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Equilibrium Constant from Nernst Equation

A cell utiliz...

Question

A cell utilizes the following reaction
$2 C o_{a q}^{3 +} + Z n (s) ⇌ 2 C o^{2 +} (a q) + Z n^{2 +} (a q)$
Choose the correct statement

E_{c e l l}

decreases when Co (II) nitrate is dissolved in cathode compartment.

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E_{c e l l}

increases when Co (III) nitrate is dissolved in cathode compartment.

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E_{c e l l}

is doubled when the area of the zinc electrode is doubled.

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E_{c e l l}

increases when additional water is added to the anode compartment.

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Solution

The correct options are
A $E_{c e l l}$ decreases when Co (II) nitrate is dissolved in cathode compartment.
B $E_{c e l l}$ increases when Co (III) nitrate is dissolved in cathode compartment.
D $E_{c e l l}$ increases when additional water is added to the anode compartment.
$E_{c e l l} : E_{c e l l}^{0} - \frac{0.059}{2} l o g \frac{[C o^{2 +}] [Z n^{2 +}]}{[C o^{3 +}]^{2}},$ Electrode area does not affect $E_{c e l l}$

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Similar questions

Z n | Z n^{2 +} | | C u^{2 +} | C u

E_{c e l l} = 1.1 v o l t

1.1 V

Z n

C u

Z n | Z n^{2 +} | | C u^{2 +} | C u

E_{c e l l} = 1.1 V

Z n (s) + C u^{2 +} (a q .) ⇌ C u (s) + Z n^{2 +} (a q .)

Q = \frac{[Z n^{2 +}]}{[C u^{2 +}]}

E_{c e l l}

Q

O A = 1.10 v o l t . E_{c e l l} = 1.1591 v o l t

Z n + C u^{2 +} (a q) ⇌ C u + Z n^{2 +} (a q)

Q = \frac{[Z n^{2 +}]}{[C u^{2 +}]}

E_{c e l l}

V . E_{c e l l}

1.1591 V

Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s)

E_{c e l l}

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