Answer : The reaction requires 242 grams of HF.
Explanation : Given,
Mass of [tex]SiO_2[/tex] = 182 g
Molar mass of [tex]SiO_2[/tex] = 60 g/mole
Molar mass of HF = 20 g/mole
First we have to calculate the moles of [tex]SiO_2[/tex]
[tex]\text{Moles of }SiO_2=\frac{\text{Mass of }SiO_2}{\text{Molar mass of }SiO_2}=\frac{182g}{60g/mole}=3.03moles[/tex]
Now we have to calculate the moles of HF.
The given balanced chemical reaction is,
[tex]SiO_2+4HF\rightarrow SiF_4+2H_2O[/tex]
From the balanced chemical reaction, we conclude that
As, 1 mole of [tex]SiO_2[/tex] react with 4 moles of HF
So, 3.03 moles of [tex]SiO_2[/tex] react with [tex]4\times 3.03=12.12[/tex] moles of HF
Now we have to calculate the mass of HF.
[tex]\text{Mass of HF}=\text{Moles of HF}\times \text{Molar mass of HF}=12.12mole\times 20g/mole=242g[/tex]
Therefore, the reaction requires 242 grams of HF.
