1.00 mol of a perfect monoatomic gas at pressure 1.00 atm and 300 K is compressed adiabatically and reversibly until its final pressure is 15.00 atm. Calculate q, w, AU, AH, and AS. answers: q=0, delta s=o, w= delta U= 7.31 kJ, delta H= 72.2kJ
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- The constant-pressure heat capacity of a sample of a perfect gas was found to vary with temperature according to the expression Cp(JK–1) = 20.17 + 0.03665(T). Calculate q, w, ΔU, and ΔH when the temperature is raised from 25°C to 300°C(a) at constant pressure(b) at constant volumeCalculate the final temperature, the work done, and the change of internal energy when 1.00 mol NH3(g) at 298 K is used in a reversible adiabatic expansion from 0.50 dm3 to 2.00 dm3.The equation of state for a certain gas is given by P[(V/n)-b] = RT. Obtain an expression for the maximum work done by the gas in a reversible isothermal expansion from V1 to V2.
- The constant-pressure heat capacity of a sample of a perfect gaswas found to vary with temperature according to the expression Cp/(J K−1) = 20.17 + 0.3665(T/K). Calculate q, w, ΔU, and ΔH when the temperature is raised from 25 °C to 100 °C (i) at constant pressure, (ii) at constant volume.calculate the final temperature of a sample of carbon dioxide of mass 16.0g that is expanded reversibly and adiabatically from 500cm3 at 298.15K to 2dm3 if Cp,m is equal 37.11J/K.mol.The value of the heat capacity at constant volume, CV,,m, for a gas sample was found to vary with temperature according to the expression CV,m (in J mol-1 K-1 ) = 11.86 + 0.3665 T. Calculate the change in the internal energy of 1.00 mol of the gas when the temperature is raised from 25oC to 200oC at constant volume.
- A sample of blood plasma occupies 0.550 dm3 at 0 °c and 1.03 bar, and is compressed isothermally by 0.57 percent by being subjected to a constant external pressure of 95.2 bar. Calculate the magnitude of the work done.Two moles of a perfect gas with CV,m = 27.6 J K-1 mol-1 at 220 K and 200 kPa is compressed reversibly and adiabatically until the temperature reaches 255 K. Calculate q, w, ΔU, ΔH and the final pressure and volume.The constant-volume heat capacity of a gas can be measured by observing the decrease in temperature when it expands adiabatically and reversibly. The value of γ = Cp/CV can be inferred if the decrease in pressure is also measured and the constant-pressure heat capacity deduced by combining the two values. A fluorocarbon gas was allowed to expand reversibly and adiabatically to twice its volume; as a result, the temperature fell from 298.15 K to 248.44 K and its pressure fell from 202.94 kPa to 81.840 kPa. Evaluate Cp and Cv
- The constant-volume heat capacity of a gas can be measured by observing the decrease in temperature when it expands adiabatically and reversibly. The value of γ = Cp/CV can be inferred if the decrease in pressure is also measured and the constant-pressure heat capacity deduced by combining the two values. A fluorocarbon gas was allowed to expand reversibly and adiabatically to twice its volume; as a result, the temperature fell from 298.15 K to 248.44 K and its pressure fell from 202.94 kPa to 81.840 kPa. Evaluate Cp,m.In the isothermal reversible compression of 52 mmol of a perfect gas at 260 K, the volume of the gas reduced to 1/3 its initial volume, calculate work for this gas?When 3.0 mol O2 is heated at a constant pressure of 3.25 atm, itstemperature increases from 260 K to 285 K. Given that the molar heatcapacity of O2 at constant pressure is 29.4 J K−1 mol−1, calculate q, ΔH,and ΔU.