Periodicity in atomic properties

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Question

How much energy will be needed to convert 2.5 mol of Li atoms in the gaseous state to form Li (g)? First I.P of Li= 5.41 eV.

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Solution

I.P. of Li = 5.41 eV ${atom}^{-}$
$\begin{array}{l} \times \frac{6.023 \times 10^{23} \times 1.602 \times 10^{- 19} {Jmol}^{-}}{1 eV {atom}^{-}} \\ = 522 \times 10^{3} J {mol}^{-} \end{array}$
$∴$ Energy needed to convert 2.5 mol Li (s) to Li (g)
$\begin{array}{l} = 2.5 mol \times 522 \times 10^{3} J {mol}^{-} \\ = 1305 kJ \end{array}$

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Periodicity in atomic properties

Remember concepts with our Masterclasses.

How much energy will be needed to convert 2.5 mol of Li atoms in the gaseous state to form Li (g)? First I.P of Li= 5.41 eV.

I.P. of Li = 5.41 eV atom-×6.023×1023×1.602×10−19Jmol−1eV atom −=522×103Jmol−∴ Energy needed to convert 2.5 mol Li (s) to Li (g) =2.5mol×522×103Jmol−=1305kJ

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