When two moles of an ideal gas `(C_(p.m.)=(5)/(2)R)` heated form 300K to 600K at constant pressure, the change in entropy of gas `(DeltaS)` is:

When two mole of an ideal gas (C​_(p.m.) = 5/2R) heated from 300K to 600K at constant volume. The change in entropy of gas will be :-

When two moles of ideal gas (C_v = 3/2R) heated from 300 K to 600 K at constant volume, calculate DeltaS_(gas) :

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.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.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.m)=(5)/(2)R) is expaned isothermally at 300K until it's volume is tripled , then change in entrop of gas is R in 3 if above expansion is carried out freely (P_(ext)=0) , then find DeltaS ?

One mole of an ideal gas is heated from 300 K to 700 K at constant pressure. The change ininternal energy of the gas for this process is 8 kJ. What would be the change in enthalpy (in kJ) for the same process? ( R=8 " J"//"mole" -K )

Pressure of 10 moles of an ideal gas is changed from 2 atm to 1 at against constant external pressure without change in temperature. If surrounding temperature (300K) and pressure (1 atm) always remains constant then calculate total entropy change (DeltaS_("system")+DeltaS_("surrounding")) for given process. [Given : ? n2 = 0.70 and R = 8.0 J/mol/K]