How is the standard cell potential (E°cell) calculated from standard reduction potentials (E°red)?

E°cell = E°red(cathode) - E°red(anode). A positive E°cell denotes a thermodynamically spontaneous reaction.

Write the Nernst equation for calculating non-standard cell potential (Ecell).

Ecell = E°cell - (R*T / (n*F)) * ln(Q) = E°cell - (0.0592 V / n) * log10(Q) at 298 K.

What condition involving ion product (Qsp) and solubility product (Ksp) indicates that a precipitate will form?

A precipitate forms when Qsp > Ksp (supersaturated solution).

What products are obtained by oxidizing a primary alcohol versus a secondary alcohol with strong oxidizing agents (e.g., KMnO4 or Jones reagent)?

Primary alcohols are oxidized to carboxylic acids (via aldehyde intermediates); secondary alcohols are oxidized to ketones (tertiary alcohols resist oxidation).

What is the role of a salt bridge in a galvanic (voltaic) cell?

To maintain electrical neutrality by permitting spectator anions to migrate toward the anode and cations toward the cathode, preventing charge buildup.

According to Le Chatelier's principle, how does increasing system pressure by decreasing volume affect a gaseous equilibrium?

The equilibrium shifts toward the side of the balanced equation with fewer total moles of gas to relieve the pressure.

What chemical transformation occurs during Fischer esterification?

A carboxylic acid reacts with an alcohol in the presence of an acid catalyst to produce an ester and water via nucleophilic acyl substitution.

What are the units of the rate constant (k) for zero-order, first-order, and second-order chemical reactions?

Zero-order: M/s (mol/(L*s)); First-order: s^-1; Second-order: M^-1 * s^-1 (L/(mol*s)).

What is the common ion effect on salt solubility?

The solubility of a sparingly soluble salt is markedly decreased in the presence of a soluble second salt that shares a common ion, driven by Le Chatelier's shift.

How does raising the temperature affect the equilibrium constant (K) for an exothermic reaction versus an endothermic reaction?

For an exothermic reaction (heat as product), increasing T decreases K (shifts left); for an endothermic reaction (heat as reactant), increasing T increases K (shifts right).

How does comparing the reaction quotient (Q) to the equilibrium constant (K) predict the direction of net reaction?

If Q K, reverse reaction proceeds (shifts left).

What is the general differential rate law for a reaction aA + bB -> products, and how are reaction orders determined?

Rate = k[A]^m[B]^n, where m and n are reaction orders with respect to A and B, determined strictly experimentally (not from stoichiometric coefficients).

Which plotted variables yield a straight line for zero-order, first-order, and second-order integrated rate laws?

Zero-order: [A] vs t (slope = -k); First-order: ln[A] vs t (slope = -k); Second-order: 1/[A] vs t (slope = +k).

What thermodynamic equation relates standard Gibbs free energy change (ΔG°) to standard cell potential (E°cell)?

ΔG° = -n * F * E°cell, where n is moles of transferred electrons and F is Faraday's constant (96,485 C/mol e-).

What defines an electrophile versus a nucleophile in organic reaction mechanisms?

An electrophile is an electron-deficient species (Lewis acid) seeking electron density; a nucleophile is an electron-rich species with a lone pair or pi bond (Lewis base) that donates electrons to form a bond.

What is dynamic chemical equilibrium, and what is true regarding forward and reverse reaction rates?

A closed system state where the rates of forward and reverse reactions are equal (rf = rr), resulting in constant macroscopic concentrations over time.

What defines aromaticity in planar cyclic conjugated molecules according to Hückel's rule?

The ring must be cyclic, planar, fully conjugated with a continuous ring of p-orbitals, and contain (4n + 2) pi electrons (where n is a non-negative integer: 2, 6, 10, 14...).

What structural feature distinguishes an aldehyde from a ketone?

Both contain a carbonyl group (C=O); an aldehyde has the carbonyl bonded to at least one hydrogen atom (terminal R-CHO), while a ketone has the carbonyl bonded to two carbon groups (internal R-CO-R').

What defines a chiral center (stereocenter) in an organic molecule?

An sp3-hybridized tetrahedral carbon atom bonded to four chemically distinct substituent groups.

What is the rate-determining step (RDS) in a multi-step reaction mechanism?

The slowest elementary step with the highest activation energy barrier, which dictates the overall reaction rate and rate law.

What is the relationship between enantiomers and diastereomers in stereochemistry?

Enantiomers are non-superimposable mirror-image stereoisomers with identical physical properties except optical rotation; diastereomers are stereoisomers that are not mirror images and possess different physical and chemical properties.

What thermodynamic equation connects standard cell potential (E°cell) to the equilibrium constant (K) at 298.15 K?

E°cell = (R*T / (n*F)) * ln(K) = (0.0592 V / n) * log10(K).

Write the Arrhenius equation and identify all variables and physical constants.

k = A * exp(-Ea / (R*T)), where k is rate constant, A is pre-exponential frequency factor, Ea is activation energy, R is gas constant (8.314 J/(mol*K)), and T is temperature in Kelvin.

How does a chemical catalyst accelerate a reaction without being consumed?

It provides an alternative reaction pathway with a lower activation energy (Ea), increasing rate constants of both forward and reverse reactions equally.

How do galvanic cells and electrolytic cells differ in spontaneity and external energy requirements?

Galvanic cells produce electrical energy spontaneously from chemical reactions (ΔG 0); electrolytic cells consume external electrical voltage to drive non-spontaneous reactions (ΔG > 0, Ecell < 0).

Why are aliphatic amines basic and nucleophilic in organic reactions?

The nitrogen atom possesses a non-bonding lone pair of electrons available to accept a proton (Brønsted base) or attack electrophilic centers (Lewis base/nucleophile).

How are primary (1°), secondary (2°), and tertiary (3°) alcohols classified structurally?

By the number of carbon atoms bonded to the carbinol carbon carrying the -OH group: 1° is bonded to one carbon, 2° to two carbons, and 3° to three carbons.

What is the solubility product constant (Ksp) expression for the dissolution of silver chromate, Ag2CrO4(s) 2 Ag+(aq) + CrO4^2-(aq)?

Ksp = [Ag+]^2 * [CrO4^2-], with solids omitted from mass action expressions.

What is the relationship between the equilibrium constants Kc and Kp for an ideal gas reaction?

Kp = Kc * (R*T)^Δn, where Δn = (moles of gaseous products) - (moles of gaseous reactants), and R = 0.08206 L*atm/(mol*K).

What is the half-life equation for a first-order chemical reaction, and why is it unique?

t_1/2 = ln(2) / k ≈ 0.693 / k; it is completely independent of the initial reactant concentration [A]0.

In an electrochemical cell, which electrode is the site of oxidation, and which is the site of reduction?

Oxidation always occurs at the anode (An Ox); reduction always occurs at the cathode (Red Cat).

Química Inorgánica — Avanzado (C1/C2) 4: Chemical Kinetics, Equilibrium, Electrochemistry & Organic Functional Groups

[Español] Química Inorgánica: Reaction rates, rate laws, Le Chatelier's principle, equilibrium constants, galvanic/electrolytic cells, and organic functional groups

Level: advanced
Languages: es → es
Cards: 32
Markdown: Química Inorgánica — Avanzado (C1/C2) 4: Chemical Kinetics, Equilibrium, Electrochemistry & Organic Functional Groups (.md)

Flashcards (32)

#	Front (Term / Question)	Back (Definition / Answer)
1	How is the standard cell potential (E°cell) calculated from standard reduction potentials (E°red)?	E°cell = E°red(cathode) - E°red(anode). A positive E°cell denotes a thermodynamically spontaneous reaction.
2	Write the Nernst equation for calculating non-standard cell potential (Ecell).	Ecell = E°cell - (RT / (nF)) * ln(Q) = E°cell - (0.0592 V / n) * log10(Q) at 298 K.
3	What condition involving ion product (Qsp) and solubility product (Ksp) indicates that a precipitate will form?	A precipitate forms when Qsp > Ksp (supersaturated solution).
4	What products are obtained by oxidizing a primary alcohol versus a secondary alcohol with strong oxidizing agents (e.g., KMnO4 or Jones reagent)?	Primary alcohols are oxidized to carboxylic acids (via aldehyde intermediates); secondary alcohols are oxidized to ketones (tertiary alcohols resist oxidation).
5	What is the role of a salt bridge in a galvanic (voltaic) cell?	To maintain electrical neutrality by permitting spectator anions to migrate toward the anode and cations toward the cathode, preventing charge buildup.
6	What functional group results from the condensation reaction between a carboxylic acid derivative and an amine?	An amide bond (-CO-NRR').
7	According to Le Chatelier's principle, how does increasing system pressure by decreasing volume affect a gaseous equilibrium?	The equilibrium shifts toward the side of the balanced equation with fewer total moles of gas to relieve the pressure.
8	What chemical transformation occurs during Fischer esterification?	A carboxylic acid reacts with an alcohol in the presence of an acid catalyst to produce an ester and water via nucleophilic acyl substitution.
9	What are the units of the rate constant (k) for zero-order, first-order, and second-order chemical reactions?	Zero-order: M/s (mol/(Ls)); First-order: s^-1; Second-order: M^-1 s^-1 (L/(mol*s)).
10	What is the common ion effect on salt solubility?	The solubility of a sparingly soluble salt is markedly decreased in the presence of a soluble second salt that shares a common ion, driven by Le Chatelier's shift.
11	How does raising the temperature affect the equilibrium constant (K) for an exothermic reaction versus an endothermic reaction?	For an exothermic reaction (heat as product), increasing T decreases K (shifts left); for an endothermic reaction (heat as reactant), increasing T increases K (shifts right).
12	How does comparing the reaction quotient (Q) to the equilibrium constant (K) predict the direction of net reaction?	If Q < K, forward reaction proceeds (shifts right); if Q = K, system is at equilibrium; if Q > K, reverse reaction proceeds (shifts left).
13	What is the general differential rate law for a reaction aA + bB -> products, and how are reaction orders determined?	Rate = k[A]^m[B]^n, where m and n are reaction orders with respect to A and B, determined strictly experimentally (not from stoichiometric coefficients).
14	Which plotted variables yield a straight line for zero-order, first-order, and second-order integrated rate laws?	Zero-order: [A] vs t (slope = -k); First-order: ln[A] vs t (slope = -k); Second-order: 1/[A] vs t (slope = +k).
15	What thermodynamic equation relates standard Gibbs free energy change (ΔG°) to standard cell potential (E°cell)?	ΔG° = -n * F * E°cell, where n is moles of transferred electrons and F is Faraday's constant (96,485 C/mol e-).
16	What defines an electrophile versus a nucleophile in organic reaction mechanisms?	An electrophile is an electron-deficient species (Lewis acid) seeking electron density; a nucleophile is an electron-rich species with a lone pair or pi bond (Lewis base) that donates electrons to form a bond.
17	What is dynamic chemical equilibrium, and what is true regarding forward and reverse reaction rates?	A closed system state where the rates of forward and reverse reactions are equal (rf = rr), resulting in constant macroscopic concentrations over time.
18	What defines aromaticity in planar cyclic conjugated molecules according to Hückel's rule?	The ring must be cyclic, planar, fully conjugated with a continuous ring of p-orbitals, and contain (4n + 2) pi electrons (where n is a non-negative integer: 2, 6, 10, 14...).
19	What structural feature distinguishes an aldehyde from a ketone?	Both contain a carbonyl group (C=O); an aldehyde has the carbonyl bonded to at least one hydrogen atom (terminal R-CHO), while a ketone has the carbonyl bonded to two carbon groups (internal R-CO-R').
20	What defines a chiral center (stereocenter) in an organic molecule?	An sp3-hybridized tetrahedral carbon atom bonded to four chemically distinct substituent groups.
21	What is the rate-determining step (RDS) in a multi-step reaction mechanism?	The slowest elementary step with the highest activation energy barrier, which dictates the overall reaction rate and rate law.
22	What is the relationship between enantiomers and diastereomers in stereochemistry?	Enantiomers are non-superimposable mirror-image stereoisomers with identical physical properties except optical rotation; diastereomers are stereoisomers that are not mirror images and possess different physical and chemical properties.
23	What thermodynamic equation connects standard cell potential (E°cell) to the equilibrium constant (K) at 298.15 K?	E°cell = (RT / (nF)) * ln(K) = (0.0592 V / n) * log10(K).
24	Write the Arrhenius equation and identify all variables and physical constants.	k = A * exp(-Ea / (RT)), where k is rate constant, A is pre-exponential frequency factor, Ea is activation energy, R is gas constant (8.314 J/(molK)), and T is temperature in Kelvin.
25	How does a chemical catalyst accelerate a reaction without being consumed?	It provides an alternative reaction pathway with a lower activation energy (Ea), increasing rate constants of both forward and reverse reactions equally.
26	How do galvanic cells and electrolytic cells differ in spontaneity and external energy requirements?	Galvanic cells produce electrical energy spontaneously from chemical reactions (ΔG < 0, Ecell > 0); electrolytic cells consume external electrical voltage to drive non-spontaneous reactions (ΔG > 0, Ecell < 0).
27	Why are aliphatic amines basic and nucleophilic in organic reactions?	The nitrogen atom possesses a non-bonding lone pair of electrons available to accept a proton (Brønsted base) or attack electrophilic centers (Lewis base/nucleophile).
28	How are primary (1°), secondary (2°), and tertiary (3°) alcohols classified structurally?	By the number of carbon atoms bonded to the carbinol carbon carrying the -OH group: 1° is bonded to one carbon, 2° to two carbons, and 3° to three carbons.
29	What is the solubility product constant (Ksp) expression for the dissolution of silver chromate, Ag2CrO4(s) <-> 2 Ag+(aq) + CrO4^2-(aq)?	Ksp = [Ag+]^2 * [CrO4^2-], with solids omitted from mass action expressions.
30	What is the relationship between the equilibrium constants Kc and Kp for an ideal gas reaction?	Kp = Kc * (RT)^Δn, where Δn = (moles of gaseous products) - (moles of gaseous reactants), and R = 0.08206 Latm/(mol*K).
31	What is the half-life equation for a first-order chemical reaction, and why is it unique?	t_1/2 = ln(2) / k ≈ 0.693 / k; it is completely independent of the initial reactant concentration [A]0.
32	In an electrochemical cell, which electrode is the site of oxidation, and which is the site of reduction?	Oxidation always occurs at the anode (An Ox); reduction always occurs at the cathode (Red Cat).