First and second ionization enthalpies of lit | vedclass

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Question

(B) The total ionization energy required to convert $1 	ext{ mole}$ of $Li(g)$ to $Li^{2+}(g)$ is the sum of the first and second ionization enthalpi

Vedclass · Accepted Answer

$4$

Vedclass · Answer

(B) The total ionization energy required to convert $1 	ext{ mole}$ of $Li(g)$ to $Li^{2+}(g)$ is the sum of the first and second ionization enthalpies: $IE_{total} = 520 + 7297 = 7817 	ext{ kJ mol}^{-1}$.Given mass of $Li = 3.5 	ext{ mg} = 3.5 	imes 10^{-3} 	ext{ g}$.Molar mass of $Li = 7 	ext{ g mol}^{-1}$.Number of moles of $Li = \frac{3.5 	imes 10^{-3} 	ext{ g}}{7 	ext{ g mol}^{-1}} = 0.5 	imes 10^{-3} 	ext{ mol}$.Total energy required = $	ext{Moles} 	imes IE_{total} = 0.5 	imes 10^{-3} 	ext{ mol} 	imes 7817 	ext{ kJ mol}^{-1} = 3.9085 	ext{ kJ}$.Rounding to the nearest integer, we get $4 	ext{ kJ}$.

Element	$IE_1$	$IE_2$	$IE_3$
$P$	$495.8$	$4562$	$6910$
$Q$	$737.7$	$1451$	$7733$
$R$	$577.5$	$1817$	$2745$

Similar Questions

The first three ionisation energies (in $kJ/mol$) of three representative elements are given below:

Element $IE_1$ $IE_2$ $IE_3$

$P$ $495.8$ $4562$ $6910$

$Q$ $737.7$ $1451$ $7733$

$R$ $577.5$ $1817$ $2745$

Which of the following options is incorrect?

The correct order of ionisation energy of $C$,$N$,$O$,and $F$ is

Which one of the following orders is correct for the first ionisation energies of the elements?

The correct order of first ionisation enthalpy of the given elements is:

The first ionization potential of $Na, Mg, Al$ and $Si$ are in the order:

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