Select the substance expected to have the largest standard entropy value at 25°C. Assume the same phase. O C2H5NH2 O C3H7NH2 O CH3NH2 O NH3

Calculate the entropy change when water freezes. Standard state entropy values for water:     H2O (s)     ΔS° = 41 J·mol-1·K-1      H2O (l)     ΔS° = 70 J·mol-1·K-1      H2O (g)     ΔS° = 189 J·mol-1·K-1

Endothermic reactions are more likely to be spontaneous. O True O False

Consider the two different systems, A and B, shown below.  If there are 3 particles with a total energy of 12 J, which system would have more entropy and why? Question 21 options:   System A has more entropy because it has greater separation between energy levels and hence more microstates than system B.   System B has more entropy because it has more than two microstates, whereas System A only has two microstates possible.   System A has more entropy because it has three microstates, whereas System B has less than three microstates possible.   System B has more entropy because it has more than three microstates, whereas System A only has three microstates possible.   System A has more entropy because it has more than one microstate, whereas System B only has one microstate possible.