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?

Question

asked Jun 14, 2022 174k views

1 Answer

Forgo · Answer 1 · 2022-06-21T01:27:17+0000

Answer: The new volume is 95.45 mL.

Step-by-step 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.

(P_(1))/(V_(1)) = (P_(2))/(V_(2))

Substitute the values into above formula as follows.

$(P_(1))/(V_(1)) = (P_(2))/(V_(2))\\(0.98 atm)/(45.0 mL) = (2.1 atm)/(V_(2))\\V_(2) = 95.45 mL$

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