Question

Avogadro's law states that one mole of an ideal gas takes up around 22 liters at standard temperature and
pressure. Assuming all reagents can be treated as ideal gases, how many grams of carbon dioxide are
produced in the complete reaction of 44 liters of butane (C4H10) with oxygen to produce carbon dioxide
(at STP)?​

Answer 1

Explanation:

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Answer 2

Answer:

44 litres of butane will produce 352 grams of carbon dioxide.

Explanation:

Since butane is reacting with oxygen to produce carbon dioxide and water. A balanced chemical equation of reaction is

$\[{C_4}{H_{10}} + \frac{{13}}{2}{O_2} \to 4C{O_2} + 5{H_2}O\]$

22 litres of gas contain 1 mole of that gas.

Therefore, 44 litres of butane gas contain 2 moles of butane.

According to the reaction:

1 mole of butane produces 4 moles of carbon dioxide.

So, 2 moles of butane will produce 8 moles of carbon dioxide.

Now,

1 mole of carbon dioxide = 44 grams

8 mole of carbon dioxide = $8\times44$ grams

8 mole of carbon dioxide = 352 grams

Therefore, 44 litres of butane after reacting with oxygen will produce 352 grams of carbon dioxide.