Question

How many grams of H 2O are produced from 28.8 g of O 2? (Molar Mass of H 2O = 18.02 g) (Molar Mass of O 2=32.00 g) 4 NH 3 (g) + 7 O 2 (g) → 4 NO 2 (g) + 6 H 2O (g)

Answer 1

Answer: 13.9 g of
`H_2O` will be produced from the given mass of oxygen

Step-by-step explanation:

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}`

`\text{Moles of} O_2=(28.8g)/(32.00g/mol)=0.900moles`

The balanced chemical reaction is:

`4NIO_2(g)+7O_2(g)\rightarrow 4NO_2(g)+6H_2O(g)`

According to stoichiometry :

7 moles of
`O_2` produce = 6 moles of
`H_2O`

Thus 0.900 moles of
`O_2` will produce =
`(6)/(7)* 0.900=0.771moles` of
`H_2O`

Mass of
`H_2O=moles* {\text {Molar mass}}=0.771moles* 18.02g/mol=13.9g`

Thus 13.9 g of
`H_2O` will be produced from the given mass of oxygen