Assume that a sealed vessel at constant pressure of 1 bar initially contains 2.00 mol of NO
Question:
Assume that a sealed vessel at constant pressure of 1 bar initially contains 2.00 mol of NO2(g). The system is allowed to equilibrate with respect to the reaction 2NO2(g) ⇋ N2O4(g). The number of moles of NO2(g) and N2O4(g) at equilibrium is 2.00 – 2ξ and ξ , respectively, where ξ is the extent of reaction.
a. Derive an expression for the entropy of mixing as a function of ξ .
b. Graphically determine the value of ξ for which ΔS mixing has its maximum value.
c. Write an expression for G pure as a function of ξ . Use Equation (6.104) to obtain values of Gom for NO2 and N2O4.
d. Plot G mixture = G pure + ΔG mixing as a function of ξ for T = 298 K and graphically determine the value of ξ for which G mixture has its minimum value. Is this value the same as for part (b)?
Step by Step Answer:
a b A plot and a detail plot locating the maximum are shown below The value of at the maximu...View the full answer
