Electrochemistry Quiz 3 – Punjab Meritorious School Preparation Portal

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Gibb's equation

Gibb's-Helmholtz equation

Nernst equation

Van der Waal's equation

+0.3

0.5

1.5

-0.5

The standard cell potential of Zn | Zn²⁺ (aq) ||Cu²⁺ (aq) |Cu cell is 1.10 V. The maximum work obtained by this cell will be

106.15 kJ

– 212.30 kJ

-318.45 kJ

-424.60 kJ

Adding powered lead and iron to a solution that is 1.0 M in both Pb²⁺ and Fe²⁺ ions, would result in a reaction, in which:

A hydrogen electrode is immersed in a solution with pH = 0 (HCI). By how much will the potential (reduction) change if an equivalent amount of NaOH is added to the solution. (Take pH₂= 1atm), T=298 K

Increase by 0.41 V

Increase by 59 mV

Decrease by 0.41 V

Decrease by 59 mV

1.006 V

0.503 V

0.235 V

-0.235 V

An electrochemical cell is set up as: Pt; H₂(1 atm) | HCI (0.1 M) || CH₃COOH (0.1 M) | H₂(latm); Pt. The e.m.f of this cell will not be zero, because

the temperature is constant

e.m.f depends on molarities of acids used

acids used in two compartments are different

pH of 0.1 M HCl and 0.1 M CH3COOH is not same

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

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