The energy required to convert all atoms present in 1.2 g magnesium to Mg 2+ ions if IE 1, and IE 2 of magnesium are 120 kJ mol -1 and 240 kJ mol -1 respectively

Question

The energy required to convert all atoms present in 1.2 g magnesium to Mg 2+ ions if IE 1, and IE 2 of magnesium are 120 kJ mol -1 and 240 kJ mol -1 respectively (A) 18 kJ (B) 36 kJ (C) 360 kJ (D) 24 kJ

Tardigrade Admin · Accepted Answer

Moles of Mg =(1.2/24)=0.05 moL Mg longrightarrow Mg 2++2 e - I.E. =I. E 1+ I .E 2=120+240 1 moL xrightarrow text energy required =360 kJ / moL 0.05 moL xrightarrow text energy required =360 × 0.05=18 kJ

Q. The energy required to convert all atoms present in $1.2 g$ magnesium to $M g^{2 +}$ ions if $I E_{1}$ , and $I E_{2}$ of magnesium are $120 k J m o l^{- 1}$ and $240 k J m o l^{- 1}$ respectively

18 kJ

36 kJ

360 kJ

24 kJ

Moles of $M g = \frac{1.2}{24} = 0.05 m o L$
$M g ⟶ M g^{2 +} + 2 e^{-}$
$I . E . = I . E_{1} + I . E_{2} = 120 + 240$
$1 m o L energy required = 360 k J / m o L$
$0.05 m o L energy required = 360 \times 0.05 = 18 k J$

Q. The energy required to convert all atoms present in 1.2g magnesium to Mg2+ ions if IE1​, and IE2​ of magnesium are 120kJmol−1 and 240kJmol−1 respectively