Given SiO2 + 4HF - -> SiF4 + 2H2O

in this chemical equation how many grams of HF are needed for 182 grams of SiO2 to react completely?

=242.47 g of HF

Explanation:

From the equation One mole of SiO₂ (Silicon (IV) Oxide) react with 4 moles of HF (Hydrogen fluoride).

This is because the reaction ratio is 1:4

The number of moles in182 grams of SiO₂ is:

Number of moles = Mass/RMM

RMM of SiO₂ is 60.08 g/mol

No. of moles=182g/60.08g/mol

=3.0293 moles.

The reaction ratio of SiO₂ to HF is 1:4

Thus the number of moles of HF required to react with 3.0293 moles of SiO₂ is:

(4*3.0293) / 1 = 12.1172 moles

The mass of 12.1172 moles of HF is.

12.1172 moles * RMM of HF

=12.1172 moles*20.01 g/mol

=242.47 g of HF