What is the change in entropy of 10 moles of ideal diatomic gas that reversibly undergoes the isothermal expansion shown in the figure? The ideal gas constant is R = 8.314 J/(mol∙K).
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What is the change in entropy of 10 moles of ideal diatomic gas that reversibly undergoes the isothermal expansion shown in the figure? The ideal gas constant is R = 8.314 J/(mol∙K).
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- 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?A 23.9 g block of copper whose temperature is 382 K is placed in an insulating box with a 57.3 g block of lead whose temperature is 228 K. (a) What is the equilibrium temperature of the two-block system? (b) What is the change in the internal energy of the two-block system between the initial state and the equilibrium state? (c) What is the change in the entropy of the two-block system? The heat capacities of copper and lead are 386 J/kg-K and 128 J/kg-K, respectively. (a) Number i (b) Number i (c) Number i Units Units UnitsA 2.00-L container has a center partition that divides it into two equal parts as shown below. The left side contains n = 0.029 0 mol of H2 gas, and the right side contains n = 0.029 0 mol of 02 gas. Both gases are at room temperature and at atmospheric pressure. The partition is removed, and the gases are allowed to mix. What is the entropy increase of the system? J/K
- The temperature at the surface of the Sun is approximately 5,600 K, and the temperature at the surface of the Earth is approximately 291 K. What entropy change of the Universe occurs when 4.50 103 J of energy is transferred by radiation from the Sun to the Earth? ____________ J/KHow much energy must be transferred as heat for a reversible isothermal expansion of an ideal gas at 132°C if the entropy of the gas increases by 46.0 KConsider 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.