`1 g` of oxygen combines with `0.1260 g` of hydrogen to form `H_(2)O`. `1 g` of nitrogen combines with `0.2160 g` of hydrogen to form `NH_(3)`. Predict the weight of oxygen required to combine with `1 g` of nitrogen to form an oxide.

Answer

A

Explanation

In `H_(2)O : 0.126 g of H_(2)` combines with `1 g` of oxygen.
`:. 1 g of H_(2)` combines with `= (1)/(0.126) = 7.936 g of O_(2)`
In `NH_(3) : 0.216 g of H_(2)` combines with `1 g of N_(2)`
`:. 1 g of H_(2)` combines with `= (1)/(0.126) = 4.629 g of N_(2)`
Ratio of `O : N` in `NH_(3)` which combines with a fixed
weight of `H_(2) (1 g) = 7.936.629 = (7.936)/(4.629) : (4.629)/(4.629) - 1.71 : 1`
`:.` weight of oxygen which comibnes with `1 g` of `N` should be `1.741 g `or its simple multiple.