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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