Chemistry 101 Practice Final Exam (Ch 10-11)
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Questions and Answers

Which of the following is not a condition listed in the kinetic theory of reactions?

  • Molecules must collide to react
  • Collisions must have correct orientation
  • Molecules must be stationary (correct)
  • Collisions must have enough energy

What is the function of a catalyst in a reaction?

  • It increases the activation energy
  • It slows down the rate of a reaction
  • It is used up during a reaction
  • None of the above (correct)

When is a reversible reaction at equilibrium?

  • Only the rate of the forward reaction changes
  • Only the rate of the reverse reaction changes
  • The reaction rate of the forward and reverse reaction are not constant
  • The forward reaction rate equals the reverse reaction rate (correct)

For the equation 2BrNO (g) ↔ Br2 (g) + 2 NO (g), what is the proper form of the equilibrium expression?

<p>\frac{[Br2][NO]^2}{[BrNO]^2} (C)</p> Signup and view all the answers

If the equilibrium constant for N2O4 (g) ↔ 2 NO2 (g) is 4.3 x 10-3 and [NO2] = 0.053 M, what is the concentration of N2O4?

<p>0.0063 M (A)</p> Signup and view all the answers

Which of the following statements about catalysts is true?

<p>Catalysts provide an alternative pathway with lower activation energy (B)</p> Signup and view all the answers

In a dynamic equilibrium, which statement is accurate?

<p>The concentrations of reactants and products remain constant (D)</p> Signup and view all the answers

Which of the following correctly describes a Bronsted-Lowry acid?

<p>It donates protons. (D)</p> Signup and view all the answers

Which statement is true regarding the acid H3PO4?

<p>It is referred to as phosphoric acid. (A)</p> Signup and view all the answers

What is the correct chemical formula for aluminum hydroxide?

<p>Al(OH)3 (C)</p> Signup and view all the answers

In the reaction NH3 (aq) + H2O (l), which species is the Bronsted-Lowry acid?

<p>H2O (D)</p> Signup and view all the answers

From the equation H2SO4 + H2PO4- ↔ HSO4- + H3PO4, identify the conjugate acid/base pairs.

<p>H2SO4/HSO4- and H2PO4-/H3PO4 (B)</p> Signup and view all the answers

Given that H2SO4 has a pKa of 1, what can be inferred about the equilibrium mixture?

<p>It contains mostly products. (A)</p> Signup and view all the answers

Which of the following acids is the strongest based on their Ka values?

<p>Sulfuric acid (C)</p> Signup and view all the answers

What does an equilibrium constant less than 1 imply about the composition of a reaction mixture at equilibrium?

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

If the equilibrium constant Kc for the reaction 3H2 (g) + N2 (g) ↔ 2NH3 (g) is 1.7 x 10^2, how much NH3 can be expected if H2 is 0.18 M and N2 is 0.020 M?

<p>0.31 M (B)</p> Signup and view all the answers

What occurs to the equilibrium position if the temperature of the following reaction is decreased: CO (g) + H2O (g) ↔ CO2 (g) + H2 (g) + Heat?

<p>Shifts left towards the reactants (A)</p> Signup and view all the answers

For the equilibrium reaction CO (g) + H2O (g) ↔ CO2 (g) + H2 (g), how does adding H2 affect the equilibrium position?

<p>Shifts right towards the products (B)</p> Signup and view all the answers

Which of the following reactions would not change its equilibrium if the volume of the container is doubled?

<p>N2 (g) + O2 (g) ↔ 2NO (g) (C)</p> Signup and view all the answers

What is the result of adding a catalyst to the reaction C2H4 (g) + Cl2 (g) ↔ C2H4Cl2 (g) + Heat?

<p>No change in equilibrium position (D)</p> Signup and view all the answers

An equilibrium constant significantly greater than 1 indicates that at equilibrium, there is a predominance of which component?

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

How would the equilibrium position change in the reaction if the concentration of a reactant was decreased?

<p>Shifts left towards the reactants (A)</p> Signup and view all the answers

Which statement about weak acids is not true?

<p>They have a weak conjugate base (A)</p> Signup and view all the answers

What is the pH of a solution that has a hydroxide ion concentration of $1.5 \times 10^{-6} \text{ M}$?

<p>8.2 (A)</p> Signup and view all the answers

What is the concentration of hydronium ions, [H3O+], in a solution with a pH of 6.5?

<p>$3.2 \times 10^{-7} \text{ M}$ (A)</p> Signup and view all the answers

What is the pH of a solution with a pOH of 4.3?

<p>9.7 (B)</p> Signup and view all the answers

What type of solution results from a pH of 9.7?

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

What gas is produced in the reaction between KHCO3 (s) and HBr (aq)?

<p>CO2 (g) (C)</p> Signup and view all the answers

What volume of $0.621 ext{ M H3PO4}$ solution is needed to titrate $10.0 ext{ mL}$ of a $0.431 ext{ M KOH}$ solution?

<p>2.31 mL (B)</p> Signup and view all the answers

What is the molarity of acetic acid if $34.7 ext{ mL}$ of $0.235 ext{ M KOH}$ titrates $26.0 ext{ mL}$ of its solution?

<p>0.521 M (D)</p> Signup and view all the answers

What is the primary function of a buffer in a solution?

<p>To maintain pH (B)</p> Signup and view all the answers

What is the density of a medication if 16.5 mL has a mass of 42.9 g?

<p>2.60 g/mL (C)</p> Signup and view all the answers

How much energy is required for a cube of silver (density 10.5 g/cm³, volume 19.0 cm³) to increase its temperature from 16 °C to 24 °C?

<p>125 cal (D)</p> Signup and view all the answers

What is the total energy content in kilojoules for two tablespoons of peanut butter containing 4g carbohydrates, 13g fat, and 7g proteins?

<p>680 kJ (C)</p> Signup and view all the answers

Calculate the heat change in kJ for melting 170g of ice at 0°C.

<p>57 kJ (C)</p> Signup and view all the answers

What type of energy is stored in an object due to its position, such as a ball held above the ground?

<p>Potential energy (C)</p> Signup and view all the answers

Identify the type of nuclear reaction represented by a specific balanced equation.

<p>Fission reaction (D)</p> Signup and view all the answers

Which element has the electron configuration 1s²2s²2p³?

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

Using VSEPR theory, NI3 has what shape?

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

Which is the correct Lewis dot structure for BF4-?

<p>Four single bonds and a formal negative charge on B (A)</p> Signup and view all the answers

For the reaction 4Cr (s) + 3O2 (g) → 2Cr2O3 (s), how much product is produced from 32.0 g of each reactant?

<p>93.5 g (C)</p> Signup and view all the answers

If 16.3 g of product was produced from the previous question, what is the percent yield?

<p>34.8% (A)</p> Signup and view all the answers

How many kilojoules are released when 68.7 g of oxygen reacts in the reaction 2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l) ΔH = -726 kJ?

<p>520 kJ (A)</p> Signup and view all the answers

What is the final pressure, in mmHg, if the volume in a 4.00 L tank is decreased to 1.18 L with an initial pressure of 2.0 atm?

<p>5150 mmHg (A)</p> Signup and view all the answers

Calculate the number of equivalents (Eq) for 3 moles of Fe3+.

<p>6 Eq (B)</p> Signup and view all the answers

Which of the following ionic compounds are soluble in water?

<p>Na3PO4 (C)</p> Signup and view all the answers

Flashcards

Bronsted-Lowry Acid

A substance that donates a proton (H+).

Bronsted-Lowry Base

A substance that accepts a proton (H+).

Conjugate Base

The species formed after a Brønsted–Lowry acid loses a proton.

Conjugate Acid

The species formed after a Brønsted–Lowry base gains a proton.

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Acid Dissociation Constant (Ka)

The equilibrium constant for the ionization of an acid. It measures the strength of the acid.

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pKa

The negative logarithm of the acid dissociation constant (Ka). It also measures the strength of the acid.

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Neutralization Reaction

The reaction between an acid and a base, resulting in the formation of salt and water. It involves the transfer of protons from the acid to the base.

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Acidic Solution

A solution with a pH less than 7.

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What does Kc < 1 indicate?

An equilibrium constant (Kc) less than 1 indicates that the equilibrium mixture contains mostly reactants, meaning the reverse reaction is favored.

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What does Kc > 1 indicate?

An equilibrium constant (Kc) greater than 1 indicates that the equilibrium mixture contains mostly products, meaning the forward reaction is favored.

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How does a catalyst affect equilibrium?

A catalyst increases the rate of both the forward and reverse reactions equally, leading to a faster attainment of equilibrium but no shift in its position.

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What happens to equilibrium when a product is added?

Adding a product to a reaction at equilibrium will cause the reaction to shift left towards the reactants to relieve the stress on the system.

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What happens to a reaction's equilibrium when temperature is decreased?

Decreasing the temperature of an exothermic reaction favors the forward reaction, shifting the equilibrium towards the products.

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What happens to equilibrium when a reactant is added?

Adding a reactant to a reaction at equilibrium will cause the reaction to shift right towards the products to relieve the stress on the system.

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What type of reaction's equilibrium is not affected by volume change?

Changing the volume of a reaction vessel at equilibrium does not affect the equilibrium position if the number of moles on both sides of the balanced chemical equation is the same.

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What is KOH?

KOH (Potassium Hydroxide) is a strong base, meaning it completely dissociates in solution, releasing OH- ions.

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Activation Energy

The minimum energy that colliding reactant molecules must possess in order to break bonds and form new ones, leading to a chemical reaction.

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Catalyst

A substance that speeds up the rate of a reaction without being consumed in the process. Catalysts lower the activation energy, making it easier for reactions to occur.

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Chemical Equilibrium

A state where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products over time.

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Equilibrium Constant (K)

A constant that expresses the ratio of product concentrations to reactant concentrations at equilibrium. It indicates the relative extent to which a reaction proceeds to completion.

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Equilibrium Expression

The expression that shows the relationship between the concentrations of reactants and products at equilibrium. It is calculated by dividing the product of the concentrations of the products (raised to their stoichiometric coefficients) by the product of the concentrations of the reactants (raised to their stoichiometric coefficients).

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Reversible Reaction

A type of chemical reaction where the products can react to reform the original reactants. Reactions can proceed in both the forward and reverse directions.

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Rate of Reaction

The condition that occurs when a system's forward reaction rate equals its reverse reaction rate.

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Kinetic Theory of Reactions

A set of principles that explain the behavior of gases and the conditions necessary for a reaction to occur. These principles involve factors like collisions, energy, and orientation of molecules.

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What is a buffer?

A buffer is a solution that resists changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid.

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What is density?

Density is a measure of mass per unit volume. It tells you how much matter is packed into a given space.

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What is specific heat?

Specific heat capacity is the amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius.

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What is potential energy?

Potential energy is the energy stored in an object due to its position or configuration. It's like energy waiting to be unleashed.

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What is Fission?

The equation represents a type of nuclear reaction that releases energy by splitting a heavy nucleus into lighter nuclei.

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What is Electron Configuration?

Electron configuration describes the distribution of electrons in an atom's energy levels and orbitals. It's like the 'address' of electrons around the nucleus.

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What is Atomic Radius?

Atomic radius is a measure of the size of an atom. It's the average distance from the nucleus to the outermost electron.

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Why does some element have the smallest atomic radius?

Smaller atomic radius means the atom has a strong attraction between the nucleus and its electrons, pulling them closer.

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What is the VSEPR shape of NI3?

The shape of the molecule NI3 is a trigonal pyramidal due to the presence of one lone pair of electrons on the central nitrogen atom.

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What is the Lewis dot structure of BF4-?

BF4- has four bonding pairs and no lone pairs on the central Boron atom. Therefore, the Lewis dot structure is tetrahedral which is the most stable arrangement for four bonding pairs.

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How much Cr2O3 is produced from 32.0g of each reactant?

This problem requires stoichiometry calculations. First, calculate the limiting reactant by finding the moles of each reactant. Then, use the mole ratio from the balanced equation to convert moles of the limiting reactant to moles of product. Finally, convert moles of product to grams using the molar mass. The final answer should be 64.0 g.

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What is the percent yield for the reaction if 16.3g of product is produced?

Percent yield is calculated using the formula (Actual Yield / Theoretical Yield) x 100%. Using the theoretical yield from the previous question and the provided actual yield of 16.3 g, the percent yield is 25.5%.

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How many kJ are released when 68.7g of oxygen reacts?

First, convert the given mass of oxygen (68.7 g) to moles using its molar mass. Then, use the enthalpy change (ΔH = -726 kJ) and the mole ratio from the balanced equation to calculate the energy released. The final answer is 1500 kJ.

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What is the final pressure in mmHg if the volume is decreased?

This problem involves Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume, assuming constant temperature. The initial pressure (P1) is 2.0 atm and the initial volume (V1) is 4.00 L. The final volume (V2) is 1.18 L. Applying Boyle's Law, the final pressure (P2) is calculated to be 6.78 atm, which converts to 5150 mmHg.

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How many Eq are in 3 moles of Fe3+?

An equivalent (Eq) is the amount of a substance that reacts with or is equivalent to one mole of hydrogen ions (H+). Fe3+ has a charge of +3, so it is equivalent to 3 moles of H+. Therefore, 3 moles of Fe3+ equals 9 Eq.

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Which ionic compound is soluble in water?

Solubility rules are used to predict whether an ionic compound will dissolve in water. Na3PO4 is soluble in water as all salts containing Group 1 metals are soluble. However, the other options are not soluble. Therefore, only Na3PO4 is soluble.

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What is the final concentration after dilution?

Using the formula M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume, we can calculate the final concentration. Plugging in the values gives us (4.0 M)(3.5 L) = (M2)(8.0 L), which results in a final concentration of 1.75 M.

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What is a characteristic of weak acids?

A weak acid has a small Ka value, which indicates that it only partially dissociates in solution, resulting in a low concentration of hydrogen ions.

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What's the relationship between pH and [H+]?

The pH of a solution is the negative logarithm of the hydrogen ion concentration ([H+]). It measures the acidity or alkalinity of a solution.

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What is pOH and how does it relate to [OH-]?

The pOH of a solution is the negative logarithm of the hydroxide ion concentration ([OH-]). It measures the alkalinity of a solution.

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What is a buffer solution?

A buffer solution resists changes in pH when small amounts of acid or base are added. It's a combination of a weak acid and its conjugate base or a weak base and its conjugate acid.

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What is titration?

Titration is a technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. It involves adding a titrant solution to the analyte solution until a chemical reaction reaches its endpoint.

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What is the equivalence point in a titration?

The equivalence point in a titration is the point at which the moles of acid and base are stoichiometrically equivalent. It's often marked by a color change in the solution, indicating completion of the reaction.

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What is solution concentration?

The concentration of a solution is the amount of solute dissolved in a given amount of solvent. It's often expressed in molarity (moles per liter).

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What is dilution?

Dilution is the process of reducing the concentration of a solution by adding more solvent. The total amount of solute remains the same, but the concentration decreases.

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Study Notes

Chemistry 101 Practice Final Exam (Chapters 10-11)

  • Exam Focus: Questions based on material from chapters 10 and 11.
  • Exam Tools: Only use the equation sheets from Exam 1. Avoid outside resources such as books, notes, or the internet.
  • Question 1: Which of the following is NOT a kinetic theory condition for reactions?
    • Correct answer is: Molecules must be stationary.
  • Question 2: What is the function of a catalyst?
    • Correct answer: It increases the rate of a reaction. It does not use or change during a reaction.
  • Question 3: When does a reversible reaction reach equilibrium?
    • Correct answer: When the rates of the forward and reverse reactions are equal.
  • Question 4: Equilibrium Constant Calculation
    • Given reaction: CO2 (g) + H2 (g) → CO (g) + H2O (g)
    • Data provided: Concentrations of reactants and products.
    • Calculate Kc.
  • Question 5: Equilibrium Expression
    • Given reaction: 2BrNO (g) → Br₂ (g) + 2 NO (g)
    • Correct expression: Kc = [Br₂][NO]² / [BrNO]²
  • Question 6: Equilibrium Constant and Concentration
    • Given reaction: N₂O₄(g) ↔ 2NO₂(g)
    • Equilibrium constant = 4.3 x 10⁻³.
    • Equilibrium [NO₂] = 0.053 M
    • Calculate the molar concentration of N₂O₄.
  • Question 7: Equilibrium Mixture Composition Based on K
    • Large Kc values indicate mostly products at equilibrium.
    • Small Kc values indicate mostly reactants at equilibrium.
  • Question 8: Equilibrium Composition and Kc
    • Kc > 1: Mostly products
    • Kc < 1: Mostly reactants.
    • Kc = 1: equal amounts of products and reactants.
  • Question 9: Using Equilibrium Constant to Calculate Concentration
    • Given reaction: 3H₂(g) + N₂(g) → 2NH₃(g)
    • Equilibrium constant (Kc) = 1.7 x 10².
    • Equilibrium concentrations of H₂ and N₂.
    • Calculate the molar concentration of NH₃.
  • Question 10: Effect of Temperature Change on Equilibrium
    • If temperature decreases, the equilibrium shifts to favor the exothermic direction (heat is a product).
  • Question 11: Effect of Adding Reactant on Equilibrium
    • Adding a reactant causes equilibrium to shift towards products.
  • Question 12: Effect of Volume Change on Equilibrium
    • An equilibrium where the number of moles of gas is the same on both sides of the equation is unaffected by a change in volume.
  • Question 13: Effect of Catalyst on Equilibrium
    • Catalysts do not affect the position of equilibrium.

Additional Chemistry Concepts (from pages 3-8)

  • Acids and Bases: Definitions, properties, and examples of acids and bases (KOH, H₃PO₄, etc.).
  • pH and pOH: Calculations and relations for pH and pOH .
  • Buffer Solutions: Their purpose, components, and pH regulation
  • Titration: Calculations for volumes and concentrations of solutions involved.
  • Redox Reactions: Calculations and equilibrium expressions in reactions
  • Nuclear Chemistry: Types of nuclear reactions.
  • VSEPR Theory: Predicting shapes of molecules and ions.
  • Thermodynamics: Heat changes, equilibrium, and calculating heat needed to increase temperature for materials.
  • Stoichiometry: Calculations relating reactants and products in a reaction (using grams).

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Test your knowledge with this practice final exam for Chemistry 101, focusing on material from chapters 10 and 11. This quiz includes questions about kinetic theory, catalysts, and equilibrium reactions. Use your equation sheets from Exam 1 to assist you in answering the questions.

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