Respuesta :
Answer:
83.64%.
Explanation:
∵ The percent yield = (actual yield/theoretical yield)*100.
actual yield of CO₂ = 2300 g.
- We need to find the theoretical yield of CO₂:
For the reaction:
CH₄ + 2O₂ → 2H₂O + CO₂,
1.0 mol of CH₄ react with 2 mol of O₂ to produce 2 mol of H₂O and 1.0 mol of CO₂.
- Firstly, we need to calculate the no. of moles of 1000 g of CH₄ using the relation:
no. of moles of CH₄ = mass/molar mass = (1000 g)/(16.0 g/mol) = 62.5 mol.
Using cross-multiplication:
1.0 mol of CH₄ produces → 1.0 mol of CO₂, from stichiometry.
∴ 62.5 mol of CH₄ produces → 62.5 mol of CO₂.
- We can calculate the theoretical yield of carbon dioxide gas using the relation:
∴ The theoretical yield of CO₂ gas = n*molar mass = (62.5 mol)(44.0 g/mol) = 2750 g.
∵ The percent yield = (actual yield/theoretical yield)*100.
actual yield = 2300 g, theoretical yield = 2750 g.
∴ the percent yield = (2300 g/2750 g)*100 = 83.64%.
The study of chemicals and bonds is called chemistry. There are two types of metals and these are metals and nonmetals.
The correct answer to the question is 83.64.
What is a combination reaction?
The formation of the new compound by joining the two different elements is called a combination reaction.
According to the question
The percent yield = (actual yield/theoretical yield)*100.
Hence, the actual yield of CO₂ = 2300 g.
The reaction is as follows: - [tex]CH_4 + 2O_2 --- > 2H_2O + CO_2[/tex]
1.0 moles of CH₄ reacts with 2 moles of O₂ to produce 2 moles of H₂O and 1.0 moles of CO₂. Firstly, we need to calculate the no. of moles of 1000 g of CH₄ using the relation:
no. of moles of CH₄ = mass/molar mass =
[tex]\frac{(1000 g)}{(16.0 g/mol)} = 62.5 mol.[/tex]
Using cross-multiplication:
- 1.0 mole of CH₄ produces ---> 1.0 mole of CO₂, from stoichiometry.
- 62.5 moles of CH₄ produces ---> 62.5 moles of CO₂.
We can calculate the theoretical yield of carbon dioxide gas using the relation:
The theoretical yield of CO₂ gas = n*molar mass =[tex](62.5 mol)(44.0 g/mol) = 2750 g.[/tex]
∵ The percent yield = (actual yield/theoretical yield)*100.
- Actual yield = 2300 g,
- Theoretical yield = 2750 g.
The percent yield = [tex](2300 g/2750 g)*100 = 83.64%[/tex]%
Hence, the correct answer is 83.64.
For more information about the reaction, refer to the link:-
https://brainly.com/question/14688752
