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What is Isothermal Expansion of a van der Waals Gas?
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- Explain the difference between expansion work against constant pressure and work of reversible expansion and their consequences.Derive the work of reversible isothermal compression of a van der Waals gas. How does it compare to the work needed to compress the ideal gas in the limit of (a) low pressure, and (b) high pressure? Calculate the work done by a sample of Ar of mass 7.60 g that initially occupies 1.750 dm3 at 350 K, and expands reversibly and isothermally by 0.350 dm3 . Assume that argon obeys the van der Waals equation of state with a = 1.373 Pa m6 mol−2 and b = 3.200 × 10−5 m3 mol−1 . Compare to the corresponding value obtained in the previous problem for an ideal gas.When 229 J of energy is supplied as heat to 3.00 mol Ar(g), the temperature of the sample increases by 2.55 K. Calculate the molar heat capacities at constant volume and constant pressure of the gas.
- When 178 J of energy is supplied as heat at constant pressure to 1.9 mol of gas molecules, the temperature of the sample increases by 1.78 K. Calculate the molar heat capacities at constant volume and constant pressure of the gas.What is the heat capacity at constant volume of nn mole monatomic gas?A sample of helium (perfect gas) undergoes a following two-step process.1. Isothermal reversible expansion state 1 (p = 3.0 atm, V = 10.0 L T = 300K) to state 2 (V = 30 L))2. Isobaric compression from state 2 to state 3 (V = 10.0 L) A) What is w and q during step 1? B) What is w and q during step 2? C) What is delta U for the whole process? E) What is delta H for the whole process?
- What is the final temperature of a 1.00 mol sample of helium gas were it undergoes to a reversible adiabatic compression from 62.4 L to 31.9 L. Assume the initial temperature was 298 K and that the heat capacity is constant to 11.43J/mol KCalculate the molar heat capacity at constant pressure (Cp) for a diatomic H2 gas(y = 1.41) with molar heat capacity at constant volume (Cv) of 20.42 J/mol-K?Investigate the dependence of pV on V for real gases.
- Derive total amount of work involved for the expansion of 1mole of van der Waal's gas from v1 to V2 in an isothermal expansion (reversible)When 229 J of energy is supplied as heat at constant pressure to 3.0 mol Ar(g) the temperature of the sample increases by 2.55 K. Calculate the molar heat capacities at constant volume and constant pressure of the gas.Why does the isobaric molar heat capacity of most substances increase abruptly when that substance condenses from a gas to a liquid?