This activity aims to introduce the topic in a way that uses the students’ synthesis skills to piece together several pieces of information.
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The second law of thermodynamics
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Chemistry for the gifted and talented: the second law of thermodynamics
Level
Specification
- Northern Ireland
- A/AS level
- CCEA Chemistry
- Unit A2 1: Further Physical and Organic Chemistry
- 4.2 Enthalpy, entropy, and free energy
- 4.2.2 recall that the balance between entropy change and enthalpy change determines the feasibility of a reaction;
- 4.2.3 recall that entropy is a measure of disorder;
- 4.2.4 calculate the standard entropy change, ΔSӨ, in a chemical reaction using standard entropy data;
- 4.2.5 use the equation ΔG = ΔH - TΔS to calculate standard free energy changes;
- 4.2.6 recall that processes are feasible when the free energy change is negative;
- 4.2.7 recall that when the enthalpy change and the entropy change have the same sign, the feasibility of the process depends on the temperature, and calculate the temperature at which these processes start or cease to be feasible;
- 4.2 Enthalpy, entropy, and free energy
- Unit A2 1: Further Physical and Organic Chemistry
- CCEA Chemistry
- A/AS level
- England
- A/AS level
- AQA Chemistry
- Edexcel Chemistry
- Topic13: Enegetics II
- Topic 13B: Entropy
- 12. understand that, since some endothermic reactions can occur at room temperature, enthalpy changes alone do not control whether reactions occur
- 13. know that entropy is a measure of the disorder of a system and that the natural direction of change is increasing total entropy (positive entropy change)
- 14. understand why entropy changes occur during: changes of state; dissolving of a solid ionic lattice; reactions in which there is a change in the number of moles from reactants to products
- Topic 13B: Entropy
- Topic13: Enegetics II
- OCR Chemistry A
- Module 5: Physical chemistry and transition elements
- 5.2 Energy
- 5.2.2 Enthalpy and entropy
- a) explanation that entropy is a measure of the dispersal of energy in a system which is greater, the more disordered a system
- b) explanation of the difference in magnitude of the entropy of a system: of solids, liquids and gases; and for a reaction in which there is a change in the number of gaseous molecules
- 5.2.2 Enthalpy and entropy
- 5.2 Energy
- Module 5: Physical chemistry and transition elements
- A/AS level
- Scotland
- Advanced Higher
- SQA Chemistry
- Inorganic and Physical Chemistry
- Reaction feasibility
- Second and third laws of thermodynamics
- The Second Law of Thermodynamics states that the total entropy of a reaction system and its surroundings always increases for a spontaneous process.
- Heat energy released by the reaction system into the surroundings increases the entropy of the surroundings, whereas heat energy absorbed by the reaction system from the surroundings decreases the entropy of the surroundings.
- Second and third laws of thermodynamics
- Reaction feasibility
- Inorganic and Physical Chemistry
- SQA Chemistry
- Advanced Higher
- Wales
- A/AS level
- WJEC Chemistry
- Unit 3: PHYSICAL AND INORGANIC CHEMISTRY
- 3.7 Entropy and feasibility of reactions
- (a) entropy, S, of a system as a measure of the freedom possessed by particles within it and the increase in entropy towards a maximum for all natural changes
- (b) particles in a solid having much less freedom than those in a gas and that, other factors being equal, entropy increasing in the sequence S(gas) > S(liquid) > S(solid)
- (c) how to calculate an entropy change from absolute entropy values, ΔS = Sfinal – Sinitial
- (d) concept of Gibbs free energy change and how it is calculated using the relationship, ΔG = ΔH – TΔS
- (e) spontaneous reactions having a negative value for ΔG and how the effect of entropy change explains the spontaneous occurrence of endothermic processes
- 3.7 Entropy and feasibility of reactions
- Unit 3: PHYSICAL AND INORGANIC CHEMISTRY
- WJEC Chemistry
- A/AS level
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