A) \[N{{H}_{2}}\]
B) \[{{N}_{3}}H\]
C) \[N{{H}_{3}}\]
D) \[{{N}_{2}}{{H}_{4}}\]
Correct Answer: D
Solution :
[d] In an unknown compounds containing N and H given % of H =12.5% | ||||||||||||
% of \[N=100-12.5=87.5%\] | ||||||||||||
Element Percentage Atomic ratio Simple ratio | ||||||||||||
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2 \[\times \] vapour density = Mol. wt = mol wt. \[=16\times 2=32.\] | ||||||||||||
Molecular formula = n \[\times \] empirical formula mass \[n=\frac{32}{16}=2\] | ||||||||||||
\[\therefore \] Molecular formula of the compound will be \[={{\left( N{{H}_{2}} \right)}_{2}}={{N}_{2}}{{H}_{4}}\] | ||||||||||||
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