How much energy in joules must be needed to convert all the atoms of sodium to sodium ions present in 4.6 mg of sodium vapours? Ionization enthalpy of sodium is 495 `"kJ mol"^(-1)`

Explanation

`underset((495kJ mol^(-1))(Na(g)+IE_(1) to Na^(+) (g)+e^(-))`
Moles of sodium vapours in the given sample `=(4.6 xx 10^(-3))/(23)=2 xx 10^(-4)"mol"`
Amount of energy needed to convert 1 mole of sodium vapours into ions =495 kJ
Amount of energy needed to convert `2 xx 10^(-4)` mole of sodium vapours into ions `=495 xx 2 xx 10^(-4)=0.0990kJ`