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. SiCl_4(s) + H_2O(g) right arrow SiO_2(s) + HCl(g) If the reaction is run with 536.0 g SiCl_4 and 103.5 g H_2O, what mass of SiO_2 will be produced, and what is the excess reactant and what mass of it remains What mass of SiO_2 will be produced g SiO_2 What is the excess reactant (Omit states-of-matter from your answer.) What mass of the excess reactant remains g

Explanation / Answer

m = 536 SiCl4

mol = masS/MW = 536 /169.9 = 3.154796 mol of SiCl4

m = 103.5 g H2O

mol = 103.5/18 = 5.75 mol of H2O

Reaction

SiCl4 + H2O = SiO2 + HCl

balanced

SiCl4 + 2H2O = SiO2 + 4HCl

then

ratio is 1:2

3.154796 Sicl4 will need 2*3.154796 = 6.309592 mol of H2O are needed

then H2O is limiting

then

5.75 mol of H2O produces 1/2*5.75 = 2.875 mol of SiO2

mass = mol*MW = 2.875*60.08 = 172.73 g of SiO2 are produced

b)

excess reactant is SiCl4

c)

mass reactatnt remaining:

3.154796 - 5.75 /2 = mol remaining

0.279796 mol of SiO2 remaining

mass = mol*MW = 60.08*0.279796 = 16.810 g are remaining

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