Ammonia and oxygen combine to produce water vapour and nitric oxide as per the chemical equation: `4NH_(3)(g) + 5O_(2)(g) to 6H_(2)O(g) + 4NO`.
(ii) How many moles of oxygen are required to burn 85 g of ammonia?

Answer

1

Explanation

Let y be the moles of nitric oxide formed when 5 mol of ammonia are completely burnt in oxygen.
`underset("4 mol ") overset("5 mol ")(4NH_(3)(g)) + 5O_(2)(g) to 6H_(2)O(g) + underset("4 mol ") overset(y)(4NO(g)) `
Ratio proportion : `("5 mol "NH_(3))/("4 mol "NH_(3)) = ("y mol NO")/("4 mol NO")`
Or, `y = (" 5 mol "NH_(3))/("4 mol "NH_(3)) xx 4 " mol NO" = 5 ` mol NO