What is the total volume of gaseous products formed when 98.1 liters of butane ($C_4H_{10}$) react completely according to the following reaction? (All gases are at the same temperature and pressure.)

\[ C_4H_{10} (g) + O_2 (g) \rightarrow CO_2 (g) + H_2O (g) \]

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Answer :

jaunty jaunty · Answer 1 · 2023-10-20T01:33:04-04:00

Answer:

Total volume of gaseous products = 882.9 L

Explanation:

The balanced equation for combustion of butane is:

[tex]C_4H_{10}+\frac{13}{2} O_{2}\ --->\ 4CO_{2}+5H_2O[/tex]

At constant temperature and pressure volume of gas is directly proportional to number of moles of the gas.

Then from the balanced equation we can say that:

1 L of butane reacts with 6.5 L of oxygen to give 4 L of carbon dioxide and 5 L of water.

98.1 L of butane gives 4*98.1 L of carbon dioxide and 5*98.1 L of water.

Hence total volume of gaseous products formed = 98.1*(4+5) L

= 98.1*9 L = 882.9 L