# The energy of one mole of photons of radiation whose frequency is $1\times 10^{14}Hz$  Option 1) $39.85\times 10^{3}\:J/mol$ Option 2) $39.90 \times10^{3}\:KJ/mol$ Option 3) $398.5 \times10^{3}\:J/mol$ Option 4) $3.985 \times10^{6}\:J/mol$

P Prateek Shrivastava

As we learned in concept

The energy (E) of a quantum of radiation -

$E=hv$

Where h is plank’s constant and $\nu$ is frequency

-

E=hv

Energy with one mole of photons

= $N_{A}\:(hv)$

= $6.022\times W^{23}\times6.626\times10^{-34}\times1\times10^{14}\:Jmol^{-1}$

= $39.9\times10^{3}\:Jmol^{-1}$

$\sim 39.85\times10^{3}\:Jmol^{-1}$

Option 1)

$39.85\times 10^{3}\:J/mol$

This option is correct.

Option 2)

$39.90 \times10^{3}\:KJ/mol$

This option is incorrect.

Option 3)

$398.5 \times10^{3}\:J/mol$

This option is incorrect.

Option 4)

$3.985 \times10^{6}\:J/mol$

This option is incorrect.

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