1. gas to liquid

2. liquid to gas
3. solid to gas
4. solid to liquid
5. gas to solid
6. liquid to solid

Please label the reactions above into the groups:
ΔH=+, ΔS=+
ΔH=+, ΔS=-
ΔH=-, ΔS=+
ΔH=-, Δs=-

1. gas to liquid.

Condensing a gas to a liquid is exothermic; therefore dH is -.
Gas to liquid means more order; therefore, dS is -

To label the reactions into the groups, we need to consider the signs of enthalpy (ΔH) and entropy (ΔS). Here's how we can determine the groups for each reaction:

1. Gas to liquid: ΔH = -, ΔS = +
This reaction corresponds to a decrease in enthalpy (heat is released) while an increase in entropy occurs (randomness increases). It belongs to the group ΔH = -, ΔS = +.

2. Liquid to gas: ΔH = +, ΔS = +
This reaction corresponds to an increase in enthalpy (heat is absorbed) and an increase in entropy (randomness increases). It belongs to the group ΔH = +, ΔS = +.

3. Solid to gas: ΔH = +, ΔS = +
This reaction corresponds to an increase in enthalpy (heat is absorbed) and an increase in entropy (randomness increases). It also belongs to the group ΔH = +, ΔS = +.

4. Solid to liquid: ΔH = +, ΔS = -
This reaction corresponds to an increase in enthalpy (heat is absorbed), but a decrease in entropy (randomness decreases). It belongs to the group ΔH = +, ΔS = -.

5. Gas to solid: ΔH = +, ΔS = -
This reaction corresponds to an increase in enthalpy (heat is absorbed) and a decrease in entropy (randomness decreases). It belongs to the group ΔH = +, ΔS = -.

6. Liquid to solid: ΔH = -, ΔS = -
This reaction corresponds to a decrease in enthalpy (heat is released) and a decrease in entropy (randomness decreases). It belongs to the group ΔH = -, ΔS = -.

Therefore:

- ΔH = +, ΔS = +: Reactions 2, 3
- ΔH = +, ΔS = -: Reactions 4, 5
- ΔH = -, ΔS = +: Reaction 1
- ΔH = -, ΔS = -: Reaction 6