GO Figure 19-26 shows two paths that may be taken by a gas from an initial point i to a final point f . Path 1 consists of an isothermal expansion (work is 50 J in magnitude), an adiabatic expansion (work is 40 J in magnitude), an isothermal compression (work is 30 J in magnitude), and then an adiabatic compression (work is 25 J in magnitude). What is the change in the internal energy of the gas if the gas goes from point i to point f along path 2? Figure 19-26 Problem 59
GO Figure 19-26 shows two paths that may be taken by a gas from an initial point i to a final point f . Path 1 consists of an isothermal expansion (work is 50 J in magnitude), an adiabatic expansion (work is 40 J in magnitude), an isothermal compression (work is 30 J in magnitude), and then an adiabatic compression (work is 25 J in magnitude). What is the change in the internal energy of the gas if the gas goes from point i to point f along path 2? Figure 19-26 Problem 59
GO Figure 19-26 shows two paths that may be taken by a gas from an initial point i to a final point f. Path 1 consists of an isothermal expansion (work is 50 J in magnitude), an adiabatic expansion (work is 40 J in magnitude), an isothermal compression (work is 30 J in magnitude), and then an adiabatic compression (work is 25 J in magnitude). What is the change in the internal energy of the gas if the gas goes from point i to point f along path 2?
Suppose a monatomic ideal gas is changed from state A to state D by one of the processes shown on the PV diagram.where P1 = 3.10 and P2 = 6.20.
Find the total work done on the gas if it follows the constant-volume path AB followed by the constant-pressure path BCD.
An ideal gas expands at constant pressure. (a) Show that PΔV = nRΔT. (b) If the gas is monatomic, start from the definition of internal energy and show that ΔU = 3/2 Wenv, where Wenv is the work done by the gas on its environment. (c) For the same monatomic ideal gas, show with the first law that Q = 5/2 Wenv. (d) Is it possible for an ideal gas to expand at constant pressure while exhausting thermal energy? Explain.
An ideal diatomic gas expands adiabatically from 0.750 m3 to 1.50 m3. If the initial pressure and temperature are 1.50 x 105 Pa and 325 K , respectively, find (a) the number of moles in the gas, (b) the final gas pressure, (c) the final gas temperature, and (d) the work done on the gas.
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