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Anhydrous barium nitrate when heated decomposes and oxygen and NO₂ gas is evolved. Similarly magnesium nitrate when heated decomposes to give out NO₂ gas and oxygen.
In both cases corresponding oxides are also formed. Select the correct answer(s) :

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NO₂ will be evolved at a lower temperature in case of Ba (NO₃)₂ as compared to that of Mg(NO₃)₂

The lattice energy value is higher for magnesium nitrate than that of barium nitrate

NO₂ will be evolved at a lower temperature in case of Mg(NO₃)₂ as compared to that Ba(NO₃)₂

In both cases [i.e., heating of Mg(NO₃)₂ and Ba(NO₃)₂] the ratio of volume of NO₂ and O₂ evolved is 4: 1

answer is A, B, D.

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Detailed Solution

The nitrates of Mg and Ba decompose as follows $2 M {({NO}_{3})}_{2} \overset{heat}{⟶} 2 MO + 4 {NO}_{2} (g) + O_{2} (g)$ [M= Mg or Ba]

The option (c) is incorrect because of the fact that Mg(NO₃)₂ is more covalent than Ba(NO₃)₂. Due to this Mg(NO₃)₂ decomposes more readily.

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