What happens to the original pressure of a sample of a gas with each of the following changes. Triple the volume and half the kelvin temperature. Half the volume and double the kelvin temperature

School's probably out on this one, but here's practicing an answer:

Assuming the sample behaves as an ideal gas, PV = nRT enables predicting what happens under the change in conditions specified. Using subsripts to describe the before (b) and after (a) conditions: Pa/Pb = TaVb/TbVa. In the first case, the pressure would be 1/6 after and four times more in the second case.