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प्रश्न
What is the effect of catalyst on: Gibbs energy (∆G)
What is the effect of adding a catalyst on Gibbs energy (ΔG) of a reaction?
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उत्तर
There will be no effect of catalyst on Gibbs energy hence, it catalyses the spontaneous reactions but does not catalyse non-spontaneous reactions
संबंधित प्रश्न
Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution :
`Ag^+(aq)+e^(-)rarrAg(s)" "" "" "E^@=+0.80V`
`H^+(aq)+e^(-)rarr1/2H_2(g)" "" "" " E^@=0.00V`
On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why ?
Calculate ΔrG° for the reaction
Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s)
Given : E°cell = + 2.71 V, 1 F = 96500 C mol–1
Write any ‘two’ advantages of calomel electrode.
Potential of saturated calomel electrode is-
For the reaction
`2AgCl (s) + H_2 (g) ("1 atm") -> 2Ag (s) + 2H^(+) (0.1 M) + 2Cl^(-) (0.1 M)`
`triangleG^0 = -43600 J at 25^@ C`
Calculate the e.m.f. of the cell
`[log 10^(-n) = -n]`
The equilibrium constant at 25°C for the given cell is:
Zn | Zn2+ (1M) | | Ag+ (1M) |
Ag is ______ × 1052.
Given that
\[\ce{E^0_{Zn/Zn^{2+}}}\] = 0.76 V
and \[\ce{E^0_{Ag/Ag^{+}}}\] = −0.80 V
The e.m.f. of cell Zn | ZnSO4 | | CuSO4 | Cu at 25°C is 0.03 V and the temperature coefficient of e.m.f. is −1.4 × 10−4 V/K. The heat of reaction for the change taking place inside the cell is ______ kJ/mol.
The cell potential for the following cell
\[\ce{Pt|H2 (g)| H+ (aq)||Cu^{2+} (0.01 M)| Cu(s)}\]
is 0.576 Vat 298 K. The pH of the solution is ____. (Nearest integer)
The standard Gibbs energy for the given cell reaction in kJ mol-1 at 2'98 K is:
\[\ce{Zn(s) + Cu^{2+} (aq) -> Zn^{2+} (aq) + Cu(s)}\]
E° = 2 V at 298 K
(Faraday's constant, F = 96000 C mol-1)
For a spontaneous reaction, the ΔG, equilibrium constant (K) and `"E"_"cell"^circ` will be respectively.
