1.25 g of a metal (M) reacts with oxygen completely to produce 1.68 g of metal oxide. The empirical formula of the metal oxide is
[molar mass of M and O are 69.7 g `mol^(-1)" and 16.0 g "mol^(-1)`, respectively]

Options

A. `M_(2)O`
B. `M_(2)O_(3)`
C. `MO_(2)`
D. `M_(3)O_(4)`

Answer

B

Explanation

`underset(1.25)underset()(M)" "+ " "O_(2)rarrunderset(1.68)underset()(MO)`
`rArr(1.25)/(E)=(1.68)/(E+8)`
`rArrE=23.25`
`"n-factor"=(69.7)/(23.25)approx3`
`therefore " Emprical formula"=M_(2)O_(3)`