In order to make modern electronics components, silicon of an extremely high pur

Question

In order to make modern electronics components, silicon of an extremely high purity is required. One of the steps in purifying silicon involves reacting the intermediate silicon tetrachloride with steam to produce high-purity silicon dioxide and hydrogen chloride gas, as shown in the unbalanced equation below.
SiCl4(s) + H2O(g) ? SiO2(s) + HCl(g)
If the reaction is run with 534.7 g SiCl4 and 103.1 g H2O, what mass of SiO2 will be produced, and what is the excess reactant and what mass of it remains?
(a) What mass of SiO2 will be produced?

I solved and checked and I get 171.7 g SiO2, not sure what I'm doing wrong please help! and please explain steps

Explanation / Answer

SiCl4(g) + 2H2O(g) ? SiO2(s) + 4HCl(g)

1mole sio2=60gm

1mole SiCl4=169.9gm

534.7g SiCl4=3.147mole

103.1 g H2O=5.72mole

2.86mole of SiCl4 react with 5.72mole H2Oand produce 2.86mole SiO2=171.6gm SiO2

excess reactant

0.287 mloe SiCl4=48.76gm SiCl4

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