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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

 

Answers (1)

best_answer

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.

Posted by

prateek

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