Chemical Equilibrium Concepts
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Questions and Answers

Which factor does NOT affect the position of equilibrium in a chemical reaction?

  • Pressure
  • Concentration of reactants
  • Color of the reactants (correct)
  • Temperature

    • Le Chatelier's Principle states that a change in pressure promotes a shift in equilibrium to favor the reactants.

    False

    What is the formula for calculating molarity?

    M = mol/L

    According to Le Chatelier's Principle, a system at equilibrium will shift to counteract the effect of a change in __________.

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

    Match each action with its corresponding effect on equilibrium:

    <p>Increasing concentration of products = Shift towards reactants Decreasing pressure = Shift towards more gas molecules Increasing temperature for an endothermic reaction = Shift towards products Adding a catalyst = No shift in equilibrium position</p> Signup and view all the answers

    How can you speed up the process of dissolving a solid in a liquid?

    <p>Increase the surface area of the solid</p> Signup and view all the answers

    A neutralization reaction always produces salts and water.

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

    What does the term 'collision theory' refer to in the context of chemical reactions?

    <p>It explains how reactants must collide with sufficient energy and proper orientation to react.</p> Signup and view all the answers

    What is the molarity of SO2Cl2 in the flask?

    <p>0.100 M</p> Signup and view all the answers

    Which direction will the reaction proceed to establish equilibrium?

    <p>Forward direction</p> Signup and view all the answers

    A solution that contains the maximum amount of solute is described as unsaturated.

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

    Define what a solute is.

    <p>A solute is the substance that is dissolved in a solvent to form a solution.</p> Signup and view all the answers

    The reaction quotient, Q, is calculated using concentrations expressed in _____ per liter.

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

    Match the solution type with its definition:

    <p>Saturated = Contains maximum solute at given temperature Unsaturated = Contains less solute than it could hold Supersaturated = Contains more solute than a saturated solution Electrolyte = Conducts electricity when dissolved in water</p> Signup and view all the answers

    What oxygen-containing compound is involved in the equilibrium reaction?

    <p>SO2</p> Signup and view all the answers

    The solubility of solids increase with temperature.

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

    Explain how agitation affects solubility.

    <p>Agitation increases the contact and collision frequency between solute and solvent particles, thus enhancing dissolution.</p> Signup and view all the answers

    Which of the following is a binary acid?

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

    A substance that does not conduct electricity when dissolved in water is called a _____ solute.

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

    At what temperature does a supersaturated solution of potassium nitrate occur?

    <p>75°C</p> Signup and view all the answers

    Hydrobromic acid is represented by the formula HBr.

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

    What is the molar concentration of aluminum sulfate if the sulfate ion concentration is 0.545 M?

    <p>0.182 M</p> Signup and view all the answers

    The reaction remains constant and does not change over time in a saturated solution.

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

    The strong base potassium hydroxide is represented by the formula ______.

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

    Calculate the molarity of Cl2 in the flask.

    <p>0.016 M</p> Signup and view all the answers

    Match the acid to its correct formula:

    <p>Nitric acid = HNO3 Sulfuric acid = H2SO4 Hydrochloric acid = HCl Phosphoric acid = H3PO4</p> Signup and view all the answers

    When calculating molarity, you divide the number of _____ by the volume of the solution in liters.

    <p>moles of solute</p> Signup and view all the answers

    Which acid is formed when one H+ ion is added to the sulfate ion?

    <p>H2SO4</p> Signup and view all the answers

    All strong acids have strong conjugate bases.

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

    Name the acid represented by the formula H2SO3.

    <p>Sulfurous acid</p> Signup and view all the answers

    The formula for acetic acid is ______.

    <p>CH3COOH or HC2H3O2</p> Signup and view all the answers

    Which of the following is NOT classified as a strong acid?

    <p>CH3COOH</p> Signup and view all the answers

    The chemical formula for hydroiodic acid is HI.

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

    What is the oxidation state of sulfur in sulfuric acid (H2SO4)?

    <p>6</p> Signup and view all the answers

    Match the following acids with their common names:

    <p>H3PO4 = Phosphoric acid HNO2 = Nitrous acid H2CO3 = Carbonic acid HCl = Hydrochloric acid</p> Signup and view all the answers

    Which reaction is favored by an increase in temperature?

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

    The addition of a catalyst will change the position of the equilibrium.

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

    What effect does an increase in pressure have on the concentration of reactants if the forward reaction is favored?

    <p>The concentration of reactants will decrease.</p> Signup and view all the answers

    In a heterogeneous equilibrium expression, _______ are not included.

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

    Match the following equilibria symbols with their meanings:

    <p>Kc = Equilibrium constant using molar concentrations Kp = Equilibrium constant using partial pressures Ksp = Solubility product Ka = Acid dissociation constant</p> Signup and view all the answers

    What condition indicates the system is at equilibrium?

    <p>Q = K</p> Signup and view all the answers

    A decrease in temperature favors the endothermic reaction.

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

    What does the reaction quotient Q represent?

    <p>The ratio of the concentrations or partial pressures of products over reactants at any state.</p> Signup and view all the answers

    The expression for Kc in the reaction aA + bB ⇄ cC + dD is __________.

    <p>Kc = [C]^c[D]^d / [A]^a[B]^b</p> Signup and view all the answers

    Which of the following affects both forward and reverse reactions equally?

    <p>Adding a catalyst</p> Signup and view all the answers

    Kc can be calculated for reactions only at equilibrium.

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

    In the reaction N2(g) + 3H2(g) ⇄ 2NH3(g), what is the expression for Kc?

    <p>Kc = [NH3]^2 / ([N2][H2]^3)</p> Signup and view all the answers

    If Q < K, the reaction will proceed _______ to reach equilibrium.

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

    Match the following reactions with their equilibrium expressions:

    <p>H2(g) + I2(g) ⇄ 2HI(g) = Kc = [HI]^2 / ([H2][I2]) CaCO3(s) ⇄ CaO(s) + CO2(g) = Kp = [PCO2] PbI2(s) ⇄ Pb+2(aq) + 2I-(aq) = Ksp = [Pb+2][I-]^2 Fe(OH)3(s) ⇄ Fe+3(aq) + 3OH-(aq) = Ksp = [Fe+3][OH-]^3</p> Signup and view all the answers

    What happens to equilibrium when the concentration of reactants is increased?

    <p>The equilibrium shifts to the right.</p> Signup and view all the answers

    If the concentration of products is decreased, the equilibrium will shift to the left to produce more products.

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

    What does Le Chatelier's principle state about equilibrium when a system is stressed?

    <p>It will shift to counteract the stress.</p> Signup and view all the answers

    An increase in _____ shifts the equilibrium towards the side with fewer moles in gaseous reactions.

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

    Match the changes in reaction conditions with their effects on equilibrium:

    <p>Increasing temperature = Favors the endothermic reaction Decreasing temperature = Favors the exothermic reaction Increasing reactant concentration = Shifts equilibrium to the right Increasing product concentration = Shifts equilibrium to the left</p> Signup and view all the answers

    The concentration of Cl− ions in a 0.035 M solution of CaCl2 is 0.070 M.

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

    In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if SO3 concentration is decreased?

    <p>Equilibrium shifts to produce more SO3.</p> Signup and view all the answers

    What is the concentration of K+ ions in a solution made from 7.5 g of K2S in 250 mL?

    <p>0.09 M</p> Signup and view all the answers

    In an exothermic reaction, increasing the temperature favors the forward reaction.

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

    What type of reaction is favored when the temperature is decreased?

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

    In the dissociation of Al2(SO4)3, the ratio of aluminum ions to sulfate ions is ___.

    <p>2:3</p> Signup and view all the answers

    Match the following ionic compounds to their respective ion concentrations:

    <p>CaCl2 = 2 Cl− CuCl3 = 3 Cl− K2S = 2 K+ and 1 S2− Na3PO4 = 3 Na+ and 1 PO4^3−</p> Signup and view all the answers

    If the concentration of a reactant decreases, the equilibrium will shift to produce more _____ of that reactant.

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

    When preparing a standard solution, what is the purpose of wetting the pipette?

    <p>To remove any residues from the pipette</p> Signup and view all the answers

    What effect does adding heat to an endothermic reaction have on equilibrium?

    <p>It shifts the equilibrium to the right.</p> Signup and view all the answers

    Match the following reactions to their conditions:

    <p>N2(g) + 3H2(g) ⇌ 2NH3(g) ΔH=−92 = Exothermic reaction Increasing reactants in a reversible reaction = Shifts towards products Increasing products in a reversible reaction = Shifts towards reactants Pressure increases in gaseous reactions = Shifts to fewer moles</p> Signup and view all the answers

    Students should discard the solution used to wet the pipette into the beaker provided or down the sink.

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

    When pressure is increased in a gaseous reaction, the equilibrium shifts to the side with more moles.

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

    What is the concentration of sulfate ions in a 0.500 M solution of sodium phosphate?

    <p>0 M</p> Signup and view all the answers

    The final step in preparing a diluted solution is to ___ the flask.

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

    What happens to the yield of ammonia when the temperature is decreased in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)?

    <p>The yield increases.</p> Signup and view all the answers

    Match the process with its description:

    <p>Dilution = Reducing concentration by adding more solvent Dissociation = Separation of soluble compounds into ions Stoichiometry = Calculating quantities in reactions Pipetting = Transferring precise volumes of liquid</p> Signup and view all the answers

    In a reversible reaction, if more _____ are added, the equilibrium shifts toward the products.

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

    If the concentration of calcium ions is 0.035 M in CaCl2, what is the total concentration of chloride ions?

    <p>0.070 M</p> Signup and view all the answers

    What best describes the outcome when the concentration of a product is increased?

    <p>The equilibrium shifts to the left.</p> Signup and view all the answers

    If the water exceeds the marked volume during dilution, the dilution must be redone.

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

    What ion concentrations must be calculated when determining ion compositions in a compound like sodium phosphate?

    <p>Sodium ion and phosphate ion concentrations</p> Signup and view all the answers

    When water is added to dissolve K2S, the resulting solution has concentrations of ___ for K+ and S2−.

    <p>0.09 M for K+, 0.03 M for S2−</p> Signup and view all the answers

    What is the correct way to express a molarity of 1.00 M?

    <p>One point oh oh molar</p> Signup and view all the answers

    The molarity of a solution is calculated based on the volume of pure water used to prepare the solution.

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

    What is Avogadro's Number?

    <p>6.022 x 10^23</p> Signup and view all the answers

    When calculating molarity, you must convert grams to __________ first.

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

    What happens to the equilibrium when pressure is increased?

    <p>It favors the side with fewer gas molecules.</p> Signup and view all the answers

    Match the compound to its molar mass:

    <p>NaCl = 58.44 g/mol KMnO4 = 158.0 g/mol C6H12O6 = 180.0 g/mol H2SO4 = 98.08 g/mol</p> Signup and view all the answers

    Which of the following is true when temperature decreases in an exothermic reaction?

    <p>The exothermic reaction is favored.</p> Signup and view all the answers

    Which of the following statements about molarity is true?

    <p>Molarity is defined as moles of solute per liter of solution.</p> Signup and view all the answers

    A catalyst has a significant effect on the position of equilibrium in a chemical reaction.

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

    What happens to the yield of NH3 when pressure is decreased in the reaction of N2 and H2?

    <p>The yield of NH3 decreases.</p> Signup and view all the answers

    A solution of 0.500 mol/L and 0.500 M represents the same concentration.

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

    In the reaction A + B ⇋ C + D, if ΔH = -75 kJ, then the reaction is _____.

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

    If you dissolve 80.0 grams of glucose in enough water to make 1.00 L of solution, what is its molarity?

    <p>0.444 M</p> Signup and view all the answers

    Match the following reactions with their respective changes in pressure:

    <p>N2(g) + 3H2(g) ⇌ 2NH3(g) = Equilibrium shifts right with increased pressure 2SO2(g) + O2(g) ⇌ 2SO3(g) = Equilibrium shifts right with increased pressure A + B ⇋ C + D (endothermic) = Equilibrium shifts left with decreased pressure C + D ⇋ A + B (exothermic) = Equilibrium shifts right with decreased pressure</p> Signup and view all the answers

    Molarity is abbreviated as __________.

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

    Match the following terms with their definitions:

    <p>Molar Mass = Mass of one mole of a substance in grams Molarity = Moles of solute per liter of solution Dilution = Process of reducing concentration by adding more solvent Concentration = Amount of solute in a given volume of solution</p> Signup and view all the answers

    When analyzing the equilibrium state in a rate-time graph, what does it indicate?

    <p>The system is at equilibrium.</p> Signup and view all the answers

    How does an increase in temperature affect an endothermic reaction?

    <p>It favors the forward reaction.</p> Signup and view all the answers

    The molarity of a solution can remain the same regardless of the solute's identity.

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

    Increasing the concentration of reactants will always result in an increased rate of the forward reaction.

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

    What volume of solution will result when 15.0 g of H2SO4 is dissolved to make a 0.200 M solution?

    <p>0.375 L</p> Signup and view all the answers

    What color change is observed when the temperature is decreased in the reaction involving NO2 and N2O4?

    <p>The color becomes paler.</p> Signup and view all the answers

    To perform a dilution calculation, the total volume created is based on the final __________ of the solution.

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

    A sharp increase in reaction rate occurs with a change in _____.

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

    What is impacted by a decrease in pressure during a reaction?

    <p>The equilibrium will shift to the side with more gas molecules.</p> Signup and view all the answers

    What is Keq and when can it be calculated?

    <p>Keq is the equilibrium constant and can only be calculated when the system is at equilibrium.</p> Signup and view all the answers

    Match the gases with their respective changes in equilibrium due to pressure changes:

    <p>N2 + 3H2 ⇌ 2NH3 = Shift right with increased pressure 2SO2 + O2 ⇌ 2SO3 = Shift right with increased pressure 2NO2 ⇋ N2O4 = Shift left with increased pressure A + B ⇋ C + D = Depends on the number of gas molecules</p> Signup and view all the answers

    Study Notes

    Equilibrium Concepts

    • Chemical equilibrium is a state where the forward and reverse reaction rates are equal, resulting in no net change in concentration.
    • Le Chatelier's Principle: A change in a system at equilibrium causes a shift to counteract the change. This includes changes in concentration, temperature, and pressure (for gaseous systems).

    Equilibrium Stress Factors

    • Concentration Changes: Adding reactants shifts equilibrium to products (forward). Adding products shifts equilibrium to reactants (reverse). Decreasing reactant concentration shifts equilibrium in the direction that produces more reactant (reverse). Decreasing product concentration shifts the equilibrium in the direction that produces more product (forward).

    • Temperature Changes: Increased temperature favors the endothermic reaction (absorbs heat). Decreased temperature favors the exothermic reaction (releases heat).

    • Pressure Changes: Increased pressure favors the side with fewer gas moles. Decreased pressure favors the side with more gas moles.

    Equilibrium Constant

    • Equilibrium constant (K) is calculated using the concentrations (or partial pressures) of products and reactants at equilibrium.
    • Formula: K = [Products]coefficient / [Reactants]coefficient (Kc for concentrations, Kp for partial pressures)
    • Solids and liquids are excluded from equilibrium constant expressions.

    Reaction Quotient (Q)

    • Q is calculated the same way as K but can be calculated for any set of conditions, not just equilibrium.
    • If Q < K, the reaction will proceed forward to reach equilibrium.
    • If Q > K, the reaction will proceed in reverse to reach equilibrium.
    • If Q = K, the system is already at equilibrium.

    Molarity Calculations

    • Molarity (M) is moles of solute per liter of solution.
    • Formula: M = moles of solute / liters of solution.
    • Convert grams of solute to moles using molar mass.

    Dilution Calculations

    • Dilution involves adding solvent to a solution to decrease its concentration.
    • Formula: M1V1 = M2V2 (where M1 and V1 are the initial concentration and volume, and M2 and V2 are the final concentration and volume).

    Acid Nomenclature

    • Binary Acids: Hydro-(root)-ic acid (e.g., HCl – hydrochloric acid).
    • Oxyacids: (root)-ic or -(root)-ous acid, based on the polyatomic ion. (e.g., HNO3 – nitric acid, H2SO4 – sulfuric acid, HNO2 – nitrous acid)

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    Description

    Explore the key principles of chemical equilibrium through this quiz. Understand Le Chatelier's Principle and how changes in concentration, temperature, and pressure affect equilibrium. Test your knowledge on these fundamental concepts in chemistry.

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