# If 15/4 L of a gas at room temperature exerts a pressure of 42 kPa on its container, what pressure will the gas exert if the container's volume changes to 12/7 L?

Feb 25, 2018

The new pressure is $= 91.875 k P a$

#### Explanation:

Apply Boyle's Law

${P}_{1} {V}_{1} = {P}_{2} {V}_{2}$, at constant temperature

The initial pressure is ${P}_{1} = 42 k P a$

The initial volume is ${V}_{1} = \frac{15}{4} L$

The final volume is ${V}_{2} = \frac{12}{7} L$

The final pressure is

${P}_{2} = {V}_{1} / {V}_{2} \cdot {P}_{1} = \frac{\frac{15}{4}}{\frac{12}{7}} \cdot 42 = 91.875 k P a$