Respuesta :
Answer: 9.6 moles of [tex]O_2[/tex] are needed to burn 3.84 moles of [tex]C_2H_2[/tex]
Explanation:
The balanced chemical reaction for combustion of acetylene is :
[tex]2C_2H_2+5O_2\rightarrow 4CO_2+2H_2O[/tex]
According to stoichiometry:
2 moles of [tex]C_2H_2[/tex] require = 5 moles of [tex]O_2[/tex]
Thus 3.84 moles of [tex]C_2H_2[/tex] require = [tex]\frac{5}{2}\times 3.84=9.6[/tex] moles of [tex]O_2[/tex]
Thus 9.6 moles of [tex]O_2[/tex] are needed to burn 3.84 moles of [tex]C_2H_2[/tex]
The number of moles of oxygen (O₂) required is 9.6 moles. The correct option is c. 9.6 moles
From the question,
The balanced chemical equation of the reaction is
2C₂H₂ + 5O₂ → 4CO₂ + 2H₂O
This means 5 moles of oxygen (O₂) are needed to burn 2 moles of ethyne (C₂H₂)
Now,
We are to determine the number of moles of oxygen (O₂) required to burn 3.84 moles of ethyne (C₂H₂)
Let the number of moles of oxygen (O₂) required be x
Since
5 moles of oxygen (O₂) are needed to burn 2 moles of ethyne (C₂H₂)
Then,
x moles of oxygen (O₂) are needed to burn 3.84 moles of ethyne (C₂H₂)
∴ [tex]x =\frac{5 \times 3.84}{2}[/tex]
[tex]x =\frac{19.2}{2}[/tex]
x = 9.6 moles
Hence, the number of moles of oxygen (O₂) required is 9.6 moles. The correct option is c. 9.6 moles
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