If a gas at 2 atm is expanded to 4 liters at constant temperature, what will be its new pressure?

To determine the new pressure of the gas when it is expanded to a larger volume while keeping the temperature constant, we can use Boyle's Law. Boyle's Law states that the pressure of a gas is inversely proportional to its volume when temperature is held constant. This can be represented mathematically as P1V1 = P2V2, where P is pressure and V is volume.

In this scenario, the initial pressure (P1) is 2 atm and the initial volume (V1) is not specified, but we can express the relationship of the initial and final conditions. The final volume (V2) is given as 4 liters.

Because we know that the pressure and volume have an inverse relationship, when the volume increases (from V1 to V2), the pressure must decrease. If we want to find the new pressure (P2), we can rearrange Boyle's Law:

P2 = (P1 * V1) / V2.

Using the concept of proportionality, if the volume doubles, the pressure will halve, given the constant temperature.

Assuming an initial volume (let's take it as 2 liters for easier calculation), if the volume goes from 2 liters (hypothetical V