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Chapter 3: Problem 66

Silicon tetrachloride \(\left(\mathrm{SiCl}_{4}\right)\) can be prepared by heating Si in chlorine gas: $$ \mathrm{Si}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SiCl}_{4}(l) $$ In one reaction, 0.507 mole of \(\mathrm{SiCl}_{4}\) is produced. How many moles of molecular chlorine were used in the reaction?

Short Answer

Expert verified
We used 1.014 moles of molecular chlorine in the reaction to produce 0.507 mole of silicon tetrachloride.

Step by step solution

01

Identify the Given and Required Quantities

We are given that 0.507 mole of Silicon tetrachloride (SiCl4) is produced in the reaction. We are asked to find out how many moles of molecular chlorine were used in the reaction.
02

Interpret the Balanced Chemical Equation

From the balanced chemical equation, Si(s) + 2Cl2(g) -> SiCl4(l), it can be seen that 2 moles of chlorine react with silicon to produce 1 mole of silicon tetrachloride.
03

Utilize Stoichiometric Ratios

Use stoichiometric analysis to calculate the number of moles of chlorine gas used in the reaction. From the equation, the stoichiometric ratio between SiCl4 and Cl2 is 1:2. Therefore, to find the moles of molecular chlorine (Cl2) used, multiply the given moles of SiCl4 by 2.
04

Calculate the Moles of Chlorine Gas

Using the stoichiometric ratio from Step 3, multiply the given moles of SiCl4 (0.507 mol) by 2. This will give us the moles of chlorine gas (Cl2) used in the reaction: Moles of Cl2 = Moles of SiCl4 * 2 = 0.507 mol * 2 = 1.014 mol.

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Most popular questions from this chapter

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