Question

Choose the member with the higher entropy in each of the following pairs, and justify your choice. (Assume constant temperature, except in problem e). Show work for each please.

a) 1 mol of SO2(g) or 1 mol of SO3(g)

b) 1 mol of CO2(s) or 1 mol of CO2(g)

c) 3 mol of O¬2(g) or 2 mol of O3(g)

d) 1 mol of KBr(s) or 1 mol of KBr(aq)

e) Seawater at 2oC or at 23oC f) 1 mol of CF4(g) or 1 mol of CCl4(g)

Answer 1

Ans a) 1 mol of SO3 because it is the larger molecule with more number of bonds and vibrational modes than SO2.

b) 1 mol of CO2 (g) because though both the molecules have same structure but the gaseous CO2 has more kinetic energy and resultant collisions as compared to CO2 (s) hence more disorderness and entropy.

c) 3 moles of O2 , as entropy is directly related with the number of moles . More the number of moles , higher is the randomness or the entropy .

d) 1 mol of KBr (aq) , because liquids have higher entropy than solids .

e) Sea water at 23^oC , because the liquid particles tend to attain the kinetic energy at higher temperatures.

f) 1 mol of CCl4 because Cl atoms have more number of disordered electron locations than F.