Question

A gas has a volume of 45.0 mL and a pressure of .98 atm. If the pressure increased to 2.1 atm and the temperature remained the same, what would be the new volume?

Answer 1

Answer: The new volume is 95.45 mL.

Explanation:

Given: $V_{1}$ = 45.0 mL,         $P_{1}$ = 0.98 atm

$P_{2}$ = 2.1 atm,               $V_{2}$ = ?

According to Boyle's law, at constant temperature the pressure of a gas is inversely proportional to its volume.

Therefore, formula used to calculate the new volume is as follows.

$\frac{P_{1}}{V_{1}} = \frac{P_{2}}{V_{2}}$

Substitute the values into above formula as follows.

$\frac{P_{1}}{V_{1}} = \frac{P_{2}}{V_{2}}\\\frac{0.98 atm}{45.0 mL} = \frac{2.1 atm}{V_{2}}\\V_{2} = 95.45 mL$

Thus, we can conclude that the new volume is 95.45 mL.