You visited us 1 times! Enjoying our articles? Unlock Full Access!

Gibb's Energy and Nernst Equation

For the diagr...

Question

For the diagram above, which statement is true about the setup shown?

The electrode potential for this cell is 1.40 V

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

The electrode potential for this cell is 2.54 V

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Electrons will be carried by the salt bridge

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Ions will be carried through the wire

No worries! We‘ve got your back. Try BYJU‘S free classes today!

The reaction is nonspontaneous

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A The electrode potential for this cell is 1.40 V
The electrode potential for this cell is 1.40 V
$E_{c e l l}^{0} = E_{N i}^{0} - E_{A l}^{0} = - 0.26 - (- 1.66) = 1.40$ V
Ions will be carried by the salt bridge
Electrons will be carried through the wire
The reaction is spontaneous as the standard cell potential is positive.

Suggest Corrections

Similar questions

2 A g^{+} + C d \to 2 A g + C d^{2 +}

A g^{+} \to A g

C d^{2 +} \to C d

0.80 v o l t

- 0.40 v o l t

E^{\circ}

p H = 3

C u^{2 +} + 2 e^{-} \to C u

n [C u^{2 +}]

E_{r e d}

- \frac{0.34 \times 4}{0.0591}

C u / C u^{2 +} (0.1 M)

S n^{4 +} / S n

C r^{3 +} / C r

2 A

5 V

0.5 Ω

10 V

Join BYJU'S Learning Program