Answer:
1.38*10^-23ln(0.65/1)
=-5.7*10^-24
Explanation:
If all the microstates have equal probability of occurring, then Boltzmann's equation tells you that the entropy of the system is given by:
S = k*ln(W)
where W is the number of microstates available to the system.
In this case, we have a change in the number of microstates, and the question is asking for teh change in entropy:
S_final - S_initial = k*[ln(W_final) - ln(W_initial)]
ΔS = k*ln(W_final/W_initial)
We are told that in this case, W_final = 0.651*W_initial, so:
S = k*ln(0.651) = -10.00*10^-23 J/(K*particle)
To get this in terms of molar entropy, multiply by Avogadro's number:
ΔS = -10.00*10^-23 J/(K*particle) * (7.22*10^23 particles/mol) = -5.7*10^-24
