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)(M)+ O_(2) to underset(1.68)(MO)`
`rArr (1.25)/(E) = (1.68)/(E+8)`
`rArr E = 23.25`
n - factor ` = (69.7)/(23.25)~~ 3`
`therefore` Empirical formula `= M_(2)O_(3)`