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?