Entropy and Gibb’s Free Energy

1)define entropy:

2)Name all of the changes in matter that result in an increase in entropy:

3)What are we describing when we discuss the spontaneity of a chemical reaction?

4)How is change in enthalpy related to the spontaneity of a reaction? Would it be positive or negative?

5)How is change in entropy related to the spontaneity of a reaction? Would it be positive or negative?

6)Is a rxn that has a ∆H of -134 kJ/mol and a ∆S of 624 J/molxK spontaneous at 57°C? What is the ∆G?

Balance the equations. Then, answer the following questions for the following reactions:

  1. What is the ΔH? Is this reaction endothermic or exothermic?
  2. What is the ΔS? Is there an increase or decrease in entropy?
  3. What is the ΔG at the given temperature? Is it spontaneous or non-spontaneous at that temperature?

7) NaOH + HCl(aq) ----> NaCl + H2O(l) (T=294.5 K)

8) NH4Cl ---> NH3(g) + HCl(g) (295.0 K)

9)Methane (CH4) burns spontaneously in the room when ignited. Verify this fact when the room is 150K.

10)What would the temperature have to be to cause the reaction from #7 to NOT be spontaneous?

Ans: more than 4141 K-773 kJ 92.4 kJ284.6J/K176kJ-110 kJ21.1J/K-103.8kJ-340 kJ

Entropy and Gibb’s Free Energy

1)define entropy:

2)Name all of the changes in matter that result in an increase in entropy:

3)What are we describing when we discuss the spontaneity of a chemical reaction?

4)How is change in enthalpy related to the spontaneity of a reaction? Would it be positive or negative?

5)How is change in entropy related to the spontaneity of a reaction? Would it be positive or negative?

6)Is a rxn that has a ∆H of -134 kJ/mol and a ∆S of 624 J/molxK spontaneous at 57°C? What is the ∆G?

7)Methane (CH4) burns spontaneously in the room when ignited. Verify this fact when the room is 150K.

8)What would the temperature have to be to cause the reaction from #7 to NOT be spontaneous?

Balance the equations. Then, answer the following questions for the following reactions:

A.What is the ΔH? Is this reaction endothermic or exothermic?

B.What is the ΔS? Is there an increase or decrease in entropy?

C.What is the ΔG at the given temperature? Is it spontaneous or non-spontaneous at that temperature?

9) NaOH + HCl(aq) ----> NaCl + H2O(l) (T=294.5 K)

10) NH4Cl ---> NH3(g) + HCl(g) (295.0 K)

Ans: more than 4141 K-773 kJ 92.4 kJ284.6J/K176kJ-110 kJ21.1J/K-103.8kJ-340 kJ

Entropy and Gibb’s Free Energy

1)define entropy:

2)Name all of the changes in matter that result in an increase in entropy:

3)What are we describing when we discuss the spontaneity of a chemical reaction?

4)How is change in enthalpy related to the spontaneity of a reaction? Would it be positive or negative?

5)How is change in entropy related to the spontaneity of a reaction? Would it be positive or negative?

6)Is a rxn that has a ∆H of -134 kJ/mol and a ∆S of 624 J/molxK spontaneous at 57°C? What is the ∆G?

7)Methane (CH4) burns spontaneously in the room when ignited. Verify this fact when the room is 150K.

8)What would the temperature have to be to cause the reaction from #7 to NOT be spontaneous?

Balance the equations. Then, answer the following questions for the following reactions:

A.What is the ΔH? Is this reaction endothermic or exothermic?

B.What is the ΔS? Is there an increase or decrease in entropy?

C.What is the ΔG at the given temperature? Is it spontaneous or non-spontaneous at that temperature?

9) NaOH + HCl(aq) ----> NaCl + H2O(l) (T=294.5 K)

10) NH4Cl ---> NH3(g) + HCl(g) (295.0 K)

Ans: more than 4141 K-773 kJ 92.4 kJ284.6J/K176kJ-110 kJ21.1J/K-103.8kJ-340 kJ