MCQ
$NH_3$ can not be obtained by
- ✓heating of $NH_4NO_3$
- Bheating of $NH_4Cl$
- Cheating of $(NH_4)_2CO_3$
- DNone
$NH _4 NO _3 \rightarrow N _2 O + H _2 O$
$NH _4 NO _2 \rightarrow N _2+ H _2 O$
$NH _4 Cl _{\rightarrow} NH _3+ HCl$
$NH _4 NO _3(a q)+ NaOH (s) \rightarrow NH _3(g)+ H _2 O (l)+ NaNO _3(a q)$
$CaCN _2+3 H _2 O \rightarrow CaCO _3+ NH _3$
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$(I)$ both the complexes can be high spin
$(II)$ $Ni(II)$ complex can very rarely be low spin.
$(III)$ with strong field ligands, $Mn(II)$ complexes can be low spin.
$(IV)$ aqueous solution of $Mn ( II )$ ions is yellow in color.
$(A)$ Dinitrogen is a diatomic gas which acts like an inert gas at room temperature.
$(B)$ The common oxidation states of these elements are $-3,+3$ and +5 .
$(C)$ Nitrogen has unique ability to form $\mathrm{p} \pi-\mathrm{p} \pi$ multiple bonds.
$(D)$ The stability of +$5$ oxidation states increases down the group.
$(E)$ Nitrogen shows a maximum covalency of $6$.
Choose the correct answer from the options given below.
${A_2}\left( g \right) + {B_2}\left( g \right) \rightleftharpoons {C_2}\left( g \right) + {D_2}\left( g \right)$
If we take $1\ mole$ of each of the four gases in a $10\ litre$ container, what would be equilibrium concentration of $A_2(g)$?