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Exam 1 - Pollard
Semester 2
33
Chemistry
Undergraduate 1
01/29/2012

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Term
The enthalpy is ________ when a A-A reactants form A-B products.
Definition
negative
Term
The entropy is ______ when there are more moles of gas on the reactant side than product side.
Definition
negative
Term
What are the 3 things to look for when determining entropy?
Definition
1. moles of gas (which side has more?)
2. complexity of products/reactants
3. size/mass of compounds
Term
The enthalpy is ___________ when A-B reactants for A-A products.
Definition
positive
Term
The entropy is ___________ when a complex/larger reactant forms a simpler/smaller product.
Definition
negative
Term
The enthalpy is ____________ when breaking ionic compounds.
Definition
positive
Term
The entropy is ___________ when the reactants form gaseous products.
Definition
positive
Term
If a chemical reaction results in ONLY a phase change, do the enthalpy and entropy have the same or opposing signs?
Definition
Same.
Term
How do you find the percent yield of a reaction?
Definition
(experimental yield/theoretical yield) X 100
Term
A reaction is spontaneous when its change in Gibbs free energy is ___________.
Definition
negative
Term
A bond is _______ and less stable when it has _______ potential energy.
Definition
weak; high
Term
Breaking bonds __________ energy while forming bonds ________ energy.
Definition
requires; releases
Term
Exothermic processes are ________ energetically stable.
Definition
more
Term
The ________ stable the products, the more likely the reaction to proceed to ___________. (____________)
Definition
more; completion; extent
Term
If the enthalpy is negative, then the process is ___________.
Definition
exothermic
Term
Exothermic processes energetically favor _________.
Definition
products
Term
If the enthalpy is positive, then the process is ____________.
Definition
endothermic
Term
Endothermic processes favor _____________.
Definition
reactants
Term
The stronger the intermolecular forces, the more ____________ the enthalpy.
Definition
negative
Term
Based on Coulomb's Law, one may expect forces between ions to be stronger in these 2 scenarios:
Definition
1. the larger the charge of the ions (larger q's)
2. the smaller the size of the ions (smaller r)
Term
The higher the entropy, the ________ configurations in a system.
Definition
more
Term
A phase change goes from solid to liquid, from liquid to gas. Thus, the process is ____________.
Definition
endothermic
Term
A phase change goes from a gas to liquid, from a liquid to solid. Thus, the process is ____________.
Definition
exothermic
Term
Chemical reactions in which the total entropy of the products is higher than the total entropy of the reactants are entropically __________.
Definition
favored
Term
These 3 descriptions point towards a reaction that is entropically favored (entropy > 0).
Definition
1. fewer constraints
2. larger molar mass
3. more complexity
Term
___________ are dominant factors for entropy.
Definition
Gases
Term
Is favorability of a reaction temperature controlled?
Definition
No.
Term
The more negative the Gibbs free energy is, the __________ the extent of the reaction and the more thermodynamically stable the ___________ than the ____________.
Definition
larger; products; reactants
Term
What is the Gibbs free energy equation?
Definition
G = H - TS
Term
What is the 2nd Law of Thermodynamics?
Definition
At constant T and P, G < 0 for thermodynamically favored processes.
Term
The Gibbs free energy equates to ____ for elements in their standard state.
Definition
0
Term
Chemical reactions tend to reach an ______________________ in which the concentration of products and reactants does not vary over time.
Definition
equilibrium state
Term
Product-favored process: G < 0, K ___ 1
Reactant-favored process: G > 0, K ____ 1
Definition
>; <
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