please help me understand this question

If measurements of a gas are 50L and 300 kilopascals and then the gas is measured a second time and found to be 75L, describe what had to happen to the pressure (if temperature remained constant). Include which law supports this observation.

Calculate the new pressure with

P1V1 = P2V2
The pressure had to decrease if the volume increased. See Boyle's Law

volume goes up, pressure goes up too

The pressure had to increase if the volume increased. See Charles' Law

It is stated that the temperature remained constant, therefore it's Boyle's Law, not Charles' and the pressure had to have decreased if the volume went up.

Charles law - volume/temp both increase because they are related

To understand this question, you need to consider the relationship between gas pressure and volume, as well as the relevant gas law that supports the observation.

The question mentions two sets of measurements for a gas: the first measurement gives a gas volume of 50L and a pressure of 300 kilopascals. The second measurement shows a gas volume of 75L. The question asks what must have happened to the pressure if the temperature remained constant and which gas law supports this.

To analyze this situation, you can use Boyle's Law, which states that at a constant temperature, the pressure and volume of a gas are inversely proportional. In other words, if one value increases, the other decreases, and vice versa.

In this case, the initial volume is 50L, and the gas is measured a second time with a volume of 75L. Since the volume has increased, according to Boyle's Law, the pressure of the gas must have decreased to maintain a constant temperature.

Therefore, to answer the question, you can state that the pressure of the gas decreased when the volume increased if the temperature remained constant. This observation is supported by Boyle's Law.