Answer: d) 16.34 grams
Explanation:
To calculate the moles :
[tex]\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex]
[tex]\text{Moles of} N_2O_5=\frac{31.5g}{108.01g/mol}=0.292moles[/tex]
[tex]4N_2+5O_2\rightarrow 2N_2O_5[/tex]
According to stoichiometry :
As 2 moles of [tex]N_2O_5[/tex] are produced by= 4 moles of [tex]N_2[/tex]
Thus 0.292 moles of [tex]N_2O_5[/tex] are produced by= =[tex]\frac{4}{2}\times 0.292=0.584moles[/tex] of [tex]N_2[/tex]
Mass of [tex]N_2=moles\times {\text {Molar mass}}=0.584moles\times 28g/mol=16.34g[/tex]
Thus 16.34 g of [tex]N_2[/tex] will be needed
