Calculated the final temprature (in Kelvin of a sample of argon of mass 12.0 g that is expanjded reversibly and adiabatically from 1.0 L at at 273 K to 3.0 L. (Take :`3sqrt9=2.08`)

Calculate the final pressure of a sample of carbon dioxide that expands reversibly and adiabatically from 57.4kPa and 1.0 to a final volume of 2.0L . Take gamma = 1.4

Calculate the final pressure of a sample of carbon dioxide that expands reversibly and adiabatically from 57.4kPa and 1.0 to a final volume of 2.0L . Take gamma = 1.4

Calculate the final temperature of a monoatomic ideal gas that is compressed reversible and adiabatically from 16L to 2L at 300 K :

Calculate the final temperature of a monoatomic ideal gas that is compressed reversible and adiabatically from 16L to 2L at 300 K :

Calculate the final temperature of a monoatomic idal gas that is compressed reversible and adiabatically from 16L to 2L at 300 K :

Calculate the final temperature of a sample of CO_(2) gas (16g) that is expanded reversibly and adiabatically from 0.5 litre to 2.0 litre at 298 K . Also calculate the work done by the gas. If C_(v.m) for CO_(2) is 42 J K^(-1) mol^(-1) . Calculate the enthalpy change in the process. (take C_(p)//C_(v) for CO_(2) as 1.33 )

A sample of carbon dioxide of mass 2.45 g at 27.0^(@) C is allowed to expand reversibly and adiabatically from 500 mL to 3.00 L What is the work done by the gass ? Take: (6)^(0.4)=2,R=(25)/(3)J//mol//K]

Calculate DeltaG (in bar-L) when a definite mass of a monoatomic ideal gas at 1 bar and 27^(@)C is expanded adiabatically against vacuum from 10 L to 20 L (In 2=0.7).

Calculate work involved in compression of 2 moles of H_(2) gas reversibly and isothermically from 1.2 L to 0.6 L at 300 K, if critical volume of H_(2) gas is 0.3L//"mol" . Given : R= 2cal//mol ,in10=2.3,log4=0.6,log5=0.7,log11=1.2]