Answer: 13.9 g of [tex]H_2O[/tex] will be produced from the given mass of oxygen
Explanation:
To calculate the moles :
[tex]\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex]
[tex]\text{Moles of} O_2=\frac{28.8g}{32.00g/mol}=0.900moles[/tex]
The balanced chemical reaction is:
[tex]4NIO_2(g)+7O_2(g)\rightarrow 4NO_2(g)+6H_2O(g)[/tex]
According to stoichiometry :
7 moles of [tex]O_2[/tex] produce = 6 moles of [tex]H_2O[/tex]
Thus 0.900 moles of [tex]O_2[/tex] will produce =[tex]\frac{6}{7}\times 0.900=0.771moles[/tex] of [tex]H_2O[/tex]
Mass of [tex]H_2O=moles\times {\text {Molar mass}}=0.771moles\times 18.02g/mol=13.9g[/tex]
Thus 13.9 g of [tex]H_2O[/tex] will be produced from the given mass of oxygen
