2 mole of an ideal mono atomic gas undergoes a reversible process for which `PV^(2)=C`. The gas is expanded from initial volume of 1L to a final volume of 3L starting from initial temperature of 300K. Find `DeltaH` for the process
One mole of an ideal monoatomic gas undergoes a process described by the equation PV^(3)=constant . The heat capacity of the gas during this process is
One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1l to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R =0.082L atm mol^(-1)K^(-1)= 8.3J mol^(-1) K^(-1) ]
1 mole of an ideal gas A ( C_(v,m)=3R ) and 2 mole of an ideal gas B are (C_(v.m)= (3)/(2)R) taken in a constainer and expanded reversible and adiabatically from 1 litre of 4 litre starting from initial temperature of 320K. DeltaE or DeltaU for the process is (in Cal) (Give your answer after divide with 240)
At 27^(@)C , two moles of an ideal mono-atomic 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 = 8.31 J/mol K)
One mole of an ideal gas expands at a constant temperature of 300 K from an initial volume of 10 litres to a final volume of 20 litres. The work done in expanding the gas is (R=8.31J/mole-K)
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
