Chemistry Exam Preparation Quiz
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Questions and Answers

What must be verified before starting the exam?

  • Check that all items are placed out of sight
  • Confirm your identification number is written down
  • Ensure the Form number on your Scantron matches the exam packet (correct)
  • Make sure you have a scientific calculator at your desk

What could happen if a student possesses unauthorized materials during the exam?

  • The materials will be confiscated but the exam will continue
  • The student may receive a warning
  • The student will receive a grade of 0 and face additional academic consequences (correct)
  • The student will earn a passing grade for the exam

What should you do if you notice missing pages in the exam packet?

  • Request a new copy of the exam immediately (correct)
  • Ask fellow students if they have the same issue
  • Ignore it and continue with the exam
  • Complete the exam and inform the instructor after

When is the deadline for submitting Scantron forms?

<p>9:35 pm (C)</p> Signup and view all the answers

What is required in order to verify your identity during the exam?

<p>A student ID must be shown (D)</p> Signup and view all the answers

What is the correct empirical formula for the compound of bromine and fluorine that contains 58.37 mass percent bromine?

<p>BrF3 (B)</p> Signup and view all the answers

Which pair of elements represents the correct atomic symbols in the context presented?

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

What is the molecular weight of nitrobenzene (C6 H5 NO2) in amu?

<p>107.11 (D)</p> Signup and view all the answers

How is the following data from a measurement considered? 23.96 g, 24.01 g, 23.98 g, 23.97 g.

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

What is the density of a wooden object with a mass of 10.782 g and a volume of 13.72 mL, determined to the appropriate significant figures?

<p>7.86 × 10^-1 g/mL (A)</p> Signup and view all the answers

What is the proper form of the result of $(4.980 - 1.8621) \times 2.5630$?

<p>7.991 (C)</p> Signup and view all the answers

In combustion analysis of C6 H12O6, what can be inferred about the mass of H2O produced if 0.600 g of glucose is analyzed?

<p>It will produce an amount of water based on stoichiometric calculations. (B)</p> Signup and view all the answers

Which of the following best describes the significance of significant figures in a measurement of 15.00 cm?

<p>All digits including the trailing zeros are significant. (C)</p> Signup and view all the answers

Which formula/name pair is incorrect?

<p>Mg3N2 magnesium nitrite (B)</p> Signup and view all the answers

Which of the following samples contains the greatest number of atoms?

<p>150 g of NaCl (A)</p> Signup and view all the answers

Which equation represents the relationship between heat, mass, specific heat capacity, and change in temperature?

<p>q = m \cdot C \cdot (T_f - T_i) (C)</p> Signup and view all the answers

What is the formula for calculating the enthalpy change of a reaction?

<p>ΔH°rxn = {SΔH°f (products) - SΔH°f (reactants)} (C)</p> Signup and view all the answers

Which of the following statements about isotopes is true?

<p>Isotopes have the same number of protons but different numbers of neutrons. (B)</p> Signup and view all the answers

In thermodynamics, what is the relationship between the work done on a system and its internal energy?

<p>W = -ΔU (C)</p> Signup and view all the answers

For a given reaction, how is the change in enthalpy (ΔH°rxn) defined?

<p>The sum of the enthalpy of products minus the sum of the enthalpy of reactants. (C)</p> Signup and view all the answers

What is the relationship between Celsius and Fahrenheit temperature scales?

<p>TF = (9/5)TC + 32 (A)</p> Signup and view all the answers

Which of the following conversion factors correctly converts liters to quarts?

<p>1 L = 1.056710 qt (D)</p> Signup and view all the answers

What is the standard molar gas constant (R) expressed in J K-1 mol-1?

<p>8.314 (D)</p> Signup and view all the answers

What is the enthalpy of vaporization (DHvap) for water?

<p>40.68 kJ/mol (A)</p> Signup and view all the answers

Which equation describes the change in internal energy (DE) of a system?

<p>DE = q + w (A)</p> Signup and view all the answers

What is the value of the electron charge in coulombs?

<p>1.602 x 10–19 C (C)</p> Signup and view all the answers

Which of the following correctly calculates the pressure in atmospheres (atm) when given in kilopascals (kPa)?

<p>1 atm = 101.325 kPa (B)</p> Signup and view all the answers

What is the density of water at standard conditions?

<p>1.00 g/mL (B)</p> Signup and view all the answers

What is the conversion for kilometers to miles?

<p>1 km = 0.62137 miles (D)</p> Signup and view all the answers

Which of the following is the correct formula to convert Celsius to Kelvin?

<p>TK = TC + 273.15 (D)</p> Signup and view all the answers

What is the correct mass percentage of hydrogen in a mixture of 1 mole of C2H6 and 1 mole of NH3?

<p>37.6% (A)</p> Signup and view all the answers

How many moles are contained in 47.51 g of aluminum oxide (Al2O3)?

<p>1.105 mol (D)</p> Signup and view all the answers

What is the empirical formula for a compound that produces 4.171 g of CO2 and 2.268 g of H2O upon combustion?

<p>C2H5O2 (C)</p> Signup and view all the answers

How many significant figures should be retained in the result of 12.00000 × 0.9893 + 13.00335 × 0.0107?

<p>4 (B)</p> Signup and view all the answers

Which of the following pairs of compounds do not share the same empirical formula?

<p>C2H4O2, C6H12O6 (D)</p> Signup and view all the answers

Which of the following expresses 550 milligrams in kilograms?

<p>5.5 × 10–4 kg (C)</p> Signup and view all the answers

What is the correct name for HNO2?

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

How many moles of oxygen atoms are contained in one million molecules of oxygen gas (O2)?

<p>6.0 × 10^23 (D)</p> Signup and view all the answers

Which of the following compounds contains the highest number of anions per mole?

<p>1 mol of Na3P (A)</p> Signup and view all the answers

Calculate the percentage by mass of oxygen in Pb(NO3)2.

<p>29.0% (A)</p> Signup and view all the answers

How many protons, neutrons, and electrons are present in 238U+5?

<p>92, 146, 87 (B)</p> Signup and view all the answers

Which of the following molecular formulas represents the carbohydrate described (40.0% C, 6.71% H, 53.3% O)?

<p>C5H10O5 (D)</p> Signup and view all the answers

Which of the following options states the average atomic mass of element X with the isotopes given?

<p>220.4 amu (D)</p> Signup and view all the answers

What is the percent composition of carbon by mass in sucrose (C12H22O11)?

<p>26.7% (D)</p> Signup and view all the answers

Which of the following substances has the smallest number of protons?

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

Flashcards

Identification Number

A unique identifier for each student, required for grading.

Matching Form Numbers

The form number on your exam must match the form number on your scantron.

Scantron submission deadline

The sheet where you bubble in your answers should be submitted by 9:35 pm

Scientific calculator

A fundamental tool for performing calculations in chemistry.

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Consequences of Cheating

Using unauthorized materials during the exam will result in a grade of 0 on the the exam, a report to Academic Judiciary, and possibly failing the course.

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Sig Figs in Multiplication/Division

The number of significant figures should match the least precise measurement when multiplying or dividing numbers.

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Naming Ionic Compounds (with polyatomic ions)

A chemical formula containing a metal and a polyatomic ion. Metal name comes first, followed by the polyatomic ion name.

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Isotopes

Atoms of the same element with different numbers of neutrons, thus different mass numbers.

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Molar Mass

The actual mass of a substance, found by adding up all of the individual atomic masses in the formula.

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Enthalpy Change (ΔH)

The heat released or absorbed in a chemical reaction at constant pressure (H). A negative value indicates an exothermic reaction.

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Calculating ΔH°rxn

The sum of enthalpy of formation of products minus the sum of enthalpy of formation of reactants. Use the values from each compound.

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Heat equation

The amount of heat required to raise the temperature of 'm' grams of a substance by 'ΔT' degrees using specific heat capacity 'Cs'

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Empirical Formula

The simplest ratio of atoms in a compound.

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RMS speed (root-mean-square)

The average speed of gas particles increases with the square root of Kelvin temperature and decreases with the square root of molar mass.

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Significant Figures

The number of digits that carry meaning regarding the precision of a measurement.

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Accuracy

How close a measurement is to the true value.

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Precision

How close multiple measurements are to each other.

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Systematic Error

Errors that bias measurements in a particular direction.

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Molecular Weight

The sum of atomic masses in a molecule.

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Density

Mass per unit volume, often in g/mL or g/cm3.

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Homogeneous mixture

A mixture where the composition is uniform throughout.

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Atomic Number

The number of protons in an atom's nucleus.

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Mass Number

The total number of protons and neutrons in an atom's nucleus.

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Ion

An atom or molecule with a net electrical charge.

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Average Atomic Mass

The mass-weighted average of all isotopes of an element.

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Element

Substance made of only one type of atom, cannot be chemically broken down further.

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Mass Percent

Percent by mass of an element in a compound.

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Specific Heat Capacity

The amount of energy needed to raise the temperature of 1 gram of a substance by 1 degree Celsius (or 1 Kelvin).

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ΔHfus (Enthalpy of Fusion)

The energy required to change a substance from a solid to a liquid at its melting point.

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ΔHvap (Enthalpy of Vaporization)

The energy required to change a substance from a liquid to a gas at its boiling point.

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Temperature

A measure of the average kinetic energy of the particles in a substance.

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Pascal (Pa)

The standard unit of pressure, defined as force per unit area.

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Avogadro's Number (N_A)

The number of particles in a mole of a substance (approximately 6.022 x 10^23).

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Enthalpy (ΔH)

The amount of energy released or absorbed during a chemical or physical process. Positive for endothermic, negative for exothermic

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Ideal Gas Law (PV = nRT)

The relationship between pressure, volume, temperature, and number of moles of a gas.

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Partial Pressure

The partial pressure of a gas is the pressure it would exert if it occupied the container alone

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Planck's Constant (h)

A constant that relates the energy of a photon to its frequency.

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Moles calculation

Amount of substance (in moles) of a compound. To find it, divide mass by molar mass.

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Same Empirical Formula

Compounds with the same ratio of atoms, but not necessarily the same molecular structure.

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Mole of atoms

The basic unit of matter with a neutral electrical charge, the number of them times the atomic is equal to the moles of each molecule or compound.

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Scientific Notation

A number written in scientific notation (e.g. 3.32 × 10-18); this number would represent 0.0000000000000000032 using decimal notation.

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Study Notes

Exam Instructions

  • Do not open the exam until told to do so.
  • Place your ID, pencils, erasers, and calculator on your desk.
  • Place all other items out of sight.
  • Verify the form number on the Scantron and exam packet match.
  • Write your last name, first name, and ID number on the Scantron.
  • Write "CHE 131" under Course Name.
  • Submit all Scantrons by 9:35 pm.
  • Record all answers on the Scantron and in the exam packet.
  • Check that all exam pages (including the Periodic Table and conversions) are present.
  • Show your ID and sign in on the attendance sheet.

General Chemistry Policies

  • Possession of cell phones, digital devices, or unauthorized materials results in a grade of 0, a report to Academic Judiciary, and a possible F for the course.
  • If you do not have an ID to verify your identity, see Dr. Ivarson the day after the exam and show a valid ID.

Conversion Factors, Constants, and Equations (Page 3)

  • Includes conversion factors for mass, temperature, length, and volume.
  • Provides physical and chemical constants (e.g., electron mass, Avogadro's number, gas constant).
  • Lists equations for energy, heat, and pressure.
  • Provides values for standard thermodynamic conditions (e.g., STP).

Periodic Table (Page 4)

  • Contains a standard periodic table, including atomic number, symbol, and atomic weight for all elements.

Multiple Choice Questions (Page 5)

  • Exam-style questions assessing understanding of fundamental concepts like formula, stoichiometry, and basic chemistry calculations (empirical formula).
  • Covers topics such as chemical quantities, isotopes, conversions, and dimensional analysis.

Additional Questions (Pages 6-7)

  • Additional chemistry questions, providing further practice on concepts including data analysis, significant figures, molecular weight problems, formula determination, and others.
  • Covers topics like mass percentage, chemical calculations, and identification of elements with their properties.

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CHE 131 Exam 1 Fall 2024 PDF

Description

Test your knowledge on essential exam protocols and chemical calculations with this quiz. Topics include verification procedures, handling unauthorized materials, and empirical formulas. This quiz also covers specific chemical concepts such as molecular weight and density calculations.

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