CHEMISTRY COMMUNITY

204932558

log and ln are not the same. Ln(x) = 2.303log(x)

204932558

They are both state functions. Gibbs free energy is another example.

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Yes. Just make sure the electrons cancel out, and that the reaction with a more negative reduction potential is one being flipped.

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The graph for zero order reaction and first order reaction is {A} against time. But for second order reaction it's 1/[A] against time, which is why the slope is negative.

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The overall order of a reaction is the sum of the order of reactions for each reactants.

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[A}0 means the initial concentration. [A} is the concentration at any given time.

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If Ecell is positive, G is negative according to G=-nEf. It means the forward reaction is spontaneous and therefore favored, resulting in a K greater than 1.

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Reducing power of a species is the ability to reduce other another species. The higher the reducing power, the lower the reduction potential, and the less likely the species itself becomes reduced.

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Yes. OH- is used in basic environment and H+ is used in acidic environment. H20 is added after the the addition of H+ and OH-, balancing the whole equation.

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Because silver loses an electron and becomes oxidized and bromine gains an electron and becomes reduced. They both need to be included in the cell expression.

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It' s zero because we use the reaction of hydrogen as a reference to calculate the potential of other redox reactions.

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Yes, as no heat or matter flows into the system or exits the system.

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Kelvin = 273 + Degree Celcius. So it doesn't matter if you use either since the temperature difference is the same for both units.

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For the first part, the degeneracy is 1^64, so S = ln(1^64) = 0. For the second part, S = ln(4^64).

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The value is fixed and given, so you don't have to calculate it.

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Cellular respiration is an exergonic process. ATP is broken down to ADP and Pi during hydrolysis and energy is released.

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DeltaU = deltaQ + work. When the gas expands, it does work to the surrounding. But that loss of internal energy can be made up by the heat flowing into the system. So overall, U can stay unchanged.

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I think generally, there is a positive correlation between polarity and bond enthalpy but the there can be exceptions.

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If gas expands against vacuum no work is being done because the external pressure is zero. An example of work done on a system would be a piston compressing the gas inside a column. Work is done on the gas.

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Bond enthalpy is an average value of the energies required to break/form a certain type of bond in MANY MOLECULES. Therefore each molecule's bond enthalpy differs.

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Molar heat capacity uses J/Kg.M as the unit.

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"En" kinda sounds like "in" and "ex" means "exit".

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Being a state property means its value is always the same under certain conditions, no matter how the value is obtained.

CHEMISTRY COMMUNITY

Search found 23 matches

Re: Equations: ln Q vs. log Q [ENDORSED]

Re: State functions?

Re: Half-reactions

Re: slope

Re: Terminology "first-order" [ENDORSED]

Re: Deriving these Equations

Re: 14.31

Re: reducing power?

Re: Basic and Acidic conditions [ENDORSED]

Re: Cell Diagram

Re: Standard Cell Potential

Re: Isolated System

Re: Question 8.31

Re: Question 9.21

Re: 9. 43

Re: Exergonic [ENDORSED]

Re: Gas Expansion [ENDORSED]

Re: bond enthalpy [ENDORSED]

Re: Examples of work being done

Re: Bond Enthalpies

Re: mass in q = m(c) delta t

Re: Endo and Exothermic Ways to Remember

Re: Why can state properties be added?