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Karteikarten von J yadonknow, aktualisiert more than 1 year ago
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Erstellt von J yadonknow
vor fast 7 Jahre
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| Frage | Antworten |
| What happens when a reaction is energetically feasible? | Spontaneous reaction |
| What is free energy change? | ΔG The overall change in energy during a chemical reaction |
| What is ΔG made up of? | The enthalpy change ΔH - heat transfer between chemical system and surroundings The entropy change at the temperature of the reaction TΔS This is the dispersal of energy within the chemical system itself |
| How is the relationship between these two described? | GIBBS' EQUATION ΔG=ΔH-TΔS |
| What is needed for a reaction to be feasible? | ΔG<0 So reaction is exergonic |
| What are the units of ΔH and ΔS? | kJmol-1 JK-1mol-1 ΔS is much smaller, we change it to kjmol-1 by dividing by 1000 (question page 366) |
| What conditions support feasibility? | When ΔH is negative (so less energy out of system) When ΔS is positive, T increases ΔS significantly because TΔS |
| What is ΔG at minimum temperature? | ΔG=0 |
| How would you rearrange the Gibbs' equation to calculate the minimum temperature? | ΔH-TΔS=0 T=ΔH/ΔS (Convert K to C if applicable.) |
| How can endothermic reactions take place at RTP? | Some ionic compounds dissolve in water at RTP, cooling down the water, as long as ΔG<0 it'll be feasible |
| What are the limitations of predictions for feasibility? | Although ΔG may indicate thermodynamic feasibility, it doesn't take into account kinetics or the rate of a reaction i.e. H2O2, has a very high activation energy so a slow reation rate. |
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