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How much energy in joules must be needed...

How much energy in joules must be needed to convert all the atoms of sodium to sodium ions present in 2.3 mg of sodium vapours ?
Given : Ionisation energy of sodium is 495 kJ `"mol"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
49.5
According to the definition of ionisation energy,
` Na(g) + IE to Na^(+) (g) +e^(-), 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 vapours present in given sample
`=(2.3 xx 10^(-3))/23 = 1 xx 10^(-4)`mol L
`therefore` Amount of energy needed to ionise `1 xx 10^(-4)` moles of sodium vapours `= 495 xx 10^(-4)` kJ/mol = 49.5 J/mol
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