CHEMISTRY COMMUNITY

ng1D

What is a "chemistry" van't Hoff analysis to calculate ∆H°, ∆S° and ∆G°?

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Why does when q = qP then ∆U = ∆H - P∆V?

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Why do solutions of weak acids have higher pH values than solutions of strong acids at the same concentration?

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How do we show how the rate of change of one species in a reaction is related to that of another species? Are they in the same reaction?

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For one of the learning outcomes, it says to write rate laws for elementary reactions. What is meant by elementary reactions?

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How do we know when to use an integrated rate law or k[A]? What is the difference?

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How do we show how the instantaneous rate is obtained by drawing a tangent to the graph of concentration versus time? Is there an equation or graph we need to know?

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How can I tell the difference between order reactions? What is the difference between order reactions and rate reactions?

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What is the electromotive force and why does it represent the maximum potential difference?

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So given a reaction, we should be able to know if it is in its reduction or oxidation form?

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What do we need to know about the relationship between free energy and cell potentials?

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From the learning outcomes, what does it mean that we should understand what is meant by the electrochemical series?

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What is the difference between E°_cell= E°_cathode − E°_anode and E°_cell= E°+E° and when would I use one over the other?

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When balancing redox reactions, are we balancing the number of atoms or electrons?

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When a reaction of a system is at equilibrium, why is there no work done by the reaction?

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How is K temperature dependent using the Van't Hoff Equations?

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In lecture, a redox reaction was separated into half reactions. What are half reactions and how are they separated?

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Does pressure affect free energy? If it does how?

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I think that when pressure increases, volume decreases and when volume decreases entropy also decreases.

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What compositions and conditions of a system would help predict which of two systems has the greater entropy?

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In class on Friday, it was mentioned that ∆G°is not measured directly. What does it mean that ∆G°is not measured directly?

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How do you how Gibbs Free Energy change accompanying a process is related to the direction of a spontaneous reaction? Does it mean that when ∆G is negative, a reaction is spontaneous?

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∆S_surr=q_(rev)/T can also be written as ∆S_surr=∆H_(sys)/T. Why can ∆H be used in place of q?

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What is the relationship between microstates and degeneracy? Are they the same thing or are the number of microstates related to degeneracy?

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In thermodynamic, why is it necessary to identify which type of system a reaction is occurring in?

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What are the differences and similarities between deltaU and deltaH?

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When a reaction has a constant pressure, why is PdeltaV insignificant when the reaction involves solids and liquids?

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What is the relationship between volume and work? What would happen if volume increases/decreases?

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Are phase changes identified by a change from solid to liquid to gas and vice versa? And why does temperature remain constant during a phase change?

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What is the standard state of a substance and how do I know if a substance is in its standard state?

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Yes, freezing would be an exothermic reaction because heat is released.

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What is Hess's Law and how does it relate to state properties?

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How do you tell whether a reaction is endothermic or exothermic by the direction of heat flow?

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Can someone explain why solutions of weak acids have higher pH values than solutions of strong acids at the
same concentration?

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How do we use equilibrium constants to predict solubility?

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There are learning outcomes for acids and bases on our class website. The link for the acid and bases learning outcomes: https://lavelle.chem.ucla.edu/wp-content/supporting-files/Chem14B/Chem14B_Outline2_Acids_and_Bases.pdf

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What is the difference between calculating weak acids or bases and strong acids or bases?

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You would add for the reactants and subtract for products

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What happens if N2 is increased, NH3 is increased, or H2 decreased? What does it mean when they go to the left or right?

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Q and K are similar in that they are calculated in the same way, Q = [P]/[R] and K = [P]/[R].

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Gases are included in equilibrium constant equations.

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The equilibrium constant will remain the same because it is not affected by the amount of reactants or products. If there is a higher pressure of reactant, the pressure of the products will change so that it equals the equilibrium constant, which remains constant.

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Kp is the partial pressure equilibrium constant, which would be used for gases, but partial pressure can be converted into concentration of a gas by using the ideal gas law. I think because partial pressure can be converted into concentration, Kc can be used for gases.

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