A) \[{{M}_{2}}{{O}_{3}}\]
B) \[MO\]
C) \[M{{O}_{2}}\]
D) \[{{M}_{2}}{{O}_{5}}\]
Correct Answer: B
Solution :
For I oxide Oxygen = 36.4% Metal\[=100-36.4=63.6%\] Given, formula of oxide\[={{M}_{2}}O\] \[\therefore \]63.6% of metal = 2 atoms of metal and 36.4% of oxygen = 1 atom of oxygen For II oxide Oxygen = 53.4% Metal\[=100-53.4=46.6%\] \[\because \]63.6% of metal = 2 atoms of metal \[\therefore \]46.6% of metal\[=\frac{2\times 46.6}{63.6}\] = 1.46 atoms of metal Again,\[\because \]36.4% of oxygen = 1 atom of oxygen \[\therefore \]53.4% of oxygen\[=\frac{1\times 53.4}{36.4}\] = 1.46 atoms of oxygen Ratio of metal and oxide \[=1.46\,\,:1.46\] \[=1:1\] Hence, formula of metal oxide = MO
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