Chemistry Quiz: Molecular Formulas and Reactions
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Questions and Answers

What is the unit for density when using the equation d = mass/volume?

  • kg/km
  • g/mL (correct)
  • cm^3
  • m^2

    • What is the theoretical percent composition of hydrogen in CH4?

  • 12.5%
  • 25%
  • 50%
  • 75% (correct)

    • Which step is NOT part of determining a molecular formula from an empirical formula?

  • Subtracting empirical mass from molar mass (correct)
  • Calculating the mass from the empirical formula
  • Calculating the ratio of molar mass to empirical mass
  • Determining the empirical formula

    • Given an empirical formula of C2H8N and a molar mass of 46.0 g/mol, what is the molecular formula of the compound?

    <p>C4H16N2</p> Signup and view all the answers

    To find the average atomic mass, which of the following factors must be considered?

    <p>Mass of isotopic elements and their percent abundances</p> Signup and view all the answers

    What is the empirical formula for a compound containing 88.8% copper and 11.2% oxygen?

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

    If you have 0.688 mol of CO2, how many grams do you have given the molar mass of CO2 is 44.01 g/mol?

    <p>30.3 g</p> Signup and view all the answers

    Which formula represents a correct method for calculating percent composition?

    <p>Percent = mass of element / total mass x 100%</p> Signup and view all the answers

    What are the products formed when solid lithium hydroxide reacts with gaseous carbon dioxide?

    <p>Li2CO3 and H2O</p> Signup and view all the answers

    In the reaction 2LiOH(s) + CO2(g) → Li2CO3(s) + H2O(l), which is the correct stoichiometric ratio of LiOH to CO2?

    <p>2:1</p> Signup and view all the answers

    Which step in the student's work calculating mass of CO2 from LiOH is incorrect?

    <p>Incorrect conversion factor between moles of products</p> Signup and view all the answers

    What is the limiting reactant when 2.40 g of Mg reacts with 10.0 g of O2 in the reaction Mg + O2 → MgO?

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

    How many moles of FeCl3 can be produced from 2.30 g of Fe in the reaction 2 Fe + 3 Cl2 → 2FeCl3?

    <p>0.04625 moles</p> Signup and view all the answers

    What is the percent yield of FeCl3 if the actual yield is 5.22 g and the theoretical yield is calculated using the limiting reactant?

    <p>85.4%</p> Signup and view all the answers

    Which of the following compounds can be named as FeCl3?

    <p>Ferric chloride</p> Signup and view all the answers

    What is the theoretical yield of MgO if 2.40 g of Mg is fully reacted?

    <p>3.98 g MgO</p> Signup and view all the answers

    What is the mass number of Carbon-13?

    <p>13</p> Signup and view all the answers

    Which of the following is an example of a physical property?

    <p>Melting point</p> Signup and view all the answers

    How many neutrons are in a Nitrogen isotope with a mass number of 14?

    <p>8</p> Signup and view all the answers

    Which part of the periodic table primarily forms negative ions?

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

    What type of mixture is sugar dissolved in water?

    <p>Homogeneous mixture</p> Signup and view all the answers

    What is a characteristic of a strong electrolyte?

    <p>Fully dissociates into ions in solution</p> Signup and view all the answers

    Which equation shows the dissociation of sodium carbonate in water?

    <p>Na2CO3(aq) → 2Na^+ + CO3^{2-}</p> Signup and view all the answers

    Which of the following best defines a compound?

    <p>A combination of two or more elements in fixed proportions</p> Signup and view all the answers

    What is the correct balanced equation for the reaction of phosphoric acid with potassium hydroxide?

    <p>1 H3PO4 + 3 KOH → 1 K3PO4 + 3 H2O</p> Signup and view all the answers

    In the reaction 2 K3PO4 (aq) + 3 BaCl2 (aq) → Ba3(PO4)2 (s) + 6 KCl (aq), what type of reaction is occurring?

    <p>Double-replacement</p> Signup and view all the answers

    Which of the following best describes the reaction type for 1 C5H12 (g) + 8 O2 (g) → CO2 (g) + H2O (g) + heat?

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

    In the equation NaOH(aq) + Fe(NO3)3(aq) → NaNO3(aq) + Fe(OH)3(s), which is the net ionic equation?

    <p>OH- + Fe3+ → Fe(OH)3</p> Signup and view all the answers

    What is the conjugate base of HOCN in the reaction HOCN(aq) + H2O(l) ⇌ OCN- (aq) + H3O+(aq)?

    <p>OCN-</p> Signup and view all the answers

    Which of the following represents a strong electrolyte?

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

    What is the oxidation number of sulfur in SO3?

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

    In the reaction 2 Al(OH)3 (aq) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 6 H2O (ℓ), which product is formed by a double-replacement reaction?

    <p>Al2(SO4)3</p> Signup and view all the answers

    What is the correct formula for copper(II) chloride?

    <p>CuCl2</p> Signup and view all the answers

    Which of the following is a covalent compound?

    <p>CO2</p> Signup and view all the answers

    What is the formula for barium hydroxide octahydrate?

    <p>Ba(OH)2 8H2O</p> Signup and view all the answers

    Identify the correct name for H2SO4.

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

    Which of the following correctly represents carbonic acid?

    <p>H2CO3</p> Signup and view all the answers

    What is the empirical formula for ammonium carbonate?

    <p>NH4CO3</p> Signup and view all the answers

    Which isotope symbol represents a carbon atom with 6 protons and 8 neutrons?

    <p>14C</p> Signup and view all the answers

    What is the formula for sulfur hexafluoride?

    <p>SF6</p> Signup and view all the answers

    Which statement about the energy of electromagnetic waves is true?

    <p>Visible light has higher energy than infrared light.</p> Signup and view all the answers

    What is the speed of light equation used to relate wavelength and frequency?

    <p>c = λν</p> Signup and view all the answers

    In the reaction Fe2+(aq) + Co(s) → Co2+(aq) + Fe(s), which substance acts as the reducing agent?

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

    How would you determine the number of valence electrons of an element using the periodic table?

    <p>By its position in the groups of the periodic table.</p> Signup and view all the answers

    What is a key characteristic of a wave, based on its properties?

    <p>Waves can exhibit particle-like behavior.</p> Signup and view all the answers

    In energy level diagrams, which transition indicates absorption?

    <p>Electrons moving to higher energy levels.</p> Signup and view all the answers

    What can be determined from a bright line spectrum's given wavelength, such as 518 nm?

    <p>Both frequency and energy can be determined.</p> Signup and view all the answers

    Which of the following represents an example of reduction?

    <p>Fe2+(aq) + 2e- → Fe(s)</p> Signup and view all the answers

    Study Notes

    Honors Chemistry Final Exam Study Guide

    • Determining Formula Mass and Number of Atoms/Molecules: Use Avogadro's number to convert between moles and number of atoms or molecules.
    • Average Atomic Mass: Calculate the average atomic mass of an element using the isotopic masses and percent abundances of its isotopes. The formula is average mass = Σ(fractional abundance × isotopic mass).
    • Percent Composition: Determine the percent composition of elements in a compound by calculating the percent by mass of each element, using its molar mass from the periodic table.
    • Determining Molecular Formulas: Five steps are needed to determine molecular formulas from empirical formulas.
    • Find the empirical formula.
    • Determine the mass of the empirical formula.
    • Calculate the molar mass from the molecular formula.
    • Determine the ratio of the Molar mass/Empirical mass.
    • Multiply the empirical formula subscripts by the ratio found in step 4 to find the molecular formula.
    • Empirical Formula from Percent Composition: Find the empirical formula by finding the mole ratio of the elements.
    • Molecular Formula Determine the molecular formula by comparing the molar mass to the mass of the empirical formula.
    • Density: Density is mass divided by volume. Units of density commonly include g/mL, g/cm3, kg/m3.
    • Dimensional Analysis: Convert between units such as nm to m or meters to centimeters.
    • Conversion factors: Use conversion factors to go between units, such as 1 x 10-9 m = 1 nm.
    • Limiting Reactant: Determine the limiting reactant to calculate theoretical yield of a product in a chemical reaction.
    • Chemical Reactions: Calculate the grams of the product.
    • Types of Reactions: Understand and balance various chemical reactions such as combustion, double replacement, single displacement, neutralization, decomposition, or redox reactions).
    • Naming Compounds: Ionic and covalent compounds. Be able to name various acids.
    • Writing formulas from names: Write chemical formulas of ionic and covalent compounds by balancing charges, using prefixes to indicate numbers of atoms in a covalent compound (prefixes such as mono-, di-, tri-).
    • Isotopes: Understand Isotopes and their properties. Know what an isotope is and be able to distinguish between isotopes.
    • Identifying Physical and Chemical Properties: Distinguish between physical properties and chemical properties, and give examples (density, melting point and reactivity, flammability).
    • Classifying Matter: Classify matter as elements, pure substances, molecules, compounds, homogeneous mixtures, and heterogeneous mixtures.
    • Ions: Explain how ions are formed and identify the locations of positive and negative ions on the periodic table.
    • Periodic Table Relationships: Understand the position of metals, nonmetals, gases and other groups on the periodic table and the relationships between elements in the periodic table.
    • Electrolytes: Distinguish between the types of electrolytes.
    • Chemical Equations: Properly write chemical (molecular) equations, complete ionic equations and net ionic equations. Be able to balance chemical equations.
    • Oxidation Numbers: Determine the oxidation numbers of elements in chemical formulas.
    • Electromagnetic Spectrum: Understand the electromagnetic spectrum, including energy levels, frequency and wavelength relationships.
    • Speed of Light Equation: Use the equation c = λν to calculate speed of light, wavelength, or frequency.
    • Energy Equation: Use the equation E=hv=hc/λ to calculate energy, frequency or wavelength.
    • Atomic Structure: Understand different types of atomic orbitals, valence and core electrons, and use electron configurations for atoms.
    • Periodic Trends: Understand periodic trends such as atomic radius, ionization energy, electron affinity, and electronegativity. Know the relationship between trends and the position of elements on the periodic table.
    • Experimental Techniques: Discuss accuracy, precision, significant figures, and experimental uncertainty using examples like measuring or identifying errors in measurements and calculations using experimental data).

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    Honors Chemistry Final Exam Study Guide Fall 2024 PDF

    Description

    Test your knowledge on the fundamentals of chemistry with this quiz. Topics include calculating molecular formulas, percent composition, and stoichiometric ratios. Ideal for students studying chemical reactions and empirical formulas.

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