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
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)
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)
Two moles of helium gas (gamma=(5)/(3)) at 27^(@)C is expanded at constant pressure until its volume is doubled. Then it undergoes an adiabatic change until the temperature returns to its initial value. The work done during adiabatic process is ________ (universal gas constant = 8.3 "J mol"^(-1)K^(-1) )
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) )
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
