2.2 Consider a reversible process that takes an ideal gas from an initial state a to a final equilibrium state b. Show that the change in entropy of the gas is given by: (Tb AS = nC₂ In +nR In T a
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- A 2.00-mol sample of H2 gas is contained in the left side of the container shown below, which has equal volumes on the left and right. The right side is evacuated. When the valve is opened, the gas streams into the right side. (a) What is the entropy change of the gas? (b) Does the temperature of the gas change? Assume the container is so large that the hydrogen behaves as an ideal gas. (Wouldn't the temperature decrease because the temperature in a vacuum would be really cold?)A certain Carnot engine operates between 290 K and 450 K. The engine does 150 J of work for every 600 J of heat absorbed from the combustion of fuel. Find the actual efficiency and the theoretical efficiency. Find the heat exhausted to the cold reservoir. Find the entropy change of the hot reservoir and the cold reservoir, and the net change of entropy of the entire engine. (For this finding the change in entropy, Qh is negative as energy is leaving the reservoir, Qc is positive)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.
- Prove that entropy change from state A to state B is the same for both paths as shown in the TV diagram in the case of an ideal gas: 1. An adiabatic reversible expansion from point A (P1, V1, T1) to point B (P2, V2, T2) 2. An isobaric reversible process from A (P1, V1, T1) to C then followed by an isothermal reversible process from C to B (P2, V2, T2) P1, V1, T1 A Adiabatic Isobaric B P2, V2, T2 Isothermal C VConsider 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).. A rigid container (0.066 m3) is filled with an ideal gas (Cv = 2.5R) at 501K and 1.1 bar. Calculate the entropy changes asked in below. When an axial mixer is installed in a container and 15,000 J of work is applied to the gas under the insulation process, what is the entropy change of the gas?
- 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.Please help mePlease answer this with in 30 mins ! I will upvote .