Answer:
a. Zero
b. 19 J
c. - 5700 J
d. Zero
e. Zero
Explanation:
a. In an isothermal process, the change in temperature is zero. There are inter-molecular forces and the gas particles have perfect collision.
b. The entropy is given as
ΔS = nRln[tex]\frac{V2}{V1}[/tex]
= 1 (8.314)ln (10/1)
= 19 J
c. The Helmholtz energy change is given by A = U - TS
= 0 - (300× 19)
= 5 700 J
d. For an ideal gas, the mathematical equation for enthalpy, H with internal energy, E and PV can be expressed as:
H = U + PV
It follows that:
ΔH = ΔU + Δ(PV)
= ΔU + Δ(nRT)
However, in the question, Δn = 0, because the gas is mono atomic, there is no change in the number of moles and also he process if isothermal. Therefore,
ΔH = ΔU
However, for an isothermal process, the change in internal energy is ΔU = 0
Note that the equations are applicable to ideal gases.
e. The gas expansion is isothermal, so there is no temperature change. Therefore, energy change is zero.
