Lecture 1 Notes on Chemical Equations
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Questions and Answers

What is produced when hydrogen reacts with oxygen?

  • Ozone
  • Nitrogen
  • Hydrogen Peroxide
  • Water (correct)

The stoichiometric factor in a reaction is defined as the ratio of the number of moles of reactants to the number of moles of products.

True (A)

What is the molar ratio of nitrogen to hydrogen in the reaction N2(g) + 3 H2(g) → 2 NH3(g)?

1:3

The molar mass of 2AL is _____ g/mol.

<p>53.94</p> Signup and view all the answers

Match the following compounds with their chemical formulas:

<p>Water = H2O Aluminum oxide = Al2O3 Nitrogen = N2 Hydrogen = H2</p> Signup and view all the answers

In the reaction 2Al + 3O2(g) → 2Al2O3, what is the stoichiometric coefficient for oxygen?

<p>3 (A)</p> Signup and view all the answers

Which condition makes a reaction irreversible?

<p>If reactants are consumed completely (C)</p> Signup and view all the answers

The reaction 2H2 + O2 → 2H2O is an example of a decomposition reaction.

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

A higher value of P is associated with Kszic being smaller than Kaso.

<p>True (A)</p> Signup and view all the answers

What does the stoichiometric coefficient represent in a reaction?

<p>The ratio of moles of reactants and products involved in the reaction.</p> Signup and view all the answers

What type of reaction is represented by the equation N2(g) + 3 H2(g) → 2 NH3(g)?

<p>Synthesis reaction</p> Signup and view all the answers

For any chemical species involved in a reaction, their consumption impacts the __________ of that species.

<p>equilibrium</p> Signup and view all the answers

Match the following concepts with their definitions:

<p>Irreversible Reaction = Reactants are consumed completely Kszic = Equilibrium constant at reduced pressure Kaso = Equilibrium constant at standard pressure Stoichiometry = Quantitative relationships in reactants and products</p> Signup and view all the answers

What is the primary effect of consuming reactants in a chemical reaction?

<p>It shifts the equilibrium position. (C)</p> Signup and view all the answers

P is considered greater than Kszic under all conditions.

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

What occurs to reactants in an irreversible reaction?

<p>They are consumed completely without returning to their original state.</p> Signup and view all the answers

What does the equilibrium constant (K) signify in a chemical reaction?

<p>The ratio of the concentration of products to reactants at equilibrium (D)</p> Signup and view all the answers

A large equilibrium constant (K) indicates that the products are favored at equilibrium.

<p>True (A)</p> Signup and view all the answers

What is represented by the letter 'a' in the law of mass action equation?

<p>Coefficient of reactant A</p> Signup and view all the answers

In the law of mass action: aA + bB ⇌ cC, the value of K can be expressed as __________.

<p>K = [C]^c / ([A]^a * [B]^b)</p> Signup and view all the answers

Match the following terms with their definitions:

<p>K = Equilibrium constant a, b, c = Stoichiometric coefficients Reactants = Substances consumed in a reaction Products = Substances formed in a reaction</p> Signup and view all the answers

What does a small equilibrium constant (K) suggest about the reaction?

<p>The reactants are favored over products (B)</p> Signup and view all the answers

In the expression for K, larger values of 'a' or 'b' increase the overall value of K.

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

In the law of mass action, what does the term 'intermediate' refer to?

<p>A species that is formed and consumed in the reaction pathway</p> Signup and view all the answers

What is primarily used to determine the rate at which a drug is removed from the body?

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

Most drugs follow zero-order elimination kinetics.

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

What is the formula for the elimination rate constant?

<p>Ke = In(2)/t1/2</p> Signup and view all the answers

The principle that describes the decrease in the concentration of a drug over time is called __________ kinetics.

<p>elimination</p> Signup and view all the answers

Match the following terms with their correct descriptions:

<p>First-order kinetics = Rate of elimination depends on drug concentration Elimination rate constant = Formula representing decay of drug concentration Half-life = Time taken for drug concentration to reduce by half Pharmacokinetics = Study of drug absorption, distribution, metabolism, and excretion</p> Signup and view all the answers

What does the rate constant (K) depend on?

<p>Temperature (A)</p> Signup and view all the answers

Rate laws are typically known before conducting experiments.

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

What is the sum of the exponents of the concentrations in a rate law called?

<p>reaction order</p> Signup and view all the answers

In a first-order reaction, the rate can be expressed as t = -k[A]. The reaction order is ____.

<p>1</p> Signup and view all the answers

Match the following reaction orders with their correct rate law equation:

<p>First-order = t = -k[A] Second-order = t = -1/k[A] + 1/B Third-order = Rate = -k[A][B] Zero-order = Rate = k</p> Signup and view all the answers

Which of the following best describes molecularity?

<p>Number of reactant molecules participating in a reaction (B)</p> Signup and view all the answers

The order of the reaction can be associated with elemental complexities.

<p>True (A)</p> Signup and view all the answers

What is the theoretical value of mols in a reaction referred to as?

<p>molecularity</p> Signup and view all the answers

For elementary reactions, molecularity is always a ____ number.

<p>whole</p> Signup and view all the answers

In which kind of reaction does the reaction order equal the sum of the exponents of the reactant concentrations?

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

What does the symbol K represent in the given content?

<p>Rate constant (A)</p> Signup and view all the answers

The half-life of a first-order reaction depends on the concentration of reactants.

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

What is the equation for the half-life of a first-order reaction?

<p>t(1/2) = 0.693/K</p> Signup and view all the answers

For a first-order reaction, the natural logarithm of the ratio of concentrations is equal to the negative product of the rate constant and time: ______

<p>In([A]t/[A]o) = -Kt.</p> Signup and view all the answers

Match the following terms to their descriptions:

<p>K = Rate constant of a reaction t(1/2) = Time required for half of the reactant to be consumed [A]o = Initial concentration of reactant A [A]t = Concentration of reactant A at time t</p> Signup and view all the answers

Which of the following equations represents a first-order reaction?

<p>[A]t = [A]oe^{-kt} (A)</p> Signup and view all the answers

The natural logarithm of the ratio of concentrations decreases as time increases for a first-order reaction.

<p>True (A)</p> Signup and view all the answers

What is indicated by the symbol [A]t?

<p>Concentration of reactant A at time t</p> Signup and view all the answers

The first-order rate equation can be expressed as [A]t = [A]o e^{-kt}. This shows that concentration [A] decreases ___ with time.

<p>exponentially</p> Signup and view all the answers

How do first-order reactions differ from zero-order reactions in terms of rate dependence?

<p>First-order reactions depend on the concentration of reactants (D)</p> Signup and view all the answers

Flashcards

Irreversible Reaction

A chemical reaction that proceeds completely in one direction, meaning all reactants are consumed and no reverse reaction occurs.

Undef Q

The state where a reaction is not at equilibrium and one direction is favored.

Reversible Reaction

A chemical reaction that can proceed in both the forward and reverse directions, with reactants and products present in equilibrium.

Equilibrium Constant (K)

The ratio of products to reactants at equilibrium.

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Reaction Quotient (Q)

The ratio of products to reactants under non-equilibrium conditions.

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Kf

The rate constant for the forward reaction.

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Kr

The rate constant for the reverse reaction.

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Stoichiometric Coefficient (ν)

The stoichiometric coefficient of a particular species in a chemical reaction, representing the number of moles of that species involved in the reaction.

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Law of Mass Action

Describes the relationship between the concentrations of reactants and products at equilibrium in a reversible chemical reaction.

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Product-Favored Reaction

A reversible reaction that favors the formation of products at equilibrium.

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Reactant-Favored Reaction

A reversible reaction that favors the formation of reactants at equilibrium.

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Large Equilibrium Constant (K)

The equilibrium constant is very large, indicating a strong preference for product formation. The reaction essentially goes to completion.

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Small Equilibrium Constant (K)

The equilibrium constant is very small, indicating a strong preference for reactant formation. The reaction hardly proceeds to completion.

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Intermediate Equilibrium Constant (K)

The presence of significant amounts of both reactants and products at equilibrium. The reaction doesn't go to completion.

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Negligible Amount

The concentration of a substance at equilibrium is so small that it's practically negligible. The reaction goes to completion.

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Balanced Chemical Equation

Shows the chemical equation with the reactants and products, balanced with stoichiometric coefficients to ensure that mass is conserved. Each coefficient indicates the number of moles of each substance involved in the reaction.

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Stoichiometric Coefficient

The numerical coefficient in front of a chemical formula in a balanced chemical equation. They represent the relative number of moles of each reactant and product involved in the reaction.

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Molar Ratio

The ratio of the moles of one substance to the moles of another substance in a balanced chemical equation.

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Mole Fraction

The ratio of the number of moles of a substance to the total number of moles of all substances in a chemical reaction.

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Stoichiometry

Quantitative relationships between reactants and products in a chemical reaction. It helps predict the amounts of reactants and products involved in a chemical reaction.

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Limiting Reactant

A substance that is completely consumed in a chemical reaction and limits the amount of product that can be formed.

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Theoretical Yield

The maximum amount of product that can be formed in a chemical reaction, assuming complete consumption of the limiting reactant.

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Actual Yield

The actual amount of product obtained in a chemical reaction, which is often less than the theoretical yield due to factors like incomplete reactions or loss of product.

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Rate Constant (k)

A constant that represents the rate of reaction at a specific temperature. It does not depend on the concentration of reactants.

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Rate of Reaction

The rate of a chemical reaction is measured as the change in concentration of a reactant or product over time. It is usually expressed in units of M/s (moles per second).

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Molecularity

The total number of reactant molecules that participate in the elementary step of a reaction. It represents the molecularity of the reaction.

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Order of Reaction

The sum of the exponents of the concentration terms in the rate law. It determines how the rate changes with the change in concentration of reactants.

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Rate Law

A mathematical expression that relates the rate of a reaction to the concentration of reactants. It determines how the reaction rate changes with the change in concentration of reactants.

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What is pharmacokinetics?

Pharmacokinetics is the study of how drugs move through the body. It helps us understand how a drug is absorbed, distributed, metabolized, and eliminated.

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What is first-order elimination?

First-order elimination describes how the body removes a drug at a rate proportional to the amount of drug present. This means a constant fraction of the drug is eliminated per unit time.

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What is the elimination rate constant (Ke)?

The elimination rate constant (Ke) determines how quickly a drug is eliminated from the body. It is calculated by dividing the natural logarithm of the drug concentration at two time points by the time difference.

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How are most drugs eliminated?

Most drugs are eliminated from the body through first-order kinetics, meaning the rate of elimination is directly proportional to the drug concentration.

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Why is the elimination rate constant (Ke) important?

The elimination rate constant (Ke) is crucial for determining dosage regimens and monitoring drug levels in a patient's body.

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Half-life (t1/2)

The time required for the concentration of a reactant to decrease to half its initial value in a first-order reaction.

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First-Order Reaction Rate Constant (k)

The rate constant for a first-order reaction is the same as the half-life divided by the natural logarithm of 2.

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Half-life Independence

The half-life of a first-order reaction is independent of the initial concentration of the reactant.

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Integrated Rate Law for First-Order Reactions

The natural logarithm of the concentration of a reactant at any time minus the natural logarithm of the initial concentration is equal to the negative of the rate constant multiplied by time.

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Equilibrium Time

The time required for a reaction to reach equilibrium, where the rates of the forward and reverse reactions are equal.

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First-Order Reaction Plot

A graphical representation of the relationship between the concentration of a reactant and time for a first-order reaction.

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Equilibrium

The condition where the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

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Study Notes

Lecture 1 Notes on Equations

  • Chemicals can change structure but keep the same formula (A → B)
  • ATP hydrolysis: A + B → C + D
  • Myoglobin → oxymyoglobin (atom change)
  • Unfolded → folded protein (A → B)
  • Reaction rate = Rate of change of concentration over time
  • Reactants need to collide to react; concentration needs to be high
  • Elementary reactions are single-step
  • Transition state: short-lived, unstable, single bond vibration
  • Intermediate: product in one elementary reaction, reactant in the next
  • Molecularity: number of molecules taking part in a reaction
  • Unimolecular (1), Bimolecular (2) etc.
  • Chemical equilibrium: no net change in concentrations of reactants and products
  • Law of mass action (aA + bB → cC + dD): k = [C]c[D]d / ([A]a[B]b)
  • k = equilibrium constant
  • Small k (k ≈ 10-3) mostly reactants
  • Intermediate k (k ≈ 10-3 to 103) both reactants and products
  • Large k (k ≈ 103) mostly products

Lecture 2 Notes on Pictures and Equations

  • Reaction mechanisms need experimental determination
  • Reaction intermediate
  • Balancing chemical equations: Determine the stoichiometric coefficients
  • Balancing reaction example: C7H16(â„“) + 11 O2(g) → 7CO2(g) + 8H2O(g)

Lecture 3 Notes on Pictures and Equations

  • Reaction mechanisms need experimental determination
  • The reaction quotient. can be used to determine direction
  • If Q < K, reaction goes to the right, if Q > K, reaction goes to the left
  • Balancing reactions like Mg(NO3)2 + 2Li → Mg + 2LiNO3

Lecture 4 Notes on Pictures, Equations, and Examples

  • Bimolecular reactions often occur in second order, nucleophilic substitutions, and example reactions
  • Reaction order often corresponds to the number of reactant species contributing to a given velocity
  • Example: N2O4(g) → 2NO2(g) is bimolecular
  • Example: 2NOCl(g) → 2NO(g) + Cl2(g) is bimolecular

Lecture 5 Notes

  • Accumulation = input - output
  • if input and output are different, could mean
  • Some other waste product
  • Consumption / accumulation
  • Leak
  • Equipment failure
  • Reaction rate
  • Half-life of a zero-order reaction and first-order reaction, integrated rate law for zeroth order

Lecture 6 Notes

  • The order of a reaction relates to the number of reactant species contributing to its rate
  • Graphing different order reactions and calculating K
  • Unimolecular, bimolecular, and termolecular reactions
  • Rate Laws and rate constants
  • Units of rate constant depend on the rate law

Lecture 7 Notes

  • Pharmacokinetics case studies
  • Reaction order is crucial in pharmacokinetics to understand how a drug moves through the body
  • Calculating half-lives for zeroth and first-order reactions

Additional Notes

  • Examples of equations, drawings and examples for each lecture shown on the images provided
  • Other notable mentions of calculations and equations provided in the notes

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