Advertisements
Advertisements
प्रश्न
Cell equation: \[\ce{A + 2B^- -> A^{2+} + 2B}\]
\[\ce{A^{2+} + 2e^- -> A}\] E0 = +0.34 V and log10 k = 15.6 at 300 K for cell reactions find E0 for \[\ce{B^+ + e^- -> B}\]
पर्याय
0.80
1.26
– 0.54
– 10.94
Advertisements
उत्तर
0.80
Explanation:
\[\ce{A + 2B^- -> A^{2+} + 2B}\]
Half reaction anode: \[\ce{A -> A^2+ + 2e^-}\]
`"E"_"ox"^0` = –0.34 V ........[Given: \[\ce{A^{2+} + 2e^- -> A}\] E0 = +0.34 V]
Cathode: \[\ce{2B^+ + 2e^- -> 2B}\] `"E"_"red"^0` = ?
log10 K = 156; T = 300 K; n = 2;
F = 96500 C
R = 8.314 JK−1 mol−1
∆G° = – 2.303 RT log K
∴ nFE° = – 2.303 RT log K
`"E"_"cell"^0 = (2.303 "RT" log "K")/("nF")`
= `(2.303 xx 8.314 xx 300 xx 15.6)/(2 xx 96500)`
= 0.4643 V
`"E"_"cell"^0 = "E"_"ox"^0 + "E"_"red"^0`
`"E"_"red"^0 = "E"_"cell"^0 + "E"_"ox"^0`
∴ 0.4643 – (–0.34)
= 0.4643 + 0.34
= 0.8043
= 0.80 V
APPEARS IN
संबंधित प्रश्न
Define cathode
Describe the electrolysis of molten NaCl using inert electrodes.
Two metals M1 and M2 have reduction potential values of −xV and +yV respectively. Which will liberate H2 and H2SO4.
Which of the following statement is correct?
`E_(cell)^Θ` for some half cell reactions are given below. On the basis of these mark the correct answer.
(a) \[\ce{H^{+} (aq) + e^{-} -> 1/2 H_2 (g); E^Θ_{cell} = 0.00V}\]
(b) \[\ce{2H2O (1) -> O2 (g) + 4H^{+} (aq) + 4e^{-}; E^Θ_{cell} = 1.23V}\]
(c) \[\ce{2SO^{2-}_{4} (aq) -> S2O^{2-}_{8} (aq) + 2e^{-}; E^Θ_{cell} = 1.96V}\]
(i) In dilute sulphuric acid solution, hydrogen will be reduced at cathode.
(ii) In concentrated sulphuric acid solution, water will be oxidised at anode.
(iii) In dilute sulphuric acid solution, water will be oxidised at anode.
(iv) In dilute sulphuric acid solution, \[\ce{SO4^{2-}}\] ion will be oxidised to tetrathionate ion at anode.
For the given cell, \[\ce{Mg | Mg^{2+} || Cu^{2+} | Cu}\]
(i) \[\ce{Mg}\] is cathode
(ii) \[\ce{Cu}\] is cathode
(iii) The cell reaction is \[\ce{Mg^+ Cu^{2+} -> Mg^{2+} + Cu}\]
(iv) \[\ce{Cu}\] is the oxidising agent
What is electrode potential?
If the value of Ksp for Hg2Cl2 (s) is X then the value of X will be ____ where pX = - log X.
Given:
\[\ce{Hg2Cl2 + 2e- -> 2Hg(l) + 2Cl-}\], E° = 0.27 V
\[\ce{Hg+2 + 2e- -> 2Hg(l)}\] E° = 0.81 V
In a solution of CuSO4, how much time will be required to precipitate 2 g copper by 0.5 ampere current?
The two half cell reaction of an electrochemical cell is given as
\[\ce{Ag+ + e- -> Ag}\], `"E"_("Ag"^+//"Ag")^circ` = - 0.3995 V
\[\ce{Fe^{2+} -> Fe^{3+} + e-}\], `"E"_("Fe"^{3+}//"Fe")^{2+}` = - 0.7120 V
The value of EMF will be ______.
