Finding enthalpy, entropy, and Gibbs Free Energy charges

How do I answer questions such as the following?

Predict the sign of the thermodynamic quantity requested for the system shown (Answer choices include : +, -, 0, or not enough information)

1. Delta S for HCL (g) + NH3 (g) ---> NH4Cl(s)


2. Delta H for Br2 (g) ---> 2Br(g)


3. Delta S(surroundings) for H2O (l) ---> H2O (g) at 100 degrees C, 1 atm


4. Delta S(universe) for H2O (l) ---> H2O(g) at 100 degrees C, 1 atm


5. Delta G for H2O (l) ----> H2O (g) at 50 degrees C, 1 atm


6. Delta G for H20 (l) ----> H2O (g) at 100 degrees C, 1 atm

Can someone please explain how they derived each answer? This is part of a study guide and I really want to understand the information. Thank you so much! :)

1 negative because entropy decrease when gas goes to solid also there is less amount of moles. entropy is the state of disorder so if a gas which is in constant motion goes to solid, entropy decreases.

2 I am not sure for this one....

3 Well S of system is positive so I would say negative for surroundings.

4 at equilibrium S universe equals 0

5 I would say positive because enthalpy is positive and entropy is negative and at low temperatures it is positive.

6 I would say negative because enthalpy is positive and entropy is negative and at high temperatures it is negative.