To understand the ideal gas law and be able to apply it to a wide variety of situations. the absolute temperature t, volume v, and pressure p of a gas sample are related by the ideal gas law, which states that pv=nrt. here n is the number of moles in the gas sample and r is a gas constant that applies to all gases. this empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. in applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and t must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as ^ -273˚c). if p is in pascals and v is in cubic meters, use r=8.3145j/(mol x k). if p is in atmospheres and v is in liters, use r=0.08206l x atm/(mol x k) instead. part a a gas sample enclosed in a rigid metal container at room temperature (20.0˚c) has an absolute pressure p1. the container is immersed in hot water until it warms to 40.0˚c. what is the new absolute pressure p2?