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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.

User Niyasc
by
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2 Answers

1 vote
SiO2 + 4HF → SiF4 + 2H2O
60 g. --> 80 g
182 g. --> x g

x = (182 * 80)/(60) \\ x = 242.7 \: g

The reaction requires 242.7 grams of HF.
User Huppo
by
8.0k points
5 votes

Answer : The reaction requires 242 grams of HF.

Explanation : Given,

Mass of
SiO_2 = 182 g

Molar mass of
SiO_2 = 60 g/mole

Molar mass of HF = 20 g/mole

First we have to calculate the moles of
SiO_2


\text{Moles of }SiO_2=\frac{\text{Mass of }SiO_2}{\text{Molar mass of }SiO_2}=(182g)/(60g/mole)=3.03moles

Now we have to calculate the moles of HF.

The given balanced chemical reaction is,


SiO_2+4HF\rightarrow SiF_4+2H_2O

From the balanced chemical reaction, we conclude that

As, 1 mole of
SiO_2 react with 4 moles of HF

So, 3.03 moles of
SiO_2 react with
4* 3.03=12.12 moles of HF

Now we have to calculate the mass of HF.


\text{Mass of HF}=\text{Moles of HF}* \text{Molar mass of HF}=12.12mole* 20g/mole=242g

Therefore, the reaction requires 242 grams of HF.

User Pbering
by
8.0k points
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