Respuesta :
Answer: The mass of carbon dioxide that can be produced is 10.3 grams
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
- For hexane:
Given mass of hexane = 3.4 g
Molar mass of hexane = 86.2 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of hexane}=\frac{3.4g}{86.2g/mol}=0.039mol[/tex]
- For oxygen gas:
Given mass of oxygen gas = 22.6 g
Molar mass of oxygen gas = 32 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of oxygen gas}=\frac{22.6g}{32g/mol}=0.706mol[/tex]
The chemical equation for the reaction of hexane and oxygen gas follows:
[tex]2C_6H_{14}+19O_2\rightarrow 12CO_2+14H_2O[/tex]
By Stoichiometry of the reaction:
2 moles of hexane reacts with 19 moles of oxygen gas
So, 0.039 moles of hexane will react with = [tex]\frac{19}{2}\times 0.039=0.370mol[/tex] of oxygen gas
As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.
Thus, hexane is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
2 moles of hexane produces 12 moles of carbon dioxide
So, 0.039 moles of hexane will produce = [tex]\frac{12}{2}\times 0.039=0.234moles[/tex] of carbon dioxide
Now, calculating the mass of carbon dioxide from equation 1, we get:
Molar mass of carbon dioxide = 44 g/mol
Moles of carbon dioxide = 0.234 moles
Putting values in equation 1, we get:
[tex]0.234mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(0.234mol\times 44g/mol)=10.3g[/tex]
Hence, the mass of carbon dioxide that can be produced is 10.3 grams
Answer:
Explanation:
I think the accurate answer to this question, based from the sources, is A) The substances will mix uniformly. Carbon dioxide and hexane at 0C exposed at extreme pressure will be able to mix together.
