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Two moles of hydrogen gas, which can be regarded as ideal with Cp=28.8 J /(Kâmol) (independent of temperature), are initially at 298.15 K in a volume of 2.5 dm^3 and a pressure of 3 bar. The gas is expanded reversibly and adiabatically until the volume is 6 dm^3. Calculate the final pressure and temperature, âU, âH.
one mole of an ideal gas with Cp = (7/2)R and Cv = (5/2)Rexpands from P1 = 8 bar and T1 = 600 K to P2 = 1 bar by each of thefollowing paths: a) constant volume b) constant temperature c)adiabatically assuming mechanical reversibility calculate W Q deltaU and delta H for each process
in this example, 2.5 mol of an ideal gas with CV,m= 12.47Jmol-1K-1 is expanded adiabatically against a constant external pressure of 1 bar. The initial temperature and pressure of the gas are 325 K and 2.5bar respectively. The final pressure is 1.25 bar. Calculate the final temperature, q, w, ÎU and ÎH