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Consider a sample containing 7.00 moles of a monatomic ideal gas at 10.0 °C and an...
Consider 8.0 moles of a monatomic ideal gas sample at 32°C and an initial pressure of 12.0 atm. The external pressure is lowered to 1.5 atm in a reversible manner. Calculate the final volume of the gas sample.
Twenty moles of a monatomic ideal gas (? = 5/3) undergo an adiabatic process. The initial pressure is 400 kPa and the initial temperature is 450 K. The final temperature of the gas is 320 K. In the situation above, the change in the internal energy of the gas, in kJ, is closest to:
Twenty moles of a monatomic ideal gas (γ = 5/3) undergo an adiabatic process. The initial pressure is 400 kPa and the initial temperature is 450 K. The final temperature of the gas is 320 K. In the situation above, the final volume of the gas, in SI units, is closest to: 0.19 0.35 0.23 0.27 0.31
A monatomic ideal gas at room temperature undergoes an adiabatic process such that its final pressure is 3.75 times its initial pressure. a) Did the gas expand or contract? (b) What is the ratio of its final volume to its initial volume? A monatomic ideal gas at room temperature undergoes an adiabatic process such that its final pressure is 3.75 times its initial pressure. (a) Did the gas expand or contract? o expand o contract (b) What is the ratio...
400 moles of an ideal monatomic gas are kept in a cylinder fitted with a light frictionless piston. The gas is maintained at the atmospheric pressure. Heat is added to the gas. The gas consequently expands slowly from an initial volume of 10 m3 to 15 m3. (a) Draw a P-V diagram for this process. (b) Is this thermodynamic process an isothermal expansion, an isobaric expansion or an adiabatic expansion? (c) Calculate the work done by the gas. (d) Calculate...
Ten. moles of ideal gas (monatomic), in the initial state P1=10atm, T1=300K are taken round the following cycle: a. A reversible isothermal expansion to V=246 liters, and b. A reversible adiabatic process to P=10 atm c. A reversible isobaric compression to V=24.6 liters Calculate the change of work (w), heat (q), internal energy (U), and entropy (S) of the system for each process?
Five moles of monatomic ideal gas have initial pressure 2.50 × 103 Pa and initial volume 2.10 m3. While undergoing an adiabatic expansion, the gas does 1780 J of work. What is the final pressure of the gas after the expansion? (kPa)
Five moles of monatomic ideal gas have initial pressure 2.50 × 103 Pa and initial volume 2.10 m3. While undergoing an adiabatic expansion, the gas does 1530 J of work. Part A What is the final pressure of the gas after the expansion? Units: kPa Units: kPa
The work done by two moles of a monatomic ideal gas (γ = 5/3) in expanding adiabatically is 920 J. The initial temperature and volume of the gas are 365 K and 0.110 m³. What is the final volume of the gas? [Hint: For an adiabatic process => T1V1γ-1 = T2V2γ-1]
The work done by two moles of a monatomic ideal gas (γ = 5/3) in expanding adiabatically is 920 J. The initial temperature and volume of the gas are 390 K and 0.120 m³. What is the final volume of the gas? [Hint: For an adiabatic process => T1V1γ-1 = T2V2γ-1]