Question

Type the correct answer in the box. Given: SiO2 4HF → SiF4 2H2O In this chemical reaction, how many grams of HF are needed for 182 grams of SiO2 to react completely? Express your answer to three significant figures. The reaction requires grams of HF.

Answer 1

The mass of the substance is the product of the molar mass and the moles of the substance in the compound. The amount of the HF required in the reaction is 242 gm.

What is the relation of the mass and moles?

Mass is given as the product of the moles of the substance and of the molar mass of the substance in the compound.

Given,

Molar mass of Silicon dioxide = 60g/mol

mass of Silicon dioxide = 182 g

Molar mass of HF = 20 g/mol

Moles of the Silicon dioxide can be calculated as,

$\begin{aligned}\rm Moles &= \rm \dfrac{mass}{molar\;mass}\\\\&= {182}{60}\\\\&= 3.03\end{aligned}$

The balanced chemical reaction can be shown as,

$\rm SiO_{2} + 4HF \rightarrow SiF_{4} + 2H_{2}O$

From the reaction, it can deduce that,

1 mole of silicon dioxide reacts with 4 moles of HF

So, 3.03 moles of silicon dioxide reacts with 12.12 moles of HF

Mass of HF can be calculated as,

$\begin{aligned}\text{mass of HF} &= \rm moles \times \rm molar \; mass\\\\&= 12.12 \times 20\\\\&= 242 \;\rm g\end{aligned}$

Therefore, the reaction requires 242 gm of HF.

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