A car tire contains 0.0360 m3 of air at a pressure of 2.70 ✕ 105 N/m2 (about 39 psi). How much more internal energy (in J) does this gas have than the same volume has at zero gauge pressure (which is equivalent to normal atmospheric pressure)? (Assume the tire pressure of 2.70 ✕ 105 N/m2 is absolute pressure, not gauge pressure. Assume for this question that air is monatomic.)

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delta V = B ( linear expansion coefficient ) Vo ( delta T )  i think you will need to find the expansion of both the container and the liquid then subtrct the liquid height from the height of the cylider. then the rest is just repeating with dif #s

Learning Goal: 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 I 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 = 8.3145 J/(mol · K). If p is in atmospheres and V is in liters, use R = 0.08206 L atm/(mol-K) instead. Part A A gas sample enclosed in a rigid metal container at…

Thank you! a) what is the kinetic energy per unit volume in an ideal gas at P=1.20 atm? b) what is the kinetic energy per unit volume in an ideal gas at P=287.0 atm?