Two moles of an ideal gas is expanded irreversibly and isothermally at `37^(@)C` until its volume is doubled and `3.41 KJ` heat is absorbed from surrounding. `DeltaS_("total")("system +surrounding")` is:
Two moles of an ideal gas is expanded irreversibly and isothermally at 37^(@)C until its volume is doubled and 3.41KJ heat is absorbed from surrounding. P DeltaS_("total") (system +surrounding) is:
Two mole of ideal gas is expanded irrversibly & isothermally at 27^(@) C until its volume is double and 3.3 kJ heat is absorbed from surrounding . Determine DeltaS_("System") & DeltaS_("surrounding" ) .
Two moles of an ideal gas is expanded isothermally and irreversibly at 27^(@)C from volume V_(1)" to" 2.5 V_(1)"and" 4.17KJ heat is absorbed from surroundings. Determine DeltaS_("sys") ?
One mole of an ideal gas is expanded freely and isothermally at 300K from 5L to 10L volume. If Delta E =0 , then Delta H is
Three moles of an ideal gas at 127^(@)C expands isothermally untill the volume is doubled. Calculate the amount of work done and heat absorbed.
One mole of an ideal gas is expanded isothermally at 300 K until its volume is tripled . Find the values of DeltaS_("sys") under the condition.
1 mole of an ideal gas is allowed to expand isothermally at 27^(@) C till its volume is tripled . If the expansion iscarried out reversibly then the DeltaS_("universe") will be?
If 1 mole of an ideal gas expands isothermally at 37^(@)C from 15 litres to 25 litres, the maximum work obtained is :
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
