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  • The energy required to ionise all atoms present in sample of magnesium to <img alt="\mathrm{Mg^{2+}}" src="/latex-image/?%5Cmat

The energy required to ionise all atoms present in \mathrm{12 g} sample of magnesium to \mathrm{Mg^{2+}} ions if \mathrm{ IE_1\: and\: IE_2} of magnesium are \mathrm{737.7 kJ mol^{-1} \: and \, 1450.7 kJ mol^{-1}}
respectively

Option: 1

\mathrm{1094.2kJ }


Option: 2

\mathrm{26260.8 kJ}
 


Option: 3

\mathrm{2188.7kJ }


Option: 4

None of the above


Answers (1)

best_answer

Moles of Magnesium in \mathrm{12 g} sample \mathrm{= 12/24 = 0.5}

\mathrm{mol \: Mg \rightarrow Mg^{+} + e^{-} ; IE_1 = 737.7 kJ/mol}

\mathrm{Mg^{+} \rightarrow Mg^{2+} + e^{-}; IE_2 = 1450.7 kJ/mol}

Then, \mathrm{Mg \rightarrow Mg^{2+} + e^{-}; IE = IE_1 + IE_2 = 2188.4 kJ/mol}

For 1 mol, it requires 2188.7 mol so for 0.5 mol, the require energy shall be \mathrm{1094.2 kJ}

Hence option 1 is correct.

Posted by

SANGALDEEP SINGH

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