P3.10 Derive the following expression for calculating the isothermal change in the constant volume heat capacity: (aCv/av)T = T(0²P/ƏT²)v.

3. Derive the thermodynamic equation of state for an ideal gas starting from internal energy then express this equation in a form without differentials. = -P +T| T LƏT.

Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.

gas undergoes an adiabatic expansion from 10 − 3 m 3 to 8 × 10 − 3 m 3 . The adiabatic line for the gas is given by P 3 V 5 = C (C is a constant). (a) Calculate the reversible work performed along the adiabatic line if the initial pressure is 10 5 P a and the initial volume = 10 − 3 m 3 . (b) What is the value of the constant C ? What is the unit of C ? (c) The gas reaches the final state in a two step process. An expansion at a constant initial pressure to the final volume followed by a decrease in pressure to the final volume 8 × 10 − 3 m 3 . What is the reversible work and heat in this process?

None

Q3) Thermodynamic Processes- 2.0 mol of a diatomic ideal gas undergoes a process in which it is compressed very slowly from state a (V. = 3.0 m³, P, = 1000 Pa) to state b (V, = 1.0 m³), in such a way that the system maintains thermal equilibrium with its surroundings at all times. P (Pa) 3000 2000 A. Find the change in internal energy during the process. 1000 B. Find the final pressure of the gas. 1 3 4 V(m³) C. Find the work done by the piston on the gas during this process. (Hint: Since Pis not constant during this process, it doesn't come out of the integral. Use the ideal gas law to find an expression for Pin terms of constants and the integration variable V) D. So what's the work done by the gas on the piston during this process? E. How much heat – if any - was transferred between the gas and surroundings during this process? Did heat flow from the gas to the surroundings or from the surroundings to the gas? Explain your reasoning. F. At the end of the process, is the average…