Chemistry Equilibrium Concepts
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Questions and Answers

What is defined as a dynamic system where concentrations of reactants and products do not change over time?

  • Static equilibrium
  • Physical equilibrium
  • Chemical completion
  • Dynamic equilibrium (correct)

In which type of system can equilibrium be achieved?

  • Open system
  • Isolated system
  • Any system
  • Closed system (correct)

What symbol is used to indicate the reversibility of a chemical reaction?

  • →
  • ⇌ (correct)
  • ↔
  • ↗

What happens at equilibrium in terms of the rates of reactions?

<p>The forward and reverse reaction rates are equal. (D)</p> Signup and view all the answers

Which type of system can neither exchange matter nor energy with its surroundings?

<p>Isolated system (C)</p> Signup and view all the answers

What is the significance of the equilibrium constant, K, in a chemical reaction?

<p>It describes the ratio of product to reactant concentrations at equilibrium. (D)</p> Signup and view all the answers

Which statement regarding irreversible reactions is accurate?

<p>Combustion is a typical example of irreversible reactions. (A)</p> Signup and view all the answers

What is likely to happen when the equilibrium mixture predominantly consists of products?

<p>The reaction has gone to completion, symbolized by → instead of ⇌. (D)</p> Signup and view all the answers

What is the IUPAC name for a compound containing a four-carbon chain with a hydroxyl group on the first carbon?

<p>Butanol (C), Butane-1-ol (D)</p> Signup and view all the answers

Which type of intermolecular force is predominantly present in alkanes?

<p>London Dispersion forces (C)</p> Signup and view all the answers

How does the solubility of alcohols in water change with increasing hydrocarbon chain length?

<p>Solubility decreases (B)</p> Signup and view all the answers

Which statement correctly describes hydrogen bonding in alcohols?

<p>It occurs between hydrogen atoms and electronegative elements. (A)</p> Signup and view all the answers

What is the major reason for the higher boiling point of alcohols compared to alkanes of similar sizes?

<p>Alcohols exhibit hydrogen bonding. (A)</p> Signup and view all the answers

Which of the following describes a characteristic of miscibility?

<p>Substances form a homogenous mixture. (A)</p> Signup and view all the answers

What is the name of the functional group in alcohols responsible for their properties?

<p>Hydroxyl group (C)</p> Signup and view all the answers

What happens to the hydrogen bonding between water molecules when hydrocarbon chains are present?

<p>Hydrogen bonds are broken. (A)</p> Signup and view all the answers

What is the main distinction between strong acids and weak acids based on pKa values?

<p>Strong acids have lower pKa values than weak acids. (A)</p> Signup and view all the answers

Which reaction illustrates the deprotonation of hydrofluoric acid?

<p>HF → H+ + F- (B)</p> Signup and view all the answers

What is the primary reason for the difference in reaction rates between strong and weak acids?

<p>Weak acids have a higher concentration of undissociated molecules. (A)</p> Signup and view all the answers

Which of the following correctly defines a monoprotic acid?

<p>An acid that can donate only one proton. (B)</p> Signup and view all the answers

In the reaction between NaOH and HCl, what is the product formed?

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

How many moles of HCl are produced if 10 mL of a 1 molL-1 solution completely reacts?

<p>0.01 moles (C)</p> Signup and view all the answers

Which of the following is true about polyprotic acids?

<p>They can lose multiple protons. (C)</p> Signup and view all the answers

Which reaction would be expected to occur in an experiment involving acetic acid (CH3COOH) and NaOH?

<p>CH3COOH + NaOH → CH3COONa + H2O (D)</p> Signup and view all the answers

Which elimination mechanism will primary alcohols primarily follow?

<p>E2 pathway (D)</p> Signup and view all the answers

What type of carbocation do tertiary alcohols form during elimination reactions?

<p>Heavily stabilized carbocation (C)</p> Signup and view all the answers

What effect do polar protic solvents have on carbocations in elimination reactions?

<p>They stabilize carbocations (B)</p> Signup and view all the answers

How are secondary alcohols categorized in terms of carbon attachments?

<p>Attached to two other carbon atoms (A)</p> Signup and view all the answers

What is the general formula for alcohols?

<p>CnH2n+1OH (D)</p> Signup and view all the answers

What is the name of the reaction that forms an alkene from an alcohol?

<p>Dehydration reaction (C)</p> Signup and view all the answers

When two -OH groups are present in a molecule, what is it called?

<p>Diol (C)</p> Signup and view all the answers

Which elimination pathway do secondary alcohols typically follow?

<p>E1 pathway (D)</p> Signup and view all the answers

What is meant by dynamic equilibrium in a reversible reaction?

<p>The rates of the forward and reverse reactions are equal, resulting in no net change. (D)</p> Signup and view all the answers

What happens to the concentration of bromine gas when bromine liquid is placed in a sealed container?

<p>It increases over time until dynamic equilibrium is reached. (D)</p> Signup and view all the answers

Why is a closed system necessary for establishing dynamic equilibrium?

<p>To prevent the loss of reactants and products from the system. (D)</p> Signup and view all the answers

At equilibrium, what is the change in concentration of bromine gas and bromine liquid?

<p>Both concentrations remain at a constant value. (D)</p> Signup and view all the answers

Which of the following describes the process that occurs when bromine vapor molecules collide with the liquid surface?

<p>Condensation occurs as vapor molecules lose energy. (B)</p> Signup and view all the answers

What will happen if the bromine system is opened to the environment?

<p>Bromine gas will escape and prevent equilibrium from forming. (B)</p> Signup and view all the answers

In a reversible reaction, what does the equation 'rate FORWARD = rate REVERSE' signify?

<p>The system is at a state where both reactions are occurring at equal amounts. (D)</p> Signup and view all the answers

How does the concentration of bromine gas affect the rate of condensation?

<p>An increase in concentration leads to a higher rate of condensation. (A)</p> Signup and view all the answers

How many moles of NaOH are in 10.00 cm3 of 0.01 M NaOH?

<p>0.001 moles (D)</p> Signup and view all the answers

What is the balanced reaction between H2SO4 and NaOH?

<p>H2SO4 + 2 NaOH → Na2SO4 + 2 H2O (A)</p> Signup and view all the answers

What information can we deduce from the equivalence point in a strong acid-weak base titration?

<p>All hydronium ions have been neutralized. (C)</p> Signup and view all the answers

What is the significance of the half-equivalence point in a weak acid-strong base titration?

<p>It indicates that an equal amount of acid and base has reacted. (B)</p> Signup and view all the answers

Why is the pH at the equivalence point in a titration of a strong acid with a weak base not equal to 7?

<p>It is lower than 7 because the resulting solution contains a weak acid. (D)</p> Signup and view all the answers

How is the concentration of H2SO4 determined from the titration with NaOH?

<p>It is calculated by rearranging the formula Concentration = Moles / Volume. (D)</p> Signup and view all the answers

Which statement best describes NH3 as a titrant in a strong acid-weak base titration?

<p>NH3 gradually increases the pH as it reacts with H3O+ ions. (C)</p> Signup and view all the answers

In a titration involving propanoic acid and KOH, what indicates that the equivalence point has been reached?

<p>A sudden color change in the indicator. (A)</p> Signup and view all the answers

Flashcards

Reversible Reaction

A chemical reaction where the products can react to form the original reactants, and both forward and reverse reactions occur simultaneously.

Equilibrium

A state where the rates of the forward and reverse reactions are equal, and there is no further change in the concentrations of reactants and products.

Equilibrium Constant (K)

The equilibrium constant is a number that represents the ratio of products to reactants at equilibrium, at a specific temperature. It indicates the extent to which a reaction proceeds to completion.

Closed System

A system where only energy can pass through its boundaries, but matter cannot.

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Open System

A system where both energy and matter can pass through its boundaries.

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Isolated System

A system where neither energy nor matter can pass through its boundaries.

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Kinetics

The study of the rate of a reaction and the factors affecting its speed.

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Thermodynamics

The study of the energy changes associated with a reaction, including the relative stability of reactants and products.

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Dynamic Equilibrium

A state in a closed system where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.

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Volatile Liquid

A liquid that readily evaporates, easily transitioning into the gaseous phase.

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Evaporation

The conversion of a substance from a liquid to a gas.

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Condensation

The conversion of a substance from a gas to a liquid.

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Reaction Rate

The rate of a chemical reaction determines how quickly reactants are converted into products.

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Deprotonation

A chemical reaction where an acid loses a proton (H+).

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Protonation

A reaction where a species donates a proton (H+) to a base. The base then becomes protonated.

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pKa

A measure of the acidity of a solution. The lower the pKa, the stronger the acid. Strong acids have a pKa less than 0.

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Strong Acid

An acid that readily donates protons (H+) in solution. They have a low pKa.

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Weak Acid

An acid that partially donates protons (H+) in solution. They have a higher pKa than strong acids.

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Deprotonation

The reverse of protonation. A base loses a lone pair and becomes protonated by accepting a proton (H+).

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pKb

A measure of the basicity of a solution. The lower the pKb, the stronger the base.

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Polyprotic Acid

An acid that can donate multiple protons (H+) per molecule. These can be diprotic (two protons) or triprotic (three protons) acids.

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Equivalence Point

The point in a titration where the moles of titrant added are exactly equal to the moles of analyte present in the solution. At this point, the reaction between the titrant and analyte is complete. The pH at the equivalence point depends on the strength of the acid and base involved.

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Titrant

A solution of known concentration used to determine the concentration of an unknown solution.

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Analyte

The substance being analyzed in a titration. It is the solution whose concentration is being determined.

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Equivalence Point Ratio

The ratio of the moles of the titrant to the moles of the analyte at the equivalence point. It indicates the stoichiometry of the reaction.

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Strong Acid - Weak Base Titration

A titration where a strong acid reacts with a weak base. The equivalence point of this titration will have a pH less than 7.

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Weak Acid - Strong Base Titration

A titration where a weak acid reacts with a strong base. The equivalence point of this titration will have a pH greater than 7.

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Half-Equivalence Point

The point in a weak acid - strong base titration where half of the weak acid has been neutralized by the strong base. The pH at this point is equal to the pKa of the weak acid.

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Primary Alcohol

Alcohols where the carbon atom attached to the -OH group is directly bonded to only one other carbon atom.

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Secondary Alcohol

Alcohols where the carbon atom attached to the -OH group is directly bonded to two other carbon atoms.

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Tertiary Alcohol

Alcohols where the carbon atom attached to the -OH group is directly bonded to three other carbon atoms.

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Alcohol Dehydration

The process of removing a water molecule (H2O) from an alcohol molecule, resulting in the formation of an alkene.

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Intermolecular Dehydration

The reaction where water molecules are removed from two alcohol molecules, resulting in the formation of an ether.

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Intramolecular Dehydration

The reaction where a water molecule is removed from within the same alcohol molecule, resulting in the formation of an alkene.

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Hydrogen Bonding

A type of intermolecular force that occurs between molecules containing hydrogen atoms bonded to highly electronegative atoms like oxygen (O), fluorine (F), or nitrogen (N).

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Hydrogen bonding in alcohols

Alcohols contain hydroxyl groups (OH) which can participate in hydrogen bonding, leading to stronger intermolecular forces compared to alkanes.

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Miscible

The ability of a substance to dissolve completely in another substance, forming a homogenous mixture.

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Solubility of alcohols

Small alcohol molecules are miscible with water due to the formation of hydrogen bonds between the alcohol's OH group and water molecules.

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Solubility decrease with chain length

As the hydrocarbon chain in an alcohol increases, solubility in water decreases due to the increased non-polar nature of the hydrocarbon chain.

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Hydrocarbon chain effect on solubility

The presence of a long hydrocarbon chain in an alcohol molecule disrupts the hydrogen bonding network between water molecules, leading to a decrease in solubility.

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Hydrogen bonding in alcohol-water mixture

The OH group of an alcohol can form new hydrogen bonds with water molecules, but the hydrocarbon chain cannot.

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Study Notes

Summary of General Chemistry Concepts

  • Chemistry is the study of matter and its properties, along with the changes it undergoes.
  • Matter is anything that has mass and occupies space.
  • Atoms are the fundamental building blocks of matter.
  • Elements are substances composed of only one type of atom.
  • Compounds are substances composed of two or more different types of atoms chemically bonded.
  • Molecules are groups of two or more atoms held together by chemical bonds.
  • Chemical reactions involve the rearrangement of atoms to form new substances.
  • Chemical equations represent chemical reactions using chemical formulas and coefficients to balance the atoms on both sides of the equation.
  • States of matter include solid, liquid, and gas.
  • Physical properties describe the characteristics of a substance without changing its chemical composition (e.g., melting point, boiling point).
  • Chemical properties describe the characteristics of a substance that involve a change in chemical composition or the ability of a substance to undergo a chemical reaction (e.g., flammability, reactivity).

Summary of Thermodynamics

  • Thermodynamics is the study of energy and its transformations in chemical and physical processes.
  • System refers to the specific part of the universe under investigation.
  • Surroundings include everything outside of the system.
  • Open system: can exchange both matter and energy with the surroundings.
  • Closed system: can exchange energy but not matter with the surroundings.
  • Isolated system: cannot exchange either matter or energy with the surroundings.
  • Energy is the capacity to do work or transfer heat.
  • Internal energy is the total energy of a system.
  • Heat is the transfer of thermal energy between two objects at different temperatures.
  • Work is a transfer of energy occurring when a force moves an object through a displacement.

Summary of Equilibrium

  • Equilibrium is a state where opposing changes or processes occur at the same rate, leading to a constant net change in the concentration of reactants and products.
  • Equilibrium can only be achieved in a closed system.
  • The Equilibrium Constant (Kc) provides information about the composition of an equilibrium mixture at a particular temperature.
  • The magnitude of Kc indicates the extent of a reaction.
  • A large Kc indicates that the equilibrium position is overwhelmingly in favor of the products.
  • A smaller Kc indicates a position of equilibrium is more in favor of the reactants.
  • Kc is unitless and depends on temperature.
  • Rates of forward and reverse reactions are equal at equilibrium.
  • Equilibrium is a dynamic state, meaning that the forward and reverse reactions still occur, but their relative rates are equal.
  • Activities are used to account for differences in behavior between ideal and real solutions.

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Lesson 7.1.1a Reversible Reactions PDF

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Test your knowledge on chemical equilibrium concepts with this quiz. Explore dynamic systems, the significance of the equilibrium constant, and intermolecular forces. This quiz covers essential topics related to chemistry and the behavior of reactions at equilibrium.

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