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| The enthalpy is ________ when a A-A reactants form A-B products. |
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Definition
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| The entropy is ______ when there are more moles of gas on the reactant side than product side. |
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Definition
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Term
| What are the 3 things to look for when determining entropy? |
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Definition
1. moles of gas (which side has more?)
2. complexity of products/reactants
3. size/mass of compounds |
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Term
| The enthalpy is ___________ when A-B reactants for A-A products. |
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Definition
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| The entropy is ___________ when a complex/larger reactant forms a simpler/smaller product. |
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Definition
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Term
| The enthalpy is ____________ when breaking ionic compounds. |
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Definition
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Term
| The entropy is ___________ when the reactants form gaseous products. |
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Definition
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Term
| If a chemical reaction results in ONLY a phase change, do the enthalpy and entropy have the same or opposing signs? |
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Definition
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Term
| How do you find the percent yield of a reaction? |
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Definition
| (experimental yield/theoretical yield) X 100 |
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Term
| A reaction is spontaneous when its change in Gibbs free energy is ___________. |
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Definition
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Term
| A bond is _______ and less stable when it has _______ potential energy. |
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Definition
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Term
| Breaking bonds __________ energy while forming bonds ________ energy. |
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Definition
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Term
| Exothermic processes are ________ energetically stable. |
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Definition
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Term
| The ________ stable the products, the more likely the reaction to proceed to ___________. (____________) |
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Definition
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Term
| If the enthalpy is negative, then the process is ___________. |
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Definition
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Term
| Exothermic processes energetically favor _________. |
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Definition
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Term
| If the enthalpy is positive, then the process is ____________. |
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Definition
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Term
| Endothermic processes favor _____________. |
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Definition
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Term
| The stronger the intermolecular forces, the more ____________ the enthalpy. |
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Definition
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Term
| Based on Coulomb's Law, one may expect forces between ions to be stronger in these 2 scenarios: |
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Definition
1. the larger the charge of the ions (larger q's)
2. the smaller the size of the ions (smaller r) |
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Term
| The higher the entropy, the ________ configurations in a system. |
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Definition
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Term
| A phase change goes from solid to liquid, from liquid to gas. Thus, the process is ____________. |
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Definition
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Term
| A phase change goes from a gas to liquid, from a liquid to solid. Thus, the process is ____________. |
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Definition
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Term
| Chemical reactions in which the total entropy of the products is higher than the total entropy of the reactants are entropically __________. |
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Definition
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Term
| These 3 descriptions point towards a reaction that is entropically favored (entropy > 0). |
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Definition
1. fewer constraints
2. larger molar mass
3. more complexity |
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Term
| ___________ are dominant factors for entropy. |
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Definition
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Term
| Is favorability of a reaction temperature controlled? |
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Definition
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Term
| The more negative the Gibbs free energy is, the __________ the extent of the reaction and the more thermodynamically stable the ___________ than the ____________. |
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Definition
| larger; products; reactants |
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Term
| What is the Gibbs free energy equation? |
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Definition
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Term
| What is the 2nd Law of Thermodynamics? |
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Definition
| At constant T and P, G < 0 for thermodynamically favored processes. |
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Term
| The Gibbs free energy equates to ____ for elements in their standard state. |
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Definition
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Term
| Chemical reactions tend to reach an ______________________ in which the concentration of products and reactants does not vary over time. |
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Definition
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Term
Product-favored process: G < 0, K ___ 1
Reactant-favored process: G > 0, K ____ 1 |
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Definition
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