A gas `(C_(v.m) = (5)/(2)R)` behaving ideally is allowed to expand reversibly and adiabatically from `1` litre to `32` litre. Its initial temperature is `327^(@)C`. The molar enthalpy change (in `J//mol`) for the process is :
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
An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If T_(1) is initial temperature and T_(f) is the final temperature, which of the following statement is correct
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)
1L of NH_(3) " at " 27^(@)C is expanded adiabatically to x litres and final temperature is -123^(@)C . What is the value of x?
5.6 litre of helium gas at STP is adiabatically compressed to 0.7 litre. If the initial temperature of the gas is TK, work done in the process is (R is universal gas constant in SI units)
When 5 moles of an ideal gas is compressed isothermally, its volume decreases from 5 litre to 1 litre. If the gas is at 27^(@) C, find the work done on the gas.
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
