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.

If one mole of an ideal gas (C_(p.m.)=(5)/(2)R) is expanded isothermally at 300K until it’s volume is tripled, then change in entropy of gas is:

If one mole of an ideal gas C_p = 5/2 R is expanded isothermally at 300 k until it's volume is tripled., if expansion is carried out freely (P_(ext)=0), then DeltaS is :

1 mol of an ideal gas is allowed to expand isothermally at 27^(@)C untill its volume is tripled. Calculated Delya_(sys)S and Delta_(univ)S under the following conditions: a. The expansion is carried out reversibly. b. The expansion is a free expansion.

An ideal gas at 300K is expanded isothermally to double its volume,then pressure of the gas will be

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:

One mole of an ideal gas expands isothermally from 10 L to 100 L. Change in entropy of the process will be

One mole of a perfect gas expands isothermally to ten times its original volume. The change in entropy is

One mole of an ideal gas at 300K is expanded isothermally from an inital volume of 1 litre to 10 litres. The DeltaE for this process is (R=2cal mol^(-1)K^(-1))

One mole of an ideal gas at 250 K is expanded isothermally from an initial volume of 5 litre to 10 litres. The Delta E for this process is (R = 2 cal. Mol^(-1)K^(-1))

If 1 mole of an ideal gas expands isothermally at 37^(@)C from 15 litres to 25 litres, the maximum work obtained is :