Element X reacts with oxygen to produce a pure sample of `X_(2)O_(3)`. In an experiment it is found that `1.00g` of X produces `1.16g" of "X_(2)O_(3)`. Calculate the atomic weight of X. (Atomic weight of oxygen, `16.0 gmol^(-1)`).

Options

A. `67`
B. `100.2`
C. `125`
D. `150`

Answer

C

Explanation

The mass of O atoms `=1.6-1.00=0.16 g`
Number of moles of O atom `=(0.16)/(16)=0.01`
In `X_(2)O_(3), ("No. of moles of X")/("No. of moles of O")=(2)/(3)`
Number of moles of, `X=(2)/(3)xx0.01=(0.02)/(3)=0.00666`
Atomic weight of, `X=("massing")/("no. of moles")=(1.0)/(0.00666)=150`