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A chemical reaction occurring in a cylinder equipped with a moveable piston produces 0.621 mol of a gaseous product.

If the cylinder contained 0.120 mol of gas before the reaction and had an initial volume of 2.18 L, what was its volume after the reaction?

(Assume constant pressure and temperature and that the initial amount of gas completely reacts.)

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dsdrajlin

Answer:

11.3 L

Explanation:

Initially, the cylinder had n₁ = 0.120 mol of gas in an initial volume V₁ = 2.18 L. At the end, it had n₂ = 0.621 mol in an unknown volume V₂. According to the Avogadro's law, in the same conditions of pressure and temperature, the volume is directly proportional to the number of moles.

[tex]\frac{V_{1}}{n_{1}} =\frac{V_{2}}{n_{2}} \\V_{2}=\frac{V_{1}\times n_{2} }{n_{1}} =\frac{2.18L \times 0.621mol}{0.120mol} =11.3L[/tex]

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