Chemistry Final Flashcards: Formulas & Equations
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Questions and Answers

What is stoichiometry?

  • A method for measuring temperature
  • A type of pressure measurement
  • A type of gas law
  • Brand of chemistry dealing with mass relationships (correct)

    • What is the percent yield formula?

    % yield = actual yield/theoretical yield x 100

    What is the formula for pressure?

    Pressure = force/unit area

    What are the standard temperature and pressure values in degrees Celsius and Kelvin?

    <p>0°C, 273 K</p> Signup and view all the answers

    How many particles are in 1 mole?

    <p>6.02 x 10^23</p> Signup and view all the answers

    How many liters does 1 mole occupy at STP?

    <p>22.4 L</p> Signup and view all the answers

    What is the order for converting from grams, liters, and moles?

    <p>Liters &gt; Moles &gt; Grams</p> Signup and view all the answers

    How many milliliters are in 1 liter?

    <p>1,000</p> Signup and view all the answers

    What does Graham's Law state about the rates of effusion/diffusion of gases?

    <p>Rate A/Rate B = √MMB/√MMA</p> Signup and view all the answers

    The rate of a gas varies directly with its mass.

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

    What are the steps in a heating curve?

    <p>solid, melting, liquid, boiling, gas</p> Signup and view all the answers

    What are the steps in a cooling curve?

    <p>gas, condensation, liquid, freezing, solid</p> Signup and view all the answers

    At sea level, at what temperature does water boil?

    <p>100°C</p> Signup and view all the answers

    If atmospheric pressure is low, it is harder for liquids to escape into gas.

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

    As matter goes from a more ordered state to a less ordered state, what type of reaction is it?

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

    As matter goes from a less ordered state to a more ordered state, what type of reaction is it?

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

    In an open system, what happens to water?

    <p>It evaporates.</p> Signup and view all the answers

    What is equilibrium in chemistry?

    <p>A dynamic condition with equal rates of opposing changes.</p> Signup and view all the answers

    What refers to the transition from solid to liquid?

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

    What refers to the transition from solid to gas?

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

    What refers to the transition from liquid to solid?

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

    What refers to the transition from liquid to gas?

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

    What refers to the transition from gas to liquid?

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

    What refers to the transition from gas to solid?

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

    What is a triple point?

    <p>Conditions where solid, liquid, and gas coexist at equilibrium.</p> Signup and view all the answers

    What is a critical point?

    <p>Temperature and pressure where the substance cannot exist in liquid state.</p> Signup and view all the answers

    What is a strong electrolyte?

    <p>All of the dissolved compound exist as ions.</p> Signup and view all the answers

    What is a weak electrolyte?

    <p>Conducts electricity poorly due to a fraction existing as ions.</p> Signup and view all the answers

    What is a non-electrolyte?

    <p>Does not yield ions and therefore cannot conduct electricity.</p> Signup and view all the answers

    What is the ionization constant for water?

    <p>1 x 10^-14</p> Signup and view all the answers

    How do you calculate the pH?

    <p>-log[H+]</p> Signup and view all the answers

    What characterizes a strong acid?

    <p>Low pH; almost completely dissociates.</p> Signup and view all the answers

    What characterizes a weak acid?

    <p>Higher pH; does not completely dissociate.</p> Signup and view all the answers

    What is enthalpy?

    <p>Heat of a reaction where Q=cm∇T.</p> Signup and view all the answers

    What does entropy represent?

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

    What does a negative change in Gibbs free energy (-∇G) indicate?

    <p>Spontaneous reaction.</p> Signup and view all the answers

    What does a positive change in Gibbs free energy (+∇G) indicate?

    <p>Not spontaneous reaction.</p> Signup and view all the answers

    Solids have high entropy.

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

    Gases have low entropy.

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

    What five factors speed up a chemical reaction?

    <p>Temperature; concentration; catalyst; surface area; nature of the reaction.</p> Signup and view all the answers

    How does temperature increase affect reactions?

    <p>Favors endothermic reactions.</p> Signup and view all the answers

    How does temperature decrease affect reactions?

    <p>Favors exothermic reactions.</p> Signup and view all the answers

    What does an increase in volume favor?

    <p>Favors the reaction with more moles.</p> Signup and view all the answers

    What does a decrease in pressure favor?

    <p>Favors the reaction with more moles.</p> Signup and view all the answers

    What does a decrease in volume favor?

    <p>Favors the reaction with less moles.</p> Signup and view all the answers

    What does an increase in pressure favor?

    <p>Favors the reaction with less moles.</p> Signup and view all the answers

    Study Notes

    Stoichiometry and Calculations

    • Stoichiometry focuses on mass relationships between reactants and products in balanced chemical equations.
    • Calculation steps: convert grams of given substance to moles, then convert moles of given to moles of unknown, and finally convert moles of unknown to grams.

    Percent Yield and Pressure

    • Percent yield formula: % yield = (actual yield/theoretical yield) x 100.
    • Pressure formula: Pressure = force/unit area; pressure is inversely related to area.

    Standard Temperature and Pressure

    • Standard Temperature and Pressure (STP) values: 0°C, 273 K, 760 mm Hg, 1 atm = 101.3 kPa.

    Moles and Volume at STP

    • 1 mole equates to 6.02 x 10^23 entities.
    • At STP, 6.02 x 10^23 entities occupy 22.4 L.

    Conversion Between Measures

    • Conversion order for grams, moles, and liters: Liters > Moles > Grams.
    • 1 L equals 1,000 mL.

    Graham's Law of Effusion

    • Gas effusion/diffusion rates are inversely proportional to the square root of their molar masses.
    • Equation: Rate A/Rate B = √(MMB/MMA).

    Heating and Cooling Curves

    • Heating Curve: solid > melting > liquid > boiling > gas; potential energy (PE) increases at plateaus and kinetic energy (KE) increases during the slopes.
    • Cooling Curve: gas > condensation > liquid > freezing > solid; PE decreases at plateaus and KE decreases during slopes.

    Boiling Points and Pressure Effects

    • At sea level, water boils at 100°C (760 mm Hg).
    • Lower atmospheric pressure makes it easier for a liquid to vaporize, reducing its boiling point (e.g., water boils at 94°C).

    Thermodynamic Reactions

    • Endothermic reactions absorb heat, increasing PE as matter transitions from ordered to less ordered states.
    • Exothermic reactions release heat, decreasing PE as matter moves from less ordered to more ordered states.

    System Types

    • In open systems, compounds can escape; in closed systems, like a sealed glass of water, evaporated molecules cannot escape.

    Equilibrium

    • Equilibrium is a dynamic state where opposing changes occur at equal rates in a closed system.
    • Condensation and evaporation are equal at equilibrium.

    Phase Changes

    • Melting (solid to liquid), sublimation (solid to gas), freezing (liquid to solid), vaporization (liquid to gas), condensation (gas to liquid), and deposition (gas to solid) represent the various phase changes.

    Critical and Triple Points

    • Triple point: specific conditions where solid, liquid, and gas co-exist in equilibrium.
    • Critical point denotes the temperature and pressure above which liquid cannot exist.

    Properties of Solids and Liquids

    • Solids have orderly structures with the highest intermolecular forces and least kinetic energy.
    • Liquids are less ordered than solids with weaker intermolecular forces and more kinetic energy.

    Solutions and Concentration

    • Molarity (M) measures concentration: M = moles of solute/liters of solvent.
    • Molality (m) formula: m = moles of solute/kilograms of solution.
    • Saturated, unsaturated, and supersaturated solutions refer to solute concentrations in solvents.

    Solvent Interactions

    • Immiscible liquids do not mix; miscible liquids dissolve freely in each other.
    • "Like dissolves like" indicates that solubility is influenced by polarity.

    Electrolytes and Colligative Properties

    • Strong electrolytes dissociate fully into ions; weak electrolytes partially dissociate.
    • Non-electrolytes do not produce ions in solution.
    • Colligative properties depend solely on solute particle number, not identity.

    Reaction Dynamics

    • REDOX reactions involve electron transfer, characterized by changes in oxidation state.
    • Oxidation signifies electron loss; reduction signifies electron gain.

    Thermodynamic Functions

    • Enthalpy (ΔH) and entropy (ΔS) indicate heat changes and disorder, respectively.
    • A negative ΔG denotes a spontaneous reaction; a positive ΔG indicates a non-spontaneous reaction.

    Factors Affecting Reaction Rates

    • Reaction speed influenced by temperature, concentration, catalysts, surface area, and reaction nature.
    • Increasing temperature favors endothermic reactions, while decreasing temperature favors exothermic reactions.

    Volume and Pressure Effects

    • Changes in volume and pressure shift equilibrium toward the side with fewer or more moles, depending on the direction of the change.

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    Description

    This quiz focuses on essential chemistry formulas and equations, specifically targeting stoichiometry and percent yield. Master these concepts to enhance your understanding of chemical reactions and their quantitative relationships. Ideal for review before your chemistry final exam.

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