Honors Chemistry Unit 7 Review
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Questions and Answers

Which of the following has the greatest number of atoms? a. 26.98 g of Al b. 1 mole of S c. 5 moles of O2 d. 18.02 g H2O e. All are the same

  • 26.98 g of Al
  • 5 moles of O2 (correct)
  • 1 mole of S
  • 18.02 g H2O
  • All are the same

Calculate the molar mass of manganese (IV) oxalate.

206.11 g/mol

How many moles are in 53.0 g of CH4?

3.30 moles

What is the mass of 6.9x10^25 molecules of NO?

<p>1,227.48 g</p> Signup and view all the answers

Which of the following iron compounds contains the greatest percentage of iron: pyrite (FeS2), hematite (Fe2O3), or siderite (FeCO3)?

<p>Hematite (Fe2O3) (C)</p> Signup and view all the answers

Determine the percent composition of Ca(NO3)2.

<p>20.04% Ca, 61.25% N, 18.71% O</p> Signup and view all the answers

A fluoride of aluminum is 67.87% F. What is the formula of this compound?

<p>AlF3</p> Signup and view all the answers

The empirical formula of C2H5OH is __________.

<p>CH3</p> Signup and view all the answers

The empirical formula of C6H12O6 is __________.

<p>CH2O</p> Signup and view all the answers

What is the empirical formula for a compound that is 40.00% C, 6.713% H and 53.28% O by mass?

<p>C3H6O</p> Signup and view all the answers

If the molecular mass of a compound is 60.052 g, what is its molecular formula if the empirical formula is C3H6O?

<p>C6H12O2</p> Signup and view all the answers

What is the limiting reactant if 14.0 g N2 is mixed with 9.0 g H2?

<p>H2</p> Signup and view all the answers

How much excess reactant is left over after the reaction?

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

What is the theoretical yield of NH3?

<p>16.8 g</p> Signup and view all the answers

What is the percent yield if 16.1 g of NH3 actually forms?

<p>96.9%</p> Signup and view all the answers

What is collision theory?

<p>A theory stating that for a reaction to occur, reactants must collide with sufficient energy and proper orientation.</p> Signup and view all the answers

What are the requirements for a successful collision?

<p>Sufficient energy and proper orientation.</p> Signup and view all the answers

How would increasing the temperature affect the rate of a reaction?

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

At equilibrium, the amount of products must equal the amount of reactants.

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

During equilibrium, the concentration of the products does not change.

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

A collision between reactants is all that is needed to cause a reaction.

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

If K > 1, __________ are favored.

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

If K < 1, ______________ are favored.

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

What are the definitions for acids & bases?

<p>Acid: A substance that donates protons; Base: A substance that accepts protons.</p> Signup and view all the answers

What is meant by the term amphiprotic?

<p>A substance that can both donate and accept protons.</p> Signup and view all the answers

What is specific heat capacity?

<p>The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.</p> Signup and view all the answers

Calculate the pH of a solution with [H+] = 0.00100 M.

<p>3.00</p> Signup and view all the answers

What is an indicator and what is it used for?

<p>An indicator is a substance that changes color at a particular pH level, used to determine acidity or alkalinity.</p> Signup and view all the answers

Flashcards

Mole concept

A mole is a quantity of a substance containing 6.022 x 10^23 particles (atoms, molecules, or ions).

Molar mass

The mass of one mole of a substance in grams.

Percent composition

The percentage by mass of each element in a compound.

Empirical formula

Simplest whole-number ratio of atoms in a compound.

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Molecular formula

Actual number of atoms of each element in a molecule.

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Chemical equation

A representation of a chemical reaction using symbols and formulas.

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Balancing equations

Adjusting coefficients to equalize the number of atoms of each element on both sides.

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Stoichiometry

Calculations relating amounts of reactants and products in a chemical reaction.

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Limiting reactant

Reactant that is completely used up in a reaction.

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Excess reactant

Reactant left over after the reaction is complete.

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Theoretical yield

Maximum amount of product that can be obtained from a reaction.

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Percent yield

Ratio of actual yield to theoretical yield expressed as a percentage.

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Saturated solution

A solution containing the maximum amount of solute that can dissolve at a given temperature.

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Unsaturated solution

A solution that can dissolve more solute at a given temperature.

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Solubility

The ability of a substance (solute) to dissolve in a solvent.

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Net ionic equation

Equation showing only the ions involved in a reaction.

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Molarity

The concentration of a solution expressed as moles of solute per liter of solution.

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Equilibrium

A state where the rates of forward and reverse reactions are equal, and there are no net changes.

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Equilibrium constant (K)

A numerical value that describes the ratio of product to reactant concentrations at equilibrium.

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Le Chatelier's principle

If a stress is applied to a system at equilibrium, the system shifts to relieve the stress and re-establish equilibrium.

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Arrhenius acid

Substance that produces H+ ions in water.

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Bronsted-Lowry acid

Proton donor.

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Exothermic reaction

A reaction that releases heat to the surroundings.

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Endothermic reaction

A reaction that absorbs heat from the surroundings.

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Specific heat capacity

The energy required to raise the temperature of 1 gram of a substance by 1°C.

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Calorimetry

Measuring the heat transfer during a chemical or physical process.

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Study Notes

Unit 7 – The Mole

  • Understand the mole concept for estimating quantities in reactions.
  • Calculate molar mass from chemical formulas and names.
  • Convert between particles, mass, and volume in chemical calculations.
  • Determine percent composition for compounds based on element mass.
  • Identify empirical and molecular formulas from composition data.

Unit 8 – Balancing Equations and Stoichiometry

  • Recognize types of chemical reactions.
  • Balance chemical equations using stoichiometric coefficients.
  • Derive chemical equations from word problems.
  • Use balanced equations for reactant/product ratios.
  • Convert between grams, particles, and liters during reactions.
  • Identify the limiting reactant and calculate excess reactant and theoretical yield.
  • Determine percent yield based on actual and theoretical yield.

Unit 9 – Reactions and Solutions

  • Differentiate between saturated, unsaturated, and supersaturated solutions.
  • Explain solubility concepts at both macroscopic and particle levels.
  • Use solubility rules to assess the solubility of ionic compounds.
  • Write solvation equations showing the dissociation of soluble ionic compounds.
  • Construct and interpret molecular, complete ionic, and net ionic equations.
  • Solve concentration problems using molarity and dilution equations.

Unit 10 – Equilibrium

  • Identify factors affecting reaction rates.
  • Explain how equilibrium is achieved in reversible reactions.
  • Write equilibrium constant expressions and calculate K values from reactions.
  • Analyze reaction extent through K value magnitudes.
  • Apply ICE tables for calculating equilibrium concentrations.
  • Utilize LeChatelier’s principle for predicting shifts in equilibrium.

Unit 11 – Acids and Bases

  • Define acids and bases using Arrhenius and Bronsted-Lowry theories.
  • Identify conjugate acid-base pairs in reactions.
  • Recognize key physical and chemical properties of acids and bases.
  • Calculate H⁺ and OH⁻ concentrations using Kw relationships.
  • Describe and compute pH values for acidic and basic solutions.
  • Explain acid-base reactions, including titrations and stoichiometric calculations.

Unit 12 – Thermochemistry

  • Distinguish between exothermic and endothermic reactions based on enthalpy.
  • Draw energy diagrams highlighting ΔH and activation energy.
  • Understand the impact of specific heat capacity on thermal properties.
  • Perform calculations with the specific heat formula.
  • Use calorimetry to determine energy changes in reactions and apply Hess’s Law for ΔH calculations.

Important Concepts and Example Calculations

  • Molar mass of compounds, percentage composition calculations.
  • Limiting reactant identification in stoichiometric equations.
  • Equilibrium constant calculations and Q comparisons to predict shifts.
  • Capitalize on the relationship between pH, [H⁺], and [OH⁻] in aqueous solutions.
  • Use reaction enthalpy to calculate energy changes in chemical processes.

Noteworthy Questions

  • Key problem-solving questions regarding mole conversions, balancing equations, and equilibrium states.
  • Practical applications of acid-base neutralization, as well as calorimetry for energy calculations.
  • Significant equations for solubility predictions, including molecular forms and precipitation reactions.

Tips for Exam Preparation

  • Practice calculations involving molar mass and concentration.
  • Engage in problems that require balancing equations and deriving net ionic equations.
  • Familiarize with equilibrium concepts and the significance of K and Q values.
  • Utilize sample acidic and basic titration problems for proficiency in pH calculations.

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LTHS Chemistry Honors Chemistry 2023-2024 Second Semester Exam Review PDF

Description

Prepare for the second semester exam in Honors Chemistry with this quiz focused on Unit 7: The Mole. Test your understanding of mole concepts, molar mass calculations, and conversions between particles, mass, and volume. Make sure you can also determine percent composition from formulas.

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