Question

A sample of Ne(g) has a volume 250 mL at 752 mm Hg. What is the

new volume if the temperature and amount of gas held constant, the
pressure is;
a) lowered to 385 mm Hg.
b) Increased to 3.68 atm.

Answer 1

Answer: a) 525 ml

b) 67.2 ml

Step-by-step explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

`P\propto (1)/(V)` (At constant temperature and number of moles)

`P_1V_1=P_2V_2`

where,

a)
`P_1` = initial pressure of gas = 752 mm Hg

`P_2` = final pressure of gas = 385 mm Hg

`V_1` = initial volume of gas = 250 ml

`V_2` = final volume of gas = ?

`752* 250=385* V_2`

`V_2=525ml`

Therefore, the volume at 385 mm Hg is 525 ml.

b)
`P_1` = initial pressure of gas = 752 mm Hg

`P_2` = final pressure of gas = 3.68 atm = 2796.8 mm Hg (760mmHg=1atm)

`V_1` = initial volume of gas = 250 ml

`V_2` = final volume of gas = ?

`752* 250=2796.8* V_2`

`V_2=67.2ml`

Therefore, the volume at 3.68 atm is 67.2 ml.