Calculate the entropy change involved in the isothermal expansion of 5 mol of ideal gas from a volume of 10 L to 100 L at 300 k

The entropy change involved in the isothermal reversible expansion of 2 mol of an ideal gas from a volume of 10 cm^(3) to a volume of 100 cm^(3) at 27^(@)C is-

The entropy change involed in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10dm^3 to a volume of 100dm^3 at 27^@C is

Work done during isothermal expension of one mole of an ideal gas from 10 atm to 1 atm at 300 K is

Calculate triangleq, W, triangleE for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0 bar to final pressure of 0.1 bar at a constant temperature of 273 K.

In isothermal expansion of 1 mol of an ideal gas, q=+12kJ . The value of w=______ and DeltaU =______.

Calculate the work done for a reversible isothermal compression of 1 mol ideal gas 20 L to half of its volume at 400K [R=8.314J*K^(-1)*mol^(-1)] .

Prove that, 1 mol of any ideal gas occupies a volume of 22.4 L at STP.

Calculate entropy change when 10 moles of an ideal gas expands reversibly and isothermally from an initial volume of 10 litre to 100 litre at 300K.

If the change in entropy of reversible isothermal expansion of 1 mol of an ideal gas is 9.135 " J mol"^(-1). K^(-1) , what will be the entropy change of the surroundings and universe ? If the above expansion of gas is allowed to occur against zero pressure, what will be the entropy change of the system and surroundings ?

The change in entropy for 2 mol ideal gas in an isothermal reversible expansion from 10 mL to 100 mL at 27^(@)C is-