Question

A sample containing helium gas at 0.20 atm compresses so that its volume is halved at constant temperature. Which is the new pressure in atmospheres?

a. 0.40 atm
b. 0.20 atm
c. 0.80 atm
d. 1.0 atm

Answer 1

According to Boyle's law, when the volume of a gas is halved at constant temperature, the pressure of the gas will double. In this case, the initial pressure of the helium gas is 0.20 atm. When the volume is halved, the new pressure will be twice the initial pressure, which is 0.40 atm.

Step-by-step explanation:

According to Boyle's law, when the volume of a gas is halved at constant temperature, the pressure of the gas will double.

In this case, the initial pressure of the helium gas is 0.20 atm. When the volume is halved, the new pressure will be twice the initial pressure, which is 0.40 atm. Therefore, the correct answer is a. 0.40 atm.

Answer 2

The correct answer is a. 0.40 atm.

Step-by-step explanation:

The pressure of a gas is inversely proportional to its volume when the temperature is constant. This is known as Boyle's Law, which can be expressed as P1V1 = P2V2.

Given that the volume is halved (V2 = 0.5V1), the pressure will double to maintain the equality. Therefore, the new pressure (P2) is 0.20 atm x 2 = 0.40 atm.

So, the correct answer is a. 0.40 atm.