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<u>Answer:</u> The moles of carbon dioxide formed in the reaction is 20 moles.
<u>Explanation:</u>
We are given:
Number of moles of butane = 5.0 moles
The chemical reaction for the combustion of butane follows the equation:
As, oxygen is present in excess. So, it is considered as an excess reagent.
Thus, butane is considered as a limiting reagent because it limits the formation of products.
By stoichiometry of the reaction:
2 moles of butane produces 8 moles of carbon dioxide.
So, 5 moles of butane will produce = of carbon dioxide.
Hence, the moles of carbon dioxide formed in the reaction is 20 moles.
Answer:
The final pressure is 0.725 atm.
Explanation:
Gay Lussac's Law establishes the relationship between pressure and temperature of a gas when the volume is constant. This law says that when there is a constant volume, as the temperature increases, the pressure of the gas increases. And when the temperature is decreased, the pressure of the gas decreases. That is, pressure and temperature are directly proportional quantities.
Mathematically, Gay-Lussac's law states that, when a gas undergoes a constant volume transformation, the quotient of the pressure exerted by the gas temperature remains constant:
When analyzing an initial state 1 and a final state 2, the following is satisfied:
In this case:
- P1= 0.81 atm
- T1= 33 C= 306 K
- P2= ?
- T2= 1 C= 274 K
Replacing:
Solving:
P2= 0.725 atm
<u><em>The final pressure is 0.725 atm.</em></u>