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

Explanation:

To calculate the moles :

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

$\text{Moles of} O_2=\frac{28.8g}{32.00g/mol}=0.900moles$

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 =$\frac{6}{7}\times 0.900=0.771moles$  of $H_2O$

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

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