Question

A chemical reaction occurring in a cylinder equipped with a moveable piston produces 0.641 mol of a gaseous product. If the cylinder contained 0.280 mol of gas before the reaction and had an initial volume of 2.05 L , what was its volume after the reaction

Answer 1

Answer: The final volume of the reaction is 4.69 L

Explanation:

The relationship of number of moles and volume at constant temperature and pressure was given by Avogadro's law. This law states that volume is directly proportional to number of moles at constant temperature and pressure.

The equation used to calculate number of moles is given by:

$\frac{V_1}{n_1}=\frac{V_2}{n_2}$

where,

$V_1\text{ and }n_1$ are the initial volume and number of moles

$V_2\text{ and }n_2$ are the final volume and number of moles

We are given:

$V_1=2.05L\\n_1=0.280mol\\V_2=?L\\n_2=0.641mol$

Putting values in above equation, we get:

$\frac{2.05}{0.280}=\frac{V_2}{0.641}\\\\V_2=\frac{2.05\times 0.641}{0.280}=4.69L$

Hence, the final volume of the reaction is 4.69 L