Question

A sample of helium gas has a volume of 150. Ml (V₁) at 0.95 atom (P₁). What will your new pressure (P₁) be if the volume is changed to 40.0 ml (V₁) and temperature remains constant?

Answer 1

Answer: The new pressure when temperature remains constant is 3.56 atm

Explanation:

To calculate the new pressure, we use the equation given by Boyle's law. This law states that pressure is inversely proportional to the volume of the gas at constant temperature.

The equation given by this law is:

$P_1V_1=P_2V_2$

where,

$P_1\text{ and }V_1$ are initial pressure and volume.

$P_2\text{ and }V_2$ are final pressure and volume.

We are given:

$P_1=0.95atm\\V_1=150mL\\P_2=?atm\\V_2=40.0mL$

Putting values in above equation, we get:

$0.95atm\times 150mL=P_2\times 40\\\\P_2=\frac{0.95\times 150}{40}=3.56atm$

Hence, the new pressure when temperature remains constant is 3.56 atm