A system consisting of 0.0538 moles of a diatomic ideal gas is taken from state A to state C along the path in the figure below. A pressure-volume graph is plotted on a coordinate plane, where the horizontal axis is V (L), and the vertical axis is P (atm). The path consists of two line segments: a segment from point A (2,0.300) to point B (2,0.800) a segment from point B (2,0.800) to point C (8,0.500) Arrows along the path are aligned such that their tails are closer to point A than are their tips. (a) How much work is done on the gas during this process?   J (b) What is the lowest temperature of the gas during this process?   K Where does it occur? Point APoint B    Point C (c) Find the change in internal energy of the gas in going from A to C. Hint: Adapt the equation (for the change in internal energy of a monatomic ideal gas) ΔU =  3 2nRΔT =  3 2Δ(PV) =  3 2(PCVC − PAVA) to a diatomic ideal gas.  J (d) Find the energy delivered to the gas in going from A to C.  J

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Maxwell speed distribution

Maxwell-Boltzmann distribution or commonly known as Maxwell speed distribution, explains the division of the energy levels of the molecules of an ideal gas on the basis of the statistical theory. In 1859, Scottish physicist James Clerk Maxwell established the context for the distribution of molecular velocities for random molecules moving in a closed environment. This theory was generalized in 1871 by German physicist Ludwig Boltzmann. He improvised the theory to express the distribution of energy levels among different molecules.