Question

A helium sample occupies 1.50 L of space at 124.6 kPa. What pressure would the helium need to experience to have a volume of 0.75 L?

A. 130 kPa
B. 97 kPa
C. 250 kPa
D. 62 kPa

Answer 1

Answer : The correct option is, (C) 250 kPa

Explanation :

Boyle's Law : It is defined as the pressure of the gas is inversely proportional to the volume of the gas at constant temperature and number of moles.

`P\propto (1)/(V)`

or,

`P_1V_1=P_2V_2`

where,

`P_1` = initial pressure = 124.6 kPa

`P_2` = final pressure = ?

`V_1` = initial volume = 1.50 L

`V_2` = final volume = 0.75 L

Now put all the given values in the above equation, we get:

`124.6kPa* 1.50L=P_2* 0.75L`

`P_2=249.2kPa\approx 250kPa`

Thus, the pressure of helium need to experience to have a volume of 0.75 L would be, 250 kPa