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How much energy in joules must be needed to convert all the atoms of sodiun to sodium ions present in 2.3 mg of sodium vapours? Ionisation enthalpy of sodium is `495 k "mol"^(-1)` (At. mass of Na= 23).

Text Solution

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According to the definition of ionisation enthalpy,
`Na_(g)+I.E to Na_((g))^(+)+e_((g))^(-)`
`I.E= 495 kj mol^(-1)`
The amount of energy needed to ionise 1 mole of sodium vapours = `495 kJ "mol"^(-1)`
Moles of sodium vupour.s present in given sample
`= (2.3 xx10^(-3))/(23)= 1 xx 10^(-4)` mol
`:.` Amount of energy needed to ionise `1 xx 10^(-4)` mole of sodium vapours =` 495 xx 1 xx 10^(-4)`
= 0.0495 kJ or 49.5 J
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