Assignment 2 thermo

You have four samples of ideal gas, each of which contains the same number of moles of gas and has the same initial temperature, volume, and pressure. You compress each sample to one-half of its initial volume. Rank the four samples in order from highest to lowest value of the final pressure. (i) A monatomic gas compressed isothermally; (ii) a monatomic gas compressed adiabatically; (iii) a diatomic gas compressed isothermally; (iv) a diatomic gas compressed adiabatically.

2mol ideal gas at 50oC temperature is available in an isolated system. By reducing the temperature of 1mol of this gas to 0oc under constant pressure, show whether it is possible to increase the temperature of the other 1mol to 100oC with the heat taken from here. It will be assumed that the molar heat capacities of the gas under constant pressure remain constant between these temperatures

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An ideal gas with molar heat capacity at constant volume, Cy,m = 3/2R undergoes a reversible isothermal expansion at 300 K until the pressure is half of its initial value with Pex = 0.500 bar and Tsur = 300 K. The ideal gas is with initial temperature, Ti = 300 K and initial pressure, P; = 1.00 bar. a) Identify the change in internal energy (AU) (in unit kJ mol*) and change in enthalpy (AH) (in unit kJ mol4). b) Calculate work done (w) (in unit kJ). c) Identify heat change (q) (in unit kJ). d) Calculate the change in entropy for the system (ASsys) and change in entropy of the surrounding (ASaur). Identify the change in total entropy (AStot). The unit of the change in entropy is J K1. e) State whether the process is spontaneous, not spontaneous or equilibrium.

(a) How much work is required to compress 4.99 mol of air at 20.4°C and 1.00 atm to one-tenth of the original volume by an isothermal process? (b) How much work is required to produce the same compression in an adiabatic process? (c) What is the final pressure in part (a)? (d) What is the final pressure in part (b)?

A sample of 3.0 moles of an ideal gas at 200 K and 200.0 kPa is compressed reversibly and adiabatically until the temperature reaches 250 K. Given the molar heat capacity at constant volume is 27.5 J K-1 mol-1, calculate q, w, delta U, delta H, the final pressure and the final volume. [0 J; 1.87 kJ; 1.87 kJ; 3.1112 kJ]

1) Consider a system consisting of 1.5 mol CO2 (g), initially at 15°C and 9.0 atm and confined to a cylinder of cross-section 100.0 cm2 , The sample is allowed to expand adiabatically against an external pressure of 1.5 atm until the piston has moved outwards through 15 cm. Assume that carbon dioxide may be considered a perfect gas with CV,m = 28.8 J K-l mol-1 , and calculate; (a) q, (b) w, (c) ∆U, (d) ∆T, (e) ∆S.

Consider a 5 L sample of CO₂(g) in a container with a movable piston at a temperature of 25 °C and 5.0 atm pressure. The gas is expanded reversibly by decreasing the pressure to 2.0 atm. Compare the final volume and temperature of the gas if the process were carried out (a) adiabatically or (b) isothermally. A) Vf(adiabatic) = Vf(isothermal); Tf(adiabatic) = Tf(isothermal) B) Vf(adiabatic) > Vf(isothermal); Tf(adiabatic) > Tf(isothermal) C) Vf(adiabatic) Vf(isothermal); Tf(adiabatic) Tf(isothermal)

a) 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.  (b)  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.  (c)  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.

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 ƏT, Əv /T

A sample of 3.0 moles of an ideal gas at 200 K and 200.0 kPa is compressed reversibly and adiabatically until the temperature reaches 250 K. Given the molar heat capacity at constant volume is 27.5 J K-1 mol-1 , calculate q, w, U, H, the final pressure and the final volume. Answer:[0 J; 1.87 kJ; 1.87 kJ; 3.1112 kJ]