1moles of a gas are initially initially under pressure 4 × 105 pa at t=300 k. in this problem, you will want to use the following relationships: definition of gibbs free energy: g=u−ts+pv equipartition: u=ndof2nkt+constentropy of an ideal gas: s=nklnv+const ideal gas law: pv=nktequation of state for system with excluded volume b: (v−nb)p=nkt

1)if the gas is ideal, how much does g change when the gas is allowed to expand isothermally until the pressure is reduced to 2 × 105 pa?

answer = -1729

2)how much did the chemical potential, change in part (1)? ? final-? initial= ?

3) now assume the gas has no interaction energy but does have an excluded volume per particle, b=1.9 × 10-28 m3, which means that s = nk ln(v-nb) + f(t, n) , where f is some function you won't need to know since t and n don't change. how much does g change when the gas expands isothermally until the pressure is reduced from 4 × 105 pa to 2 × 105pa? gfinal-ginitial= ?

4) how much did the chemical potential change in the process of part (3)? ? final-? initial= ?