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The ideal gas initially at 500 K and 1 atm was compressed adiabatically under two conditions...
Two mole of ideal gas, is compressed adiabatically in a piston/cylinder device from 2 bar and 25oC to 7 bar. The process is irreversible and requires 25% more work than a reversible, adiabatic compression from the same initial state to the same final pressure. What is the entropy change of the gas? Assume Cv=(5/2)R in this calculation.
An ideal gas, initially at a pressure of 9.1 atm and a temperature of 311 K, is allowed to expand adiabatically until its volume doubles.What is the gas’s final pressure, in atmospheres, if the gas is diatomic?
A monatomic ideal gas at an initial temperature of 390 K is compressed adiabatically from an initial volume of 120 L to a final volume of 40.0 L. What is the final temperature of the gas?
3) Suppose a di-atomic gas, initially at 300.00 K and 2.00 atm, is reduced adiabatically to one quarter of its initial volume. a) Find its final pressure Final rempreature Volume(m2) tob oniono ad b) If it was a mono-atomic gas, would the final pressure be larger or smaller than part a)? Explain c) If there are 5.00 mol of the gas, what is the final volume? (1.00 atm 101.3 kPa) Heebl oimelsonem to lom-a aowdns ls bni worle ploy o-die...
Suppose 1.50 m^3 of a gas with = 1.40, initially at 300 K and 1.0 atm, is suddenly compressed adiabatically to one half of its initial volume. (1 atm = 101.3 kPa). Find its final pressure final temperature
Neon gas is heated from 298 K (1 atm pressure) to 500 K under the following conditions: (a) at constant volume; (b) at constant pressure. In each case, find the molar entropy of the gas in its final state (at 500 K) given that its standard molar entropy at 298 K is 146.33 J/mol K. Assume that neon is ideal gas.
A monatomic ideal gas is initially at volume, pressure, temperature (Vi, Pi, Ti). Consider two different paths for expansion. Path 1: The gas expands quasistatically and isothermally to (Va, Pz. T2) Path 2: First the gas expands quasistatically and adiabatically (V2, P.,T-),where you will calculate P T. Then the gas is heated quasistically at constant volume to (Va. P2 T1). a. Sketch both paths on a P-V diagram. b. Calculate the entropy change of the system along all three segments...
An ideal gas is compressed at a constant pressure of 0.80 atm from 19.0 L to 12.0 L. The initial temperature of the gas is 27°C. 1 atm (atmosphere) = 1.013 ~ 10% Pa, 1 L (liter) = 10² m². What is the final temperature of the gas in °C? Hint: pV / T = nR, and n does not change, so you can use piVi / T1 = p2V2 / T2. Do not forget to convert the unit of...
One mole of ideal gas initially at 27 degree C is compressed adiabatically from 6 dm^3 to 3 dm^3 against constant external pressure of 15 atm. Calculate Delta E, Delta H, Q, and W for this process.
200 moles of an ideal gas at 1 atm pressure and T=300K, compress adiabatically to 2 atm, go isochorically back to 1 atm, then isobarically back to the initial conditions, how much work is done by the gas?