A sample of methane gas of mass 25 g at 250 K and 18.8 atm expands isothermally until its pressure is 2.5 atm. Calculate the change in entropy of the gas. (assume ideal gas behaviour).
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A sample of methane gas of mass 25 g at 250 K and 18.8 atm expands isothermally until
its pressure is 2.5 atm. Calculate the change in entropy of the gas. (assume ideal gas
behaviour).
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- Calculate the efficiency of the reversible cycle in figure for an ideal monoatomic gas where the transformation from 1->2 is described by the equation P2 V = A= constant (Assume V2 = 4 V1). P 3 1 V1 2 V2 V Hint: You might need to use the following integral: = √ + GA little bit of a problem can be found for Q1-2 = AU + W where the integral above may result useful to know.We trapped 28 kg of dry air, and it initially has standard pressure and temperature. The trapped air parcel rises in the atmosphere until the temperature is 188 K. What is the change in entropy if the pressure decreases by 28% after the parcel rises?Consider 4.00 mol of an ideal gas with a constant‑volume molar specific heat of 12.5 J/(mol·K), an initial temperature of 26.8 ∘C, and an initial pressure of 5.710×104 Pa. The state of the gas is then changed to a final temperature of 48.1 ∘C and a final pressure of 3.090×104 Pa. What is the change in the entropy Δ? of the gas during this process? The gas constant is 8.31 J/(mol·K).
- Two moles of an ideal gas undergo an irreversible isothermal expansion fromVa=100 liters to Vb=300 liters at T=300K.(a) What is the entropy change for this process?(b) What is the Gibbs free energy change?(c) Is this process spontaneous or not? Explain your answer.What is the entropy change for 3.20 mol of an ideal monatomic gas undergoing a reversible increase in temperature from 380 K to 425 K at constant volume?A 2000kg car travelling at 90km/hr crashes into a concrete wall. After that, the wreckage equilibrates to an ambient temperature of 24'C. Calculate the contribution of the crash to the entropy change of the universe.
- Consider the adiabatic free expansion of n moles of an ideal gas from volume V₁ to volume V2, where V₂ > V₁. [Hint: check lecture 19, chapter 5.6, process number 5. Note that such a process happens quasi-instantaneously, thus, it is irreversible.] (1) Calculate the change in entropy of the gas. (2) Calculate the change in entropy of the environment. (3) Evaluate the total change in entropy (AS = ASgas + ASenv.) for 1 mole, with V₂ = 2V/₁.Needs Complete solution with 100 % accuracy don't use chat gpt or ai plz plz plz.Suppose that 10 distinguishable particles are equipartitioned in a container that has 100 equal-sized compartments. What is the entropy on this system?