When a 375 mL sample of nitrogen is kept at constant temperature, it has a pressure of 1.2 atmospheres. What pressure does it exert when compressed to 125 mL

It exerts a pressure of 3.6 atm

Explanation:

This is a gas law problem. We are looking at volume and pressure with temperature being kept constant, thus, the gas law to use is Boyle's law. It states that at a given constant temperature, the volume of a given mass of gas is inversely proportional to the pressure of the gas.

Mathematically; P1V1 = P2V2

Let's identify the parameters according to the question.

P1 = 1.2 atm

V1 = 375mL

P2 = ?

v2 = 125mL

We arrange the equation to make room for P2 and this can be written as:

P2 = P1V1/V2

P2 = (1.2 * 375) / 125

P2 = 3.6 atm

3.6 atm.

Explanation:

Given:

V1 = 375 ml

P1 = 1.2 atm

V2 = 125 ml

Using Boyle's law,

P1 * V1 = P2 * V2

P2 = (1.2 * 375) / 125

= 3.6 atm.