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Why is N(2)O(5) more acidic than N(2)O(3...

Why is `N_(2)O_(5)` more acidic than `N_(2)O_(3)` ?

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Since the oxidation state of N is +5 in `N_(2)O_(5)and+3" in "N_(2)O_(3)`, therefore, `N_(2)O_(5)` can accept electrons more readily than `N_(2)O_(3)` and hence `N_(2)O_(5)` is a stronger acid than `N_(2)O_(3)`.
Alternatively, `N_(2)O_(5)andN_(2)O_(3)` dissolve in `H_(2)O` forming `HNO_(3)andHNO_(2)` respectively.

Due to higher oxidation state of +5 of N in `HNO_(3)` than +3 in `HNO_(2),NO_(2)` pulls the electrons of the O-H in `HNO_(3)` more strongly than NO pulls the electrons of the O-H bond in `HNO_(2)`. In other words, `HNO_(3)` releases a proton more releases a proton more reaidily than `HNO_(2)` and hence `HNO_(3)orN_(2)O_(5)` is a stronger acid than `HNO_(2)or N_(2)O_(3)`.
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Give reasons for the following: (a) Red phosphorus is less reactive than white phosphorus. (b) Electron gain enthalpies of halogens are largely negative. (c) N_(2)O_(5) is more acidic than N_(2)O_(3) .

Assertion (A) : P_(2)O_(3) is more basic than N_(2)O_(3) Reason (R) : Metallic nature of the central atom increases down the group

Why is O_(3) more reactive than O_(2) ?

Bond order for N_(2)^(o+) and N_(2)^(Theta) are same (i.e2.5) Reasoning N_(2)^(o+) is more stable than N_(2)^(Theta) .

When N_(2)O_(5) is heated at certain temperature, it dissociates as N_(2)O_(5)(g)hArrN_(2)O_(3)(g)+O_(2)(g),K_(c)=2.5 At the same time N_(2)O_(3) also decomposes as : N_(2)O_(3)(g)hArrN_(2)O(g)+O_(2)(g). "If initially" 4.0 moles of N_(2)O_(5) "are taken in" 1.0 litre flask and alowed to dissociate. Concentration of O_(2) at equilibrium is 2.5 M. "Equilibrium concentratio of " N_(2)O_(5) is :

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