Two moles of an ideal monoatomic gas is heated from `27 ^o C` to `627 ^o C`, reversibly and isochorically. The entropy of gas

The entropy change when two moles of ideal monatomic gas is heated from 200 "to" 300^(@) C reversibly and isochorically ?

4 moles of an ideal monoatomic gas is heated isobarically so that its absolute temperature increases 2 times. Then the entropy increment of the gas in this process is

One mole of an ideal and monoatomic gas is expanded reversibly and isothermally at 298K temperature according to the given diagram, calculate work done.

One mole of an ideal monoatomic gas is caused to go through the cycle shown in figure. Then the change in the internal energy of gas from a to b and b to c is respectively

The energy produced by the de - excitation of (1)/(1000) moles of H - atoms from 1^(st) excited to ground state is supplied to 2 moles of an ideal gas. 10 litres of that gas at 27^(@)C are allow to expand reversibly & isothermally. The final volume fo the gas will be

Two moles of an ideal monatomic gas occupies a volume V at 27 °C. The gas expands adiabatically to a volume 2V. Calculate (i) the final temperature of the gas and (ii) change in its internal energy.

One mole of an ideal monoatomic gas at 27^(@)C is subjected to a reversible isoentropic compression until the temperature reached to 327^(@)C . If the initial pressure was 1.0 atm , then find the value of ln P_(2) ( Given : ln 2=0.7)

Enthalpy of 1 mole monoatomic ideal gas is equals to :-

Two moles of an ideal monoatomic gas occupy a volume 2V at temperature 300K, it expands to a volume 4V adiabatically, then the final temperature of gas is

If one mole of monoatomic ideal gas expanded from 2 atm to 0.5 atm at 27°C, then the entropy change will be