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Chapter 9: Problem 133

For the reaction \(\mathrm{SiCl}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{SiO}_{2}+\mathrm{HCl}\), (a) Balance the equation. (b) If you want to make \(120.0 \mathrm{~g}\) of \(\mathrm{HCl}\), how many grams of \(\mathrm{SiCl}_{4}\) and \(\mathrm{H}_{2} \mathrm{O}\) do you need? (c) How many grams of \(\mathrm{SiO}_{2}\) are produced from the quantities calculated in (b)?

Short Answer

Expert verified
(a) The balanced equation is \(SiCl_4 + 2H_2O \rightarrow SiO_2 + 4HCl\). (b) To produce 120.0 g of HCl, you would need 139.5 g of SiCl4 and 29.58 g of H2O. (c) 49.36 g of SiO2 are produced from the calculated amounts of SiCl4 and H2O.

Step by step solution

01

(Step 1: Balance the chemical equation)

First, let's balance the given chemical equation: \(SiCl_4 + H_2O \rightarrow SiO_2 + HCl\) \(SiCl_4 + 2H_2O \rightarrow SiO_2 + 4HCl\) Now the chemical equation is balanced.
02

(Step 2: Calculate moles of HCl)

To find the moles of HCl needed to produce 120.0 g of HCl, use the molar mass of HCl (M(HCl) = 1 + 35.5 = 36.5 g/mol): Moles of HCl = (mass of HCl) / M(HCl) = (120.0 g) / (36.5 g/mol) = 3.287 moles
03

(Step 3: Determine moles of SiCl4 and H2O required)

Using the balanced chemical equation and the stoichiometry of the reaction, calculate the moles of SiCl4 and H2O needed to produce 3.287 moles of HCl: Moles of SiCl4 = (3.287 moles HCl) * (1 mol SiCl4 / 4 mol HCl) = 0.8218 moles SiCl4 Moles of H2O = (3.287 moles HCl) * (2 mol H2O / 4 mol HCl) = 1.6435 moles H2O
04

(Step 4: Calculate grams of SiCl4 and H2O required)

Now, find the mass of SiCl4 and H2O needed by multiplying their moles by their respective molar masses (M(SiCl4) = 169.9 g/mol and M(H2O) = 18.0 g/mol): Mass of SiCl4 = (0.8218 moles SiCl4) * (169.9 g/mol) = 139.5 g Mass of H2O = (1.6435 moles H2O) * (18.0 g/mol) = 29.58 g So, 139.5 g of SiCl4 and 29.58 g of H2O are needed to produce 120.0 g of HCl.
05

(Step 5: Calculate grams of SiO2 produced)

Using the balanced chemical equation, calculate the mass of SiO2 produced from 0.8218 moles of SiCl4. We already know M(SiO2) = 60.1 g/mol: Mass of SiO2 = (0.8218 moles SiCl4) * (1 mol SiO2 / 1 mol SiCl4) * (60.1 g/mol) = 49.36 g Thus, 49.36 g of SiO2 are produced from the calculated amounts of SiCl4 and H2O.

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Most popular questions from this chapter

Consider the following unbalanced chemical equation: \(\mathrm{P}+\mathrm{O}_{2} \rightarrow \mathrm{P}_{2} \mathrm{O}_{5}\) (a) How many grams of phosphorus (P) are required to react completely with \(20.0 \mathrm{~g}\) of \(\mathrm{O}_{2} ?\) (b) What is the theoretical yield in grams if you combine the amounts of reactants in part (a)?

The compound \(\mathrm{P}_{4} \mathrm{O}_{10}\) has an empirical formula of \(\mathrm{P}_{2} \mathrm{O}_{5} .\) By what factor will the percent by mass composition differ for each element between these two formulas? Explain your answer.

Consider a \(5.00-\mathrm{g}\) sample of silver nitrate, \(\mathrm{AgNO}_{3}(s)\) (a) How many moles of \(\mathrm{AgNO}_{3}\) are in this sample? (b) How many moles of \(\mathrm{O}\) are in this sample? (c) How many grams of \(\mathrm{N}\) are in this sample? (d) How many Ag atoms are in this sample?

An organic compound of carbon and hydrogen has the empirical formula CH. What is its molecular formula if its molar mass is: (a) \(26 \mathrm{~g} / \mathrm{mol}\) (b) \(52 \mathrm{~g} / \mathrm{mol}\) (c) \(78 \mathrm{~g} / \mathrm{mol}\)

Chlorine \(\left(\mathrm{Cl}_{2}\right)\) and fluorine \(\left(\mathrm{F}_{2}\right)\) react to form \(\mathrm{ClF}_{3}\). A reaction vessel contains \(10.00 \mathrm{~g} \mathrm{Cl}_{2}\) and \(10.00 \mathrm{~g} \mathrm{~F}_{2}\). (Hint: Refer to Problem 9.82.) (a) Write a balanced chemical equation for this reaction. (b) Which reactant is limiting? (c) What is the theoretical yield for this reaction in grams? (d) How many grams of excess reactant are left over at the end of the reaction? (e) When this reaction is actually performed, \(12.50 \mathrm{~g}\) of \(\mathrm{ClF}_{3}\) is recovered. What is the percent yield of the reaction?
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