Respuesta :
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 CCl₄ formed is used as a reactant in the second step as follow:
CCl₄ + 2 HF ⟶ CCl₂ + F₂ + 2 HCl
- First reaction
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 CH₄ forms 1 mole of CCl₄ and 4 moles of HCl.
Then, it is possible to determine the amount of moles of CCl₂ produced by the following rule of three: if by stoichiometry 1 mole of CH₄ forms 1 mole of CCl₄, if 3 mole of CH₄ react how many moles of CCl₄ 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 CCl₄= 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 CH₄ forms 4 moles of HCl, if 3 mole of CH₄ 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. 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%. Then, the amount of CCl₄ and HCl actually produced in the reaction is obtained by:
- amount of moles of CCl₄= 0.90×3 moles → amount of moles of CCl₄= 2.7 moles
- amount of moles of HCl = 0.90×12 moles → amount of moles of HCl = 10.8 moles
- Second reaction
By stoichiometry of the reaction, in the second chemical equation you can see that 1 mole of CC₄ forms 2 moles of HCl.
As the CCl₄ 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 CCl₄ forms 2 moles of HCl, if 2.7 mole of CCl₄ 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 = 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.
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