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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)

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Solution :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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