0` = −0.44 V
Identify the strongest reducing agent from the data given below:
| Element | `"E"^0 ("V")` |
| Al | −1.66 |
| Fe | −0.44 |
| Hg | +0.79 |
| Cu | +0.337 |
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For the following cell, standard potential of copper electrode is 0.337 V and standard cell potential is 0.463 V.
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Answer the following in one or two sentences.
What is the standard cell potential for the reaction?
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if \[\ce{E{^{\circ}_{Ni}}}\] = −0.25 V and \[\ce{E{^{\circ}_{Al}}}\] = −1.66 V?
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\[\ce{Zn + Cu^{2+} -> Zn^{2+} + Cu}\],
is 1.10 V at 25°C. The EMF of the cell reaction, when 0.1 M Cu2+ and 0.1 M Zn2+ solutions are used at 25°C is:
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Define standard electrode potential.
Calculate the emf of the following cell at 25°C.
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Write the value of `(2.303 RT)/F` in the Nernst equation?
Write the four applications of emf series.
Standard potential (E°) of
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What is standard potential of reaction
\[2\mathrm{Zn}_{(\mathrm{s})}\longrightarrow2\mathrm{Zn}_{(\mathrm{aq})}^{+2}+4\mathrm{e}^{-}\] ?
If \[\mathrm{E^o\left(Cd_{(aq)}^{+2}|Cd_{(s)}\right)=-0.40~V}\]. What is potential for \[\mathrm{Cd}_{(s)}\xrightarrow{}\mathrm{Cd}_{(aq)}^{+2}\left(0.01\mathrm{M}\right)+2\mathrm{e}^{-}\] at 298 K?
What is the reduction potential of hydrogen gas electrode when pure hydrogen gas is at 1 atmosphere pressure and platinum electrode is in contact with HCI of pH 2 at 298 K?
The cell potential for the following cell notation is approximately:
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`E_(M^(3+)//M)^0` = 0.6 V and `E_(N^(2+)//N)^0` = 0.1 V
Which from following is CORRECT expression for Ecell of following cell?
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