A sample of chlorine gas starting at 686 mm Hg is placed under a pressure of 991 mm Hg and reduced to a volume of 507.6 mL. What was the initial volume of the chlorine gas container if the process was performed at constant temperature

The initial volume of the chlorine gas

Explanation:

Given:

P1= 686mmHg

P2= 991mmHg

V2= 5076mL

V1=?

According to Boyle's law which states that at a constant temperature, the pressure on a gas increases as it's volume decreases.

It can be expressed as : P1V1 = P2V2

Where P1 is the initial pressure

P2= final pressure

V1= initial volume

V2 = final volume

V1= (991mmHg*507.6mL)/686mmHg

V1=503031.6/686

Therefore, The initial volume of the chlorine gas

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)

a is the correct answer