Chemistry Chapter 5 Flashcards
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Questions and Answers

Reactants and products in a chemical equation are arranged how?

  • Reactants on the left, products on the right (correct)
  • Reactants and products are mixed
  • Reactants on the right, products on the left
  • There is no specific arrangement

    • What type of reaction does calcium carbonate undergo when heated strongly?

    Decomposition

    What is a limiting reactant?

    The substance that is depleted first and stops a reaction

    What are the coefficients that properly balance the equation NaOH + H2S --> Na2S + H2O?

    <p>2, 1, 1, 2</p> Signup and view all the answers

    What type of reaction is represented by CaCO3 --> CaO + CO2?

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

    What is the mole ratio to convert from KO2 to oxygen in the equation KO2 + H2O --> KOH + O2?

    <p>3 mol O2 / 4 mol KO2</p> Signup and view all the answers

    How many moles of S8 can be produced from 0.250 mole of SO2 in the reaction 16H2S + 8SO2 --> 16H2O + 3S8?

    <p>0.0938 mole</p> Signup and view all the answers

    What is the percent yield for the combustion of ethanol given 75.0 g C2H5OH reacted with 105 g O2 and produced 65.0 g CO2?

    <p>67.5%</p> Signup and view all the answers

    If 10.0 moles of potassium react, how many moles of bromine are required according to 2K + Br2 --> 2KBr?

    <p>5.00</p> Signup and view all the answers

    Which reactant is the limiting reactant when 2.00 grams of potassium react with 2.00 grams of bromine in 2K + Br2 --> 2KBr?

    <p>Br2</p> Signup and view all the answers

    What mass of potassium chloride can be produced from 5.2 g of potassium and 7.9 g of chlorine in 2K + Cl2 --> 2KCl?

    <p>9.9 g KCl</p> Signup and view all the answers

    [Blank] lower the [Blank] of a reaction and therefore increase the reaction rate.

    <p>Catalysts, activation energy</p> Signup and view all the answers

    What is a synthesis reaction?

    <p>2 or more elements or compounds combine to form one or more complex compounds A + B --&gt; AB</p> Signup and view all the answers

    What occurs in a decomposition reaction?

    <p>Breakdown of one compound to form elements or simpler compounds AB --&gt; A + B</p> Signup and view all the answers

    What characterizes a single replacement reaction?

    <p>One element trades places with a different element A + BC --&gt; AC + B</p> Signup and view all the answers

    What characterizes a double replacement reaction?

    <p>One element trades places with a different element in a compound AB + CD --&gt; AD + CB</p> Signup and view all the answers

    What is reduction in a chemical reaction?

    <p>Gain of one or more electrons</p> Signup and view all the answers

    What is oxidation?

    <p>Loss of one or more electrons</p> Signup and view all the answers

    What are redox reactions?

    <p>Involves transfer of electrons, oxidation and reduction ALWAYS occur together</p> Signup and view all the answers

    What is the oxidizing agent?

    <p>The thing that is reduced is the oxidizing agent</p> Signup and view all the answers

    What are reducing agents?

    <p>The thing that is oxidized is the reducing agent</p> Signup and view all the answers

    What is stoichiometry?

    <p>Study of moles and mass relationships in a chemical reaction; coefficients refer to the number of moles of the compound</p> Signup and view all the answers

    How many moles of Cl2 are required to produce 9.6 moles of PCl3 in the reaction P4 + 6Cl2 --> 4PCl3?

    <p>14.4 moles</p> Signup and view all the answers

    If excess H2O is present, what masses of NH3 and CO2 are produced from 0.92 moles of urea?

    <p>31.4 grams</p> Signup and view all the answers

    How many grams of NaCl will be produced by 6.5 grams of NaHCO3 in the reaction NaHCO3 + HCl --> NaCl + H2O + CO2?

    <p>4.5 g NaCl</p> Signup and view all the answers

    What is a limiting reagent?

    <p>The reagent used up first in a chemical reaction</p> Signup and view all the answers

    What are excess reagents?

    <p>Total reactant - reactant used = excess reactant</p> Signup and view all the answers

    What is theoretical yield?

    <p>The maximum amount of product that can be obtained</p> Signup and view all the answers

    Percent yield is the same as actual yield.

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

    What is actual yield?

    <p>Amount of product obtained from a reaction</p> Signup and view all the answers

    What is free energy in a reaction?

    <p>Energy released or gained in a reaction; sum of energy of bonds broken and bonds made</p> Signup and view all the answers

    What are spontaneous reactions?

    <p>Negative value, energy is released, continue by themselves once it has started</p> Signup and view all the answers

    What are nonspontaneous reactions?

    <p>Will not take place unless something starts them and keeps them going; positive value, energy consumed</p> Signup and view all the answers

    What defines an exothermic reaction?

    <p>Combustion reaction releases energy in the form of heat</p> Signup and view all the answers

    What defines an endothermic reaction?

    <p>Energy is added to the system for the reaction to occur</p> Signup and view all the answers

    What happens to reaction rate if you lower the activation energy?

    <p>Reaction rate is increased</p> Signup and view all the answers

    What happens when you add a catalyst to a reaction?

    <p>Lowers the activation energy</p> Signup and view all the answers

    Study Notes

    Chemical Reactions

    • Reactants and Products: Reactants are positioned on the left, products on the right of a chemical equation.
    • Decomposition Reaction: Calcium carbonate (CaCO3) decomposes when heated to form calcium oxide (CaO) and carbon dioxide (CO2).
    • Limiting Reactant: The limiting reactant is the substance that is consumed first, halting the reaction.

    Balancing Chemical Equations

    • Balanced Equation Coefficients: For the equation NaOH + H2S → Na2S + H2O, the coefficients are 2, 1, 1, and 2, respectively.
    • Mole Ratios: When balancing KO2 + H2O → KOH + O2, the mole ratio of O2 to KO2 is 3 mol O2/4 mol KO2.

    Mole Calculations

    • Sulfur Production: From the reaction 16H2S + 8SO2 → 16H2O + 3S8, 0.250 mole of SO2 produces 0.0938 mole of S8.
    • Percent Yield of Ethanol Combustion: The combustion of 75.0 g of ethanol gives a percent yield of 67.5% for the production of CO2.
    • Moles of Reactants: In the reaction 2K + Br2 → 2KBr, 10.0 moles of potassium require 5.00 moles of bromine.
    • Limiting Reactant in a Potassium and Bromine Reaction: In the reaction of 2.00 grams each of potassium and bromine, bromine (Br2) is the limiting reactant.
    • Mass Calculation of Potassium Chloride: From 5.2 g of potassium and 7.9 g of chlorine, 9.9 g of potassium chloride (KCl) can be produced.

    Reaction Types

    • Catalysts: Catalysts lower the activation energy, enhancing the reaction rate.
    • Synthesis Reaction: Involves combining multiple elements or compounds to form one complex product (A + B → AB).
    • Decomposition Reaction: A single compound breaks down into simpler substances (AB → A + B).
    • Single Replacement Reaction: One element replaces another in a compound (A + BC → AC + B).
    • Double Replacement Reaction: Elements in two compounds exchange partners (AB + CD → AD + CB).

    Redox Reactions

    • Reduction: The gain of electrons during a reaction.
    • Oxidation: The loss of electrons during a reaction.
    • Redox Reactions: These always involve both oxidation and reduction processes and electron transfer.

    Stoichiometry

    • Stoichiometry: The study of relationships between moles and mass in chemical reactions; coefficients signify the number of moles.
    • Limiting and Excess Reagents: The limiting reagent is consumed first, while excess reagents are leftover reactants after the reaction.
    • Theoretical Yield: The highest possible quantity of product produced from a given amount of reactants.

    Yield and Free Energy

    • Actual Yield: The real amount of product obtained from a chemical reaction.
    • Free Energy: Energy gained or released in a reaction based on bond breaking and formation.
    • Spontaneous Reactions: Occur without ongoing input of energy and have a negative free energy value.
    • Nonspontaneous Reactions: Require energy input to proceed and have a positive free energy value.

    Reaction Dynamics

    • Exothermic Reactions: Release heat energy, common in combustion processes.
    • Endothermic Reactions: Absorb energy to proceed, requiring external energy input.
    • Reaction Rate: The speed at which products form in a reaction.
    • Activation Energy (Eact): The barrier energy necessary to transition from reactants to products; reducing the activation energy increases the reaction rate.
    • Factors Affecting Reaction Rate: Changing temperature, concentration, or adding a catalyst can alter the speed of a reaction.

    Key Outcomes

    • Lowering Activation Energy: Increases reaction rate, facilitating faster product formation.
    • Adding Catalysts: Permanently lowers activation energy and accelerates reactions without being consumed.

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    Test your knowledge of key concepts from Chemistry Chapter 5 with these flashcards. Each card provides definitions and examples related to chemical equations, reactants, products, and reaction types. Perfect for mastering the foundational elements of chemical reactions.

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