Two mole of an ideal gas is heated at constant pressure of one atmosphere from `27^(@)C` to `127^(@)C`. If `C_(v,m)=20+10^(-2)"T JK"^(-1).mol^(-1)`, then q and `DeltaU` for the process are respectively:
10 mole of an ideal gas is heated at constant pressure of one atmosphere from 27^(@)C to 127^(@)C . If C_(v,m)=21.686+10^(-3)T(JK^(-1).mol^(-1)) , then DeltaH for the process is :
3.0 moles of ideal gas is heated at constant pressure from 27^(@)C to 127^(@)C . Then the work expansion of gas is
One mole of an ideal monoatomic gas is heated at a constant pressure of 1 atmosphere from 0^(@) C to 100^(@0 C. Work done by the gas is
One mole of an ideal monoatomic gas is heated at a constant pressure of one atmosphere from 0^(@) to 100^(@)C. Then the change in the internal energy is
The work done is heating one mole of an ideal gas at constant pressure from 15^(@)C to 25^(@)C is
If one mole of an ideal gas with C_(v) = (3)/(2) R is heated at a constant pressure of 1 atm 25^(@)C to 100^(@)C . Which is correct
One moles of an ideal gas which C_(V) = 3//2 R is heated at a constant pressure of 1 atm from 25^(@)C to 100^(@)C . Calculate DeltaU, DeltaH and the entropy change during the process.
Two moles of an ideal monatomic gas is heated at constant pressure so that its temperature increases from 127^° C to 227^° C , then work done by gas
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
