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Energy required for the excitation of H-...

Energy required for the excitation of H-atom its ground state to the `2^(nd)` excited state is `2.67` times smaller than dissociation energy of `H_(2)(g)`. If `H_(2)(g)` placed in `1.0` litre flask at `27^(@)C`and `1.0` bar is to be excited to their `2^(nd)` excited state, what will be the total energy consumption?

Text Solution

Verified by Experts

The correct Answer is:
`21.8kJ`
`E_(ext)=2.18xx10^(-19)(1-(1)/(9))xx6.023xx10^(23)=116.71kJ//molH`
`D.E.=116.71xx2.67=311.62 " "kJ//molH_(2)`
`n=(PV)/(RT)=(1)/(0.082xx300)=0.04`
`implies T.E.=0.04xx311.62+0.08xx116.71=21.8kJ`
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