Question

A gas that exerts a pressure of 125.0 mm Hg in a container with a volume of _____ mL will exert a pressure of 145 mm Hg when transferred to a container with a volume of 0.4650 L.

Answer 1

Answer:

Initial volume of container = 0.5394 L (≅0.539 L)

Explanation:

Given:

Initial pressure of gas, P1 = 125.0 mmHg

Final pressure of gas, P2 = 145 mmHg

Final volume, V2 = 0.4650 L

To determine:

The initial volume V1 occupied by the gas

Explanation:

Based on the ideal gas equation

$PV = nRT$

where P = pressure, V = volume ; n = moles of gas

R = gas constant, T = temperature

At constant n and T, the above equation becomes:

PV = constant

This is the Boyle's law

Therefore:

$P1V1 = P2V2\\\\V1 = \frac{P2V2}{P1} = \frac{145 mmHg*0.4650L}{125mmHg} = 0.5394L$

Answer 2

I believe you use Boyles Law so P₁V₁=P₂V₂

so 125.0mmHg(x) = (145mmHg)(.4650L) 

keep in mind this will give you an answer in L and you want mL