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Standard XII

Chemistry

Nernst Equation

If the 0.05 m...

Question

If the 0.05 molar solution of $M^{+}$ is replaced by 0.0025 molar $M^{+}$ solution, then the magnitude of the cell potential would be:

35 mV

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70 mV

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140 mV

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700 mV

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Solution

The correct option is D 140 mV
From above equation $\frac{2.303 R T}{F} = 0.0538$
So, $E_{c e l l} = E_{c e l l}^{o} - \frac{0.0538}{1} log 0.0025$
$= 0 - \frac{0.0538}{1} log 0.0025$ $\approx 0.13988 V$ $\approx 140 m V$

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If the 0.05 molar solution of M+ is replaced by 0.0025 molar M+ solution, then the magnitude of the cell potential would be:

The correct option is D 140 mVFrom above equation 2.303RTF=0.0538So, Ecell=Eocell−0.05381log0.0025=0−0.05381log0.0025≈0.13988V≈140mV

If the 0.05 molar solution of $M^{+}$ is replaced by 0.0025 molar $M^{+}$ solution, then the magnitude of the cell potential would be:

The correct option is D 140 mV
From above equation $\frac{2.303 R T}{F} = 0.0538$
So, $E_{c e l l} = E_{c e l l}^{o} - \frac{0.0538}{1} log 0.0025$
$= 0 - \frac{0.0538}{1} log 0.0025$ $\approx 0.13988 V$ $\approx 140 m V$