Chemistry Chapter 11 Quiz

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Questions and Answers

What is a characteristic property of the solid state of matter?

Solids retain their own volume.

Which type of interaction, intramolecular or intermolecular, is generally stronger?

Intramolecular interactions are generally stronger.

What kind of interactions are broken when a liquid is converted to a gas?

Intermolecular interactions are broken.

Provide an example of an intermolecular force.

Hydrogen bonding. Signup and view all the answers

What are the two types of interactions that are broken when a substance melts?

Both intermolecular and intramolecular interactions are broken. Signup and view all the answers

If you have two substances with similar molecular weights, but one is a liquid at room temperature and the other is a gas, what can you conclude about the intermolecular forces between the molecules of each substance?

The substance that is a liquid at room temperature has stronger intermolecular forces than the substance that is a gas. Signup and view all the answers

What is the difference between intermolecular and intramolecular forces?

Intermolecular forces exist between molecules, whereas intramolecular forces exist within molecules. Signup and view all the answers

Which of the following substances is most likely to be a liquid at room temperature: methane ($CH_4$), water ($H_2O$), or nitrogen ($N_2$)? Explain your reasoning.

Water ($H_2O$) is most likely to be a liquid at room temperature due to its strong hydrogen bonding. Signup and view all the answers

What type of solution has the capacity to dissolve more solute at a given temperature?

An unsaturated solution. Signup and view all the answers

Which of the following solids is held together by the weakest interactions: metallic solids, covalent network solids, ionic solids, or molecular solids?

Molecular solids are held together by the weakest interactions. Signup and view all the answers

What type of bond is responsible for holding together metallic solids?

Metallic solids are held together by a delocalized 'sea' of collectively shared valence electrons. Signup and view all the answers

How does the solubility of a gas in a solvent change with increasing partial pressure of the gas above the solvent?

The solubility of a gas in a solvent increases with increasing partial pressure of the gas above the solvent. Signup and view all the answers

Why do substances with similar intermolecular attractive forces tend to be soluble in one another?

Substances with similar intermolecular attractive forces tend to be soluble in one another because they can interact favorably, creating a stable solution. Signup and view all the answers

Explain why the solubility of most solid solutes in water generally decreases as the temperature increases.

The solubility of most solid solutes in water generally decreases as the temperature increases because the process of dissolving a solid in water is usually an endothermic process. Signup and view all the answers

Explain why the solubility of a gas in water generally decreases as the temperature increases.

The solubility of a gas in water generally decreases as the temperature increases because the process of dissolving a gas in water is usually an exothermic process. Signup and view all the answers

What type of intermolecular force is responsible for the attraction between molecules of hydrogen peroxide (H2O2)?

Hydrogen bonding Signup and view all the answers

Which of the following molecules would exhibit both London dispersion forces and dipole-dipole forces: hydrogen sulfide (H2S), fluoromethane (CH3F), or formaldehyde (H2CO)?

Hydrogen sulfide (H2S) and fluoromethane (CH3F) Signup and view all the answers

Describe the difference between ion-dipole forces and dipole-dipole forces.

Ion-dipole forces occur between an ion and a polar molecule, while dipole-dipole forces occur between two polar molecules. Signup and view all the answers

What physical property of a liquid is measured by the time it takes for a specific amount of the liquid to flow through a narrow vertical tube?

Viscosity Signup and view all the answers

What is the relationship between the viscosity of a liquid and its temperature?

Viscosity generally decreases with increasing temperature. Signup and view all the answers

What is the specific point on a phase diagram where a substance can exist in all three phases (solid, liquid, and gas) in equilibrium?

Triple point Signup and view all the answers

Explain the difference between the critical point and the triple point on a phase diagram.

The critical point represents the highest temperature and pressure at which a liquid can exist, while the triple point is the point where all three phases coexist in equilibrium. Signup and view all the answers

What is meant by the term "normal boiling point"?

The normal boiling point is the temperature at which a liquid boils at standard atmospheric pressure (1 atm). Signup and view all the answers

Why is the molecularity of the step described as "termolecular"?

It's termolecular because the reaction rate law is third order, meaning the rate is dependent on the concentration of three reactants (A and B in this case). Signup and view all the answers

If a reaction has the following rate law, what is the order of the reaction? `rate = k[A][B]^2`

The overall order of the reaction is three, as the exponents in the rate law add up to three. Signup and view all the answers

How does increasing the temperature generally affect the rate of chemical reactions?

Increasing temperature generally increases the rate of chemical reactions. Signup and view all the answers

What is the relationship between the order of a reaction and its molecularity?

There is no direct relationship. Order refers to how the rate of a reaction depends on the concentration of reactants, while molecularity describes the number of molecules involved in the elementary step. Signup and view all the answers

What is the rate law for the following reaction: `2NO(g) + 2H2(g) → N2(g) + 2H2O(g)` given that the rate is first order in H2 and second order in NO?

The rate law is <code>rate = k[H2][NO]^2</code>. Signup and view all the answers

What are the units typically associated with reaction rates?

The units for reaction rates are typically expressed as moles/s. Signup and view all the answers

How is the frequency factor (A) related to the rate constant (k)?

The frequency factor (A) is related to the rate constant (k) through the Arrhenius equation: <code>k = A * exp(-Ea/RT)</code> Signup and view all the answers

What is the activation energy? How does it influence a reaction?

The activation energy is the minimum energy required for a reaction to occur. It is the energy difference between the reactants and the transition state. A higher activation energy results in a slower reaction rate since fewer molecules will have enough energy to react. Signup and view all the answers

What is the freezing point depression of a solution containing 475.0 g of ethylene glycol in 5.00 kg of water? The Kf for water is 1.86 °C/m.

2.85 °C Signup and view all the answers

A 90 mg sample of an unknown white powder is dissolved in 1.56 mL of ethanol, and the freezing point of the solution is lowered to -115.6 °C. If the normal freezing point of ethanol is -114.6 °C and the Kf for ethanol is 1.99 °C/m, what is the molar mass of the unknown powder?

The molar mass of the unknown powder can be calculated using the formula ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the freezing point depression constant, and m is the molality of the solution. The molality of the solution can be calculated from the mass of the unknown powder and the mass of the ethanol. The molar mass of the unknown powder can then be calculated from the molality and the mass of the unknown powder. Signup and view all the answers

What is the average rate of disappearance of A in the reaction A → B, if the initial concentration of A is 0.91 M and the concentration of A after 90 minutes is 0.11 M?

The average rate of disappearance of A is -8.9 × 10^-3 M/min. This is calculated using the formula Rate = -Δ[A]/Δt where Δ[A] is the change in concentration of A and Δt is the change in time. Signup and view all the answers

For the reaction 2AsH3(g) → As2(g) + 3H2(g), express the reaction rate in terms of the change in concentration of H2 over time.

The reaction rate can be expressed as +3Δ[H2]/Δt. This is because the stoichiometric coefficient of H2 in the balanced chemical equation is 3. Signup and view all the answers

Explain the concept of colligative properties and give two examples of colligative properties.

Colligative properties are properties of solutions that depend only on the number of solute particles present, not on their identity. Two examples of colligative properties are freezing point depression and boiling point elevation. Signup and view all the answers

What is the difference between a strong electrolyte and a weak electrolyte? Give an example of each.

A strong electrolyte is a substance that dissociates completely into ions when dissolved in water, while a weak electrolyte only partially dissociates. A strong electrolyte example is NaCl (sodium chloride), while a weak electrolyte example is CH3COOH (acetic acid). Signup and view all the answers

Explain the concept of reaction rate and how it is measured.

Reaction rate is the change in concentration of a reactant or product over time. It is measured by monitoring the change in concentration of a species over a specific time interval. Signup and view all the answers

Describe the factors that affect the rate of a chemical reaction. Give an example for each factor.

Several factors affect the rate of a chemical reaction, including: <ol> <li>Concentration: Increasing the concentration of reactants increases the frequency of collisions, thus increasing the rate. Example: Burning wood burns faster in pure oxygen than in air.</li> <li>Temperature: Increasing temperature increases the kinetic energy of molecules, leading to more collisions and a higher rate. Example: Food spoils faster at room temperature than in a refrigerator.</li> <li>Surface area: For reactions involving solids, increasing the surface area exposes more reactant molecules, promoting faster reactions. Example: Powdered sugar dissolves faster than sugar cubes.</li> <li>Catalyst: A catalyst speeds up the reaction without being consumed, by providing an alternative reaction pathway with lower activation energy. Example: Enzymes in biological systems catalyze reactions.</li> </ol> Signup and view all the answers

What is the molarity of a solution that is prepared by dissolving 15.0 grams of Na3PO4 in enough water to make 250.0 mL of solution?

0.366 M Signup and view all the answers

If 0.550 grams of Mg(NO3)2 are dissolved in 250.0 mL of water, what is the molarity of the solution?

0.0164 M Signup and view all the answers

What is the molarity of a solution prepared by dissolving 22.5 g of LiClO4 • 3H2O in 125 mL of water?

1.23 M Signup and view all the answers

What is the molarity of a solution prepared by diluting 30.0 mL of 3.60 M HNO3 solution to 0.250 L?

0.432 M Signup and view all the answers

Calculate the molarity of a solution prepared by dissolving 35.1 grams of Al2(SO4)3 in 0.250 L of solution?

0.332 M Signup and view all the answers

What is the molarity of a solution prepared by dissolving 27.9 g of Mn(NO3)2 • 2H2O in 175 mL of solution?

0.860 M Signup and view all the answers

A solution is prepared by diluting 31.0 mL of 5.01 M H2SO4 to 0.500 L. What is the molarity of the diluted solution?

0.311 M Signup and view all the answers

Explain why the solubility of gases in water increases as the temperature decreases.

As the temperature decreases, the kinetic energy of the gas molecules decreases and the gas molecules are less likely to escape from the solution. This makes the gas more soluble in water. Signup and view all the answers

Flashcards

Solid State of Matter

A characteristic property of solids is that they retain their own volume and shape.

Intermolecular vs Intramolecular

Intramolecular interactions are generally stronger than intermolecular interactions.