Calculate the energy in joules required to convert all the atoms of sodium to sodium ions present in 2.3 mg of sodium vapours? Ionization enthalpy of sodium is `495 kJ "mol"^(-1 )` (Atomic mass of Na = 23)

Explanation

According to the definition of ionisatino enthalpy,
`Na (g) + IE to Na ^(+) (g) + e ^(-) (g)`
`I.E. = 495kg mol ^(-1)`
The amount of energy needed to ionize 1 mole of sodium vapours `= 495 kJ mol ^(-1)`
Moles of sodium vapours present in given sample
`= (2.3 xx 10 ^(-8))/(23) = 1 xx 10 ^(-4) mol`
`therefore` Amount of energy needed to ionize `1 xx 10^(-4)` mol of sodium vapours
`= 495 xx 1xx 10 ^(-4)`
` =0.0495 kJ or 49.5J`