Status: Not yet answered | Points possible: 1.00 A sample of chlorine gas starting at 681 mm Hg is placed under a pressure of 992 mm Hg and reduced to a volume of 543.8 mL.
What was the initial volume, in ml, of the chlorine gas container if the process was performed at constant temperature?
Type

V1 = 792.1 ml

Explanation:

The product of pressure and volume is constant when temperature is constant. This relationship is known as Boyle's law.

To answer this, I assume the chlorine gas will behave as a perfect gas. In reality this is not completely true.

P1*V1 = P2*V2

Given:

P1 = 681 mm Hg

V1 = ?

P2 = 992 mm Hg

V2 = 543.8 ml

V1 = ( P2 * V2 ) / P1

V1 = (992 *543.8 ) / 681

V1 = 792.143318649046 ml

V1 = 792.1 ml

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3