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)
0.5 mole each of two ideal gases A (C_(v.m)= (5)/(2)R) and B (C_(v.m)=3R) are taken in a container and expanded reversibly and adiabtically, during this process temperature of gaseous mixture decreases from 350K and 250K. Find DH (in cal/mol) for the process
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
Calculate work done when 1 mole of an ideal gas is expanded reversibly from 20 L to 40 L at a constant temperature of 300 K.
One mole of an ideal gas at 300K is expanded isothermally reversibly from an initial volume of 1 litre to 10 litres. The Delta E for this process is (R = 2 cal mol^(-1) K^(-1) )
Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The internal energy change (in kJ) for the process (R = 8.3J)
One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:
One mole of an ideal gas for which C_(V)= 3//2R heated at a constant pressure of 1 atm from 25^(0)C "to" 100^(0)C What will be the amount of work done in the process?
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
