Chemistry 5.2-5.3 Chemical Concepts

<p>Varying the concentration of one of the aqueous reactants. (C)</p> Signup and view all the answers

<p>The ratio of product to reactant concentrations at any point in a reaction. (D)</p> Signup and view all the answers

<p>It is the slowest step in the reaction mechanism. (D)</p> Signup and view all the answers

<p>An entity formed and consumed during the reaction sequence, but is neither a reactant nor a final product. (A)</p> Signup and view all the answers

<p>They reflect the concentrations at a specific moment. (C)</p> Signup and view all the answers

<p>They always have a first order rate law. (B)</p> Signup and view all the answers

<p>The equilibrium will shift to produce the missing substance. (A)</p> Signup and view all the answers

<p>The rates of dissolving and precipitating are equal. (A)</p> Signup and view all the answers

<p>Because it's unlikely for any three molecules to simultaneously collide. (B)</p> Signup and view all the answers

<p>It is written directly from the balanced equations representing elementary steps. (D)</p> Signup and view all the answers

<p>The solution contains the maximum possible amount of solute. (D)</p> Signup and view all the answers

<p>It depends on the number of reactant molecules (one or two). (B)</p> Signup and view all the answers

<p>Solubility equilibrium (D)</p> Signup and view all the answers

<p>The sum of all elementary steps must equal the overall balanced equation, and it must agree with the experimentally determined rate law. (C)</p> Signup and view all the answers

<p>The equilibrium constant for a solubility equilibrium (D)</p> Signup and view all the answers

<p>The rates of the forward and reverse reactions are equal, resulting in constant concentrations. (A)</p> Signup and view all the answers

<p>Higher charge typically means lower solubility due to higher energy requirements to break ionic bonds (B)</p> Signup and view all the answers

<p>Solubility is the maximum amount of solute that will dissolve at specific conditions, whereas the product constant is a fixed value for equilibrium (C)</p> Signup and view all the answers

<p>The equilibrium position lies far to the right, indicating extensive ionization. (C)</p> Signup and view all the answers

<p>The stronger the acid, the weaker its conjugate base. (D)</p> Signup and view all the answers

<p>It only partially reacts with water to produce hydroxide ions. (C)</p> Signup and view all the answers

<p>It increases the likelihood of effective collisions between reactants. (D)</p> Signup and view all the answers

<p>The transfer of a hydrogen ion from one water molecule to another. (D)</p> Signup and view all the answers

<p>By providing an alternate reaction pathway with a lower activation energy. (A)</p> Signup and view all the answers

<p>1.0 x 10^-14 (C)</p> Signup and view all the answers

<p>The equation that relates the rate of a reaction to the concentration of the reactants. (A)</p> Signup and view all the answers

<p>Ka x Kb = Kw (B)</p> Signup and view all the answers

<p>It is unique for each reaction and must be determined experimentally. (B)</p> Signup and view all the answers

<p>The hydrogen ion concentration decreases. (A)</p> Signup and view all the answers

<p>The exponent describing the relationship between initial concentration of a reactant and rate of the reaction. (C)</p> Signup and view all the answers

<p>They dissolve completely in water. (D)</p> Signup and view all the answers

<p>A step involving one-, two-, or three-entity collisions that cannot be explained in terms of simpler reactions (A)</p> Signup and view all the answers

<p>The series of elementary steps by which a chemical reaction occurs. (D)</p> Signup and view all the answers

<p>Their bonds must be broken before new bonds can be formed. (A)</p> Signup and view all the answers

<p>The rates of the forward and reverse reactions are equal, resulting in constant concentrations of the reactants and products (D)</p> Signup and view all the answers

<p>The relative concentrations of reactants and products at equilibrium (C)</p> Signup and view all the answers

<p>The rate of the forward reaction decreases as the rate of the reverse increases, until both rates are equal (D)</p> Signup and view all the answers

<p>The initial concentrations of reactants. (D)</p> Signup and view all the answers

<p>One constant is the reciprocal of the other. (C)</p> Signup and view all the answers

<p>The equilibrium position is far to the right (favors products). (D)</p> Signup and view all the answers

<p>An equilibrium where all the reactants and products are in the same state of matter. (C)</p> Signup and view all the answers

<p>K = $k_f$ / $k_r$ (A)</p> Signup and view all the answers

Reactions that require breaking existing bonds before forming new ones need more energy than reactions involving ion combination.

Complex molecules with intricate bonds have higher activation energy and are less reactive due to their stable structure.

Increasing reactant concentrations leads to more frequent collisions, increasing the likelihood of effective collisions and faster reaction rates.

Increasing surface area, like breaking up a large solid into smaller pieces, increases the chance of effective collisions, leading to faster reactions.

A catalyst speeds up a reaction by providing an alternative pathway with a lower activation energy, without changing the number of collisions or reactant energy.

A chemical rate law is an equation that relates the rate of a reaction to the concentrations of reactants at specific temperature and pressure.

The order of reaction is the exponent that represents the relationship between a reactant's concentration and the reaction rate.

An elementary step is a single step in a reaction mechanism involving one, two, or three entities, and cannot be further simplified.

The slowest step in a reaction mechanism that determines the overall rate of the reaction.

An intermediate is formed during a reaction but is not a starting reactant or final product.

Reactions involving a single reactant molecule breaking down. Usually involves collisions with the container walls.

Reactions with three reactant molecules colliding simultaneously are extremely rare.

A dynamic state in which the rates of the forward and reverse reactions are equal, leading to constant concentrations of reactants and products.

A reaction mechanism must satisfy two conditions: it should add up to the overall balanced equation, and it should agree with the experimentally determined rate law.

The rate law for an elementary step directly reflects the number of reactant molecules.

Chemical equilibrium is a dynamic state where the forward and reverse processes occur at equal rates, resulting in constant concentrations.

The relative amounts of reactants and products in a reaction at equilibrium, where the forward and reverse reaction rates are equal.

A chemical reaction that can proceed in both forward and reverse directions, resulting in a dynamic state where the rates of the forward and reverse reactions are equal.

A numerical value that defines the equilibrium position of a given reaction system, indicating the relative amounts of reactants and products at equilibrium.

The equilibrium constant is independent of the initial concentrations of reactants and products, but it does depend on the temperature.

A reaction where all reactants and products exist in the same physical state.

The equilibrium constant (K) can be used to predict the direction a reaction will shift to reach equilibrium.

A change in the conditions of a system at equilibrium, such as adding heat, removing products, or adding reactants, that causes the equilibrium to shift in a direction to relieve the stress.

The equilibrium constant (K) for a forward reaction is the reciprocal of the equilibrium constant (K') for the reverse reaction.

A change in the conditions of a system at equilibrium, such as adding heat or removing heat, that can cause the equilibrium to shift.

A measure of the partial pressure exerted by a gas in a mixture of gases, representing the pressure it would exert if it occupied the entire volume alone.

A specific set of concentrations of reactants and products at a precise moment in time.

The maximum amount of a solute that can dissolve in a given solvent at a specific temperature and pressure.

A type of chemical equilibrium where a solid ionic compound is in equilibrium with its dissolved ions in a saturated solution.

The equilibrium constant for the solubility of an ionic compound. It represents the product of the ion concentrations raised to their stoichiometric coefficients in a saturated solution.

Ionic compounds with highly charged ions (like Ca2+) tend to have lower solubility compared to those with monovalent ions (like Na+).

The maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature to form a saturated solution.

A dynamic equilibrium where the rate of dissolution of ions from a solid is equal to the rate of precipitation of ions from the solution.

The ability of a substance to act as both a proton donor (acid) and a proton acceptor (base).

A chemical entity (like water or HCO3-) that can donate a proton (H+), forming its conjugate base.

A chemical entity (like OH- or NH3) that can accept a proton (H+), forming its conjugate acid.

The equilibrium constant for the ionization of an acid in water; represents the extent of acid dissociation. Higher Ka indicates stronger acid.

The stronger the acid, the weaker its conjugate base, and vice-versa; a strong acid completely dissociates in solution, while a weak acid only partially dissociates.

The equilibrium constant for the autoionization of water (transfer of a proton from one water molecule to another), representing the concentration of H+ and OH- ions at equilibrium.

A measure of the hydrogen ion concentration in a solution, expressed on a logarithmic scale from 0 to 14 where 0 is the most acidic, 14 is the most basic, and 7 is neutral.

A device used to measure the pH of a solution by detecting the hydrogen ion concentration.