The E °in the given diagram is,

What is cell entropy change of the following cell?

Pt(s) | H₂ (g) | CH₃ COOH, HCl || KCl (aq) |Hg₂ Cl₂ | (s) | Hg

P = 1 atm        0.1M               0.1M

Emf of the cell is found to be 0.045 V at 298 K and temperature coefficient is  

3.4 x10^–4  VK^–1

Given Ka _(CH3COOH) = 10^–5 M

Following cell has EMF 0.7995 V.

Pt | H₂ (1 atm) | HNO₃ (1M) || AgNO₃ (1M) | Ag

If we add enough KCl to the Ag cell so that the final Cl^- is 1M. Now the measured emf of the cell is 0.222 V.

The K_sp of AgCl would be :

The solubility of [Co(NH₃ )₄ Cl₂ ] CIO₄ _________ if the  = 50,  = 70, and the measured resistance was 33.5 Ω in a cell with cell constant of 0.20 is ____.

We have taken a saturated solution of AgBr.K_sp  of AgBr is 12 x 10 ^–14  . If 10  ^–7  mole of AgNO₃  are added to 1 litre of this solution then the conductivity of this solution in terms of  10  ^–7  Sm  ^–1  units will be

[given    Sm²  mol^-1   Sm²   mol^-1 , 5 x 10^-3   Sm² mol^-1 ]

At 298K the standard free energy of formation of H₂ O(L) is –237.20kJ/mole while that of its ionisation into H⁺ ion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be

 H₂ (g,1 bar) | H⁺ (1M) || OH^– (1M) | O₂ (g, 1bar)

Which of the following cell can produce more electric work.

A hydrogen electrodes is immersed in a solution with pH = 0 (HCl). By how much will the potential (reduction) change if an equivalent amount of NaOH is added to the solution. (Take P_H2 = 1 atm) T = 298 K.

At what  does the following cell have its reaction at equilibrium?

 Ag(s) | Ag₂ CO₃ (s) | Na₂ CO₃ (aq) || KBr(aq) | AgBr(s) | Ag(s)

 K_SP = 8 x  10 ^–12 for  Ag₂ CO₃ and K_SP = 4 x  10 ^–13 for AgBr

Calculate the EMF of the cell at 298 K

Pt|H₂ (1atm)|NaOH(xM),NaCl(xM)|AgCl(s)|Ag

If E °_cl-/AgCl/Ag  = + 0.222 V