5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K If C_(V) = 28 J K^(-1)mol^(-1) , calculate DeltaU and DeltapV for this process. (R = 8.0 JK^(-1)mol^(-1) ]
One mole of an ideal gas is heated from 300 K to 700 K at constant pressure. The change ininternal energy of the gas for this process is 8 kJ. What would be the change in enthalpy (in kJ) for the same process? ( R=8 " J"//"mole" -K )
1 mole of an ideal gas expands from 5 dm^(3) " to" 25 dm^(3) isothermally and irreversibly at 27^(@) C. Find work done in the process [R=8.3 J//mol//K ]
Three moles of an ideal gas (C_(v,m) = 12.5 J K^(-1) mol^(-1)) are at 300 K and 5 dm^(3) . If the gas is heated to 320K and the volume changed to 10 dm^(3) , calculate the entropy change.
One mole of an ideal gas at 250 K is expanded isothermally from an initial volume of 5 litre to 10 litres. The Delta E for this process is (R = 2 cal. Mol^(-1)K^(-1))
At 27^@C two moles of an ideal monatomic gas occupy a volume V. The gas expands adiabatically to a volume 2V . Calculate (a) final temperature of the gas (b) change in its internal energy and (c) the work done by the gas during the process. [ R=8.31J//mol-K ]
The specific heat of a gas constant volume is 20 J/mol K. when two moles of such gas is heated through 10^(@)C at constant pressure, what is the increase in thernal energy and work done? (R=8 J/mol K)
