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

    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</p> Signup and view all the answers

    Which condition makes a reaction irreversible?

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

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

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

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

    <p>True</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.</p> Signup and view all the answers

    P is considered greater than Kszic under all conditions.

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

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

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

    Most drugs follow zero-order elimination kinetics.

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

    Rate laws are typically known before conducting experiments.

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

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

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

    What does the symbol K represent in the given content?

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

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

    <p>False</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}</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</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</p> Signup and view all the answers

    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(ℓ) + 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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    Explore the fundamentals of chemical equations and reaction dynamics in this quiz. Topics include ATP hydrolysis, reaction rates, and the concept of chemical equilibrium. Test your understanding of elementary reactions, molecularity, and the law of mass action.

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