The entropy of `v = 4.0` moles of an ideal gas increases by `Delta S = 23 J//K` due to the isothermal expansion. How many times should the volume `v = 4.0` moles of the gas be increased ?

Find the entropy increment of v = 2.0 moles of an ideal gas whose adiabatic exponent gamma = 1.30 if, as a result of a certain process, the gas volume increased alpha = 2.0 times while the pressure dropped beta = 3.0 times.

Suppose 0.5 moles of an ideal gas undergoes an isothermal expansion as energy is added to it as heat Q. graph shows the final volume V_(f) versus Q. the temperature of the gas is (use In 9 = 2 and R = (25)/(3) J//mol-K)

Suppose 0.5 moles of an ideal gas undergoes an isothermal expansion as energy is added to it as heat Q. graph shows the final volume V_(f) versus Q. the temperature of the gas is (use In 9 = 2 and R = (25)/(3) J//mol-K )

Suppose 0.5 moles of an ideal gas undergoes an isothermal expansion as energy is added to it as heat Q. graph shows the final volume V_(f) versus Q. the temperature of the gas is (use In 9 = 2 and R = (25)/(3) J//mol-K)

Suppose 0.5 moles of an ideal gas undergoes an isothermal expansion as energy is added to it as heat Q. graph shows the final volume V_(f) versus Q. the temperature of the gas is (use In 9 = 2 and R = (25)/(3) J//mol-K)

Suppose 0.5 moles of an ideal gas undergoes an isothermal expansion as energy is added to it as heat Q. graph shows the final volume V_(f) versus Q. the temperature of the gas is (use In 3 = 1 and R = (25)/(3) J//mol-K)

Entropy change for an isothermal expansion of one mole of an ideal gas from volume V_(1) to V_(2) is :

Temperature of 4 moles of gas increases from 300 K to 500 K find C_v if DeltaU = 5000 J .

Temperature of 4 moles of gas increases from 300 K to 500 K find C_v if DeltaU = 5000 J .