Answer:
4.86 moles of HCl
Explanation:
1. First write the balanced chemical equations involved in the process:
[tex]CH_{4}+_4Cl_{2}=CCl_{4}+_4HCl[/tex]
[tex]CCl_{4}+_2HF=CCl_{2}+F_{2}+_2HCl[/tex]
2. Calculate what amount of [tex]CCl_{4}[/tex] is formed in the first reaction.
[tex]3.00molesCH_{4}*\frac{1molCCl_{4}}{1molCH_{4}}=3.00molesCCl_{4}[/tex]
As the yield of each reaction is 90.0%, the amount of [tex]CCl_{4}[/tex] produced is the following:
[tex]3.00molesCCl_{4}*0.90=2.7molesCCl_{4}[/tex]
3. Calculate the amount of HCl produced.
[tex]2.7molesCCl_{4}*\frac{2molHCl}{1molCCl_{4}}=5.4molesHCl[/tex]
The total amount of HCl produced with a 90.0% yield is:
[tex]5.4molesHCl*0.90=4.86molesHCl[/tex]
Taking into account the stoichiometry of the reaction and yield of the reaction, the total amount of HCl produced is 15.66 moles.
You know that:
CH₄ + 4 Cl₂ ⟶ CCl₄ + 4 HCl
The CClâ‚„ formed is used as a reactant in the second step as follow:
CCl₄ + 2 HF ⟶ CCl₂ + F₂ + 2 HCl
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), in the first chemical equation you can see that 1 mole of CHâ‚„ forms 1 mole of CClâ‚„ and 4 moles of HCl.
Then, it is possible to determine the amount of moles of CClâ‚‚ produced by the following rule of three: if by stoichiometry 1 mole of CHâ‚„ forms 1 mole of CClâ‚„, if 3 mole of CHâ‚„ react how many moles of CClâ‚„ will be formed?
[tex]amount of moles of CCl_{4} =\frac{3 moles of CH_{4} x1 mole of CCl_{4}}{1 mole of CH_{4} }[/tex]
amount of moles of CClâ‚„= 3 moles
In the same way, it is possible to determine the amount of moles of HCl produced by the following rule of three: if by stoichiometry 1 mole of CHâ‚„ forms 4 moles of HCl, if 3 mole of CHâ‚„ react how many moles of HCl will be formed?
[tex]amount of moles of HCl =\frac{3 moles of CH_{4} x4 moles of HCl}{1 mole of CH_{4} }[/tex]
amount of moles of HCl =12 moles
In general, when a chemical reaction occurs, smaller amounts of product are obtained than could theoretically be expected from the stoichiometry of the reaction. Â Then, the amount of product actually formed is simply called the yield or reaction yield.
In this case, each step in the process has a yield of 90.0%. Â Then, the amount of CClâ‚„ and HCl actually produced in the reaction is obtained by:
By stoichiometry of the reaction, in the second chemical equation you can see that 1 mole of CCâ‚„ forms 2 moles of HCl.
As the CClâ‚„ formed in this first step is used as a reagent in the second step, it is possible to determine the amount of moles of HCl produced by the following rule of three: if by stoichiometry 1 mole of CClâ‚„ forms 2 moles of HCl, if 2.7 mole of CClâ‚„ reacts how many moles of HCl will be formed?
[tex]amount of moles of HCl =\frac{2.7 moles of CCl_{4} x2 mole of HCl}{1 mole of CCl_{4} }[/tex]
amount of moles of HCl =5.4 moles
As each step in the process has a yield of 90.0%, the amount of HCl actually produced in the reaction is calculated as:
amount of moles of HCl =0.90× 5.4 moles
amount of moles of HCl = 4.86 moles
The total amount of HCl produced is the sum of the amount produced in the first and second reactions:
total amount of HCl produced = Â 10.8 moles + 4.86 moles
total amount of HCl produced = 15.66 moles
In summary, the total amount of HCl produced is 15.66 moles.
Learn more:
