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?

\frac{[Br2][NO]^2}{[BrNO]^2} 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?

0.0063 M Signup and view all the answers

Which of the following statements about catalysts is true?

Catalysts provide an alternative pathway with lower activation energy Signup and view all the answers

In a dynamic equilibrium, which statement is accurate?

The concentrations of reactants and products remain constant Signup and view all the answers

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

It donates protons. Signup and view all the answers

Which statement is true regarding the acid H3PO4?

It is referred to as phosphoric acid. Signup and view all the answers

What is the correct chemical formula for aluminum hydroxide?

Al(OH)3 Signup and view all the answers

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

H2O Signup and view all the answers

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

H2SO4/HSO4- and H2PO4-/H3PO4 Signup and view all the answers

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

It contains mostly products. Signup and view all the answers

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

Sulfuric acid Signup and view all the answers

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

Mostly reactants 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?

0.31 M 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?

Shifts left towards the reactants 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?

Shifts right towards the products Signup and view all the answers

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

N2 (g) + O2 (g) ↔ 2NO (g) Signup and view all the answers

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

No change in equilibrium position Signup and view all the answers

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

Mostly products Signup and view all the answers

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

Shifts left towards the reactants Signup and view all the answers

Which statement about weak acids is not true?

They have a weak conjugate base Signup and view all the answers

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

8.2 Signup and view all the answers

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

$3.2 \times 10^{-7} \text{ M}$ Signup and view all the answers

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

9.7 Signup and view all the answers

What type of solution results from a pH of 9.7?

Basic Signup and view all the answers

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

CO2 (g) 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?

2.31 mL 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?

0.521 M Signup and view all the answers

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

To maintain pH Signup and view all the answers

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

2.60 g/mL 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?

125 cal 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?

680 kJ Signup and view all the answers

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

57 kJ 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?

Potential energy Signup and view all the answers

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

Fission reaction Signup and view all the answers

Which element has the electron configuration 1s²2s²2p³?

Nitrogen Signup and view all the answers

Using VSEPR theory, NI3 has what shape?

trigonal pyramidal Signup and view all the answers

Which is the correct Lewis dot structure for BF4-?

Four single bonds and a formal negative charge on B 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?

93.5 g Signup and view all the answers

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

34.8% 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?

520 kJ 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?

5150 mmHg Signup and view all the answers

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

6 Eq Signup and view all the answers

Which of the following ionic compounds are soluble in water?

Na3PO4 Signup and view all the answers

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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Description

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.