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Questions and Answers
What is the complete ground-state electronic configuration for Selenium (Se)?
What is the complete ground-state electronic configuration for Selenium (Se)?
In the reaction 2PbS(s) + 3O2(g) → 2PbO(s) + 2SO2(g), which species acts as the oxidizing agent?
In the reaction 2PbS(s) + 3O2(g) → 2PbO(s) + 2SO2(g), which species acts as the oxidizing agent?
If a 25.0mL sample of HCl solution is neutralized by 24.16mL of 0.106M NaOH, what is the concentration of the HCl solution?
If a 25.0mL sample of HCl solution is neutralized by 24.16mL of 0.106M NaOH, what is the concentration of the HCl solution?
What is the mass of a single molecule of aspirin (C9H8O4)?
What is the mass of a single molecule of aspirin (C9H8O4)?
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What is the molar mass of C7H5(NO2)3?
What is the molar mass of C7H5(NO2)3?
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How many covalent bonds are normally formed by nitrogen (N)?
How many covalent bonds are normally formed by nitrogen (N)?
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In balancing the redox reaction Cl2(g) → Cl(aq) + ClO(aq), what is the coefficient of ClO in the balanced equation?
In balancing the redox reaction Cl2(g) → Cl(aq) + ClO(aq), what is the coefficient of ClO in the balanced equation?
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What is the number of significant figures in the value 0.000040?
What is the number of significant figures in the value 0.000040?
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What type of thermochemical reaction is represented by the equation C3H8 + 5O2 → 3CO2 + 4H2O + heat?
What type of thermochemical reaction is represented by the equation C3H8 + 5O2 → 3CO2 + 4H2O + heat?
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How many electrons can be represented by the quantum numbers n=5, M₁=0?
How many electrons can be represented by the quantum numbers n=5, M₁=0?
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What is the molarity of a solution if 4.6g of (NH4)3PO4 is dissolved in enough water to make 1.65L of solution?
What is the molarity of a solution if 4.6g of (NH4)3PO4 is dissolved in enough water to make 1.65L of solution?
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Given the reaction 3BaCl2(aq) + Fe2(SO4)3(aq) → 3BaSO4(s) + 2FeCl3(aq), what mass of BaSO4 is produced from 100mL of a 0.100M solution of barium chloride?
Given the reaction 3BaCl2(aq) + Fe2(SO4)3(aq) → 3BaSO4(s) + 2FeCl3(aq), what mass of BaSO4 is produced from 100mL of a 0.100M solution of barium chloride?
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Which sets of quantum numbers describe valid outer shell (valence) electrons for cesium (Cs)?
Which sets of quantum numbers describe valid outer shell (valence) electrons for cesium (Cs)?
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How much heat is released when 1/2 mole of liquid water cools from 100.0°C to 10.0°C?
How much heat is released when 1/2 mole of liquid water cools from 100.0°C to 10.0°C?
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Calculate the molarity of C9H8O4 if 85.0g is dissolved in 250mL of solution.
Calculate the molarity of C9H8O4 if 85.0g is dissolved in 250mL of solution.
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Which of the following compounds has polar bonds?
Which of the following compounds has polar bonds?
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Study Notes
Chemistry 111 Work Problems
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Problem 1: Convert -200 degrees Fahrenheit to Celsius and Kelvin.
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Problem 2a: Convert 831g to kg.
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Problem 2b: Convert 51.2mL to cubic centimeters (cc).
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Problem 2c: Convert 215cm to kilometers (km).
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Problem 3: Calculate the volume of 75g of uranium, given its density is 18.95g/mL.
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Problem 4a: Determine the number of significant figures in 6543.
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Problem 4b: Determine the number of significant figures in 73.0001.
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Problem 4c: Determine the number of significant figures in 0.000040.
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Problem 4d: Determine the number of significant figures in 6500.
Additional Problems (Page 2)
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Problem 5: Round the following numbers to two significant figures:
- 0.393974
- 0.087498
- 31.4
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Problem 6: Calculate the mass number of an atom with 91 protons, 88 electrons, and 140 neutrons.
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Problem 7: Determine the number of electrons, protons, and neutrons in Sr2+ with a mass number of 87.
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Problem 8: Write the complete and abbreviated electronic configuration for Selenium (Se).
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Problem 9: Identify the sublevels in the 4th energy level and find the number of orbitals in each subshell.
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Problem 10a: Determine the number of covalent bonds normally formed by chlorine (Cl).
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Problem 10b: Determine the number of covalent bonds normally formed by carbon (C).
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Problem 10c: Determine the number of covalent bonds normally formed by nitrogen (N).
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Problem 11: Identify the oxidizing agent in the reaction 2PbS(s) + 3O2(g) → 2PbO(s) + 2SO2(g).
Additional Problems (Page 3)
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Problem 12: Balance the oxidation-reduction reaction Cl₂(g) → Cl⁻(aq) + ClO⁻(aq) in a basic solution.
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Problem 13: Calculate the concentration of an HCl solution if 25.0mL of it takes 24.16mL of 0.106M NaOH for complete neutralization.
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Problem 14: Calculate the formula mass and molar mass of C₇H₅(NO₂)₃.
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Problem 15: Determine the number of moles of C₂₀H₂₄N₂O₂ in 51.6g of the compound.
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Problem 16: Calculate the number of moles of sulfur (S) atoms in 3.5 x 10³ moles of Al₂(SO₄)₃.
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Problem 17: Calculate the mass in grams of a single aspirin (C₉H₈O₄) molecule.
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Problem 18: Determine the number of water molecules in 0.0500g of water.
Additional Problems (Page 4)
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Problem 19a: Balance the equation Fe₂O₃ + CO → Fe + CO₂.
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Problem 19b: Balance the equation Al³⁺ + S²⁻ → Al₂S₃
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Problem 20a: If 2g of N₂ is reacted with excess H₂, calculate the grams of NH₃ produced.
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Problem 20b: If 3.00g of H₂ is reacted with excess N₂, calculate the grams of NH₃ produced.
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Problem 21: Determine the percentage yield if the theoretical yield of a reaction is 85.2g and the actual yield is 71.4g.
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Problem 22: Calculate the grams of vitamin C (C₆H₈O₆) in 0.731 moles of vitamin C.
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Problem 23: Determine the formal charge on each atom in CIF₅.
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Problem 24: Determine the shape and number of bonding and non-bonding electron pairs for PO₄³⁻.
Additional Problems (Page 5)
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Problem 25: Determine the electron pair shape and molecular shape of I₃⁻.
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Problem 26a: Determine the oxidation number of the underlined atom in Na₃PO₄.
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Problem 26b: Determine the oxidation number of the underlined atom in NaCl.
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Problem 26c: Determine the oxidation number of the underlined atom in H₂SO₄.
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Problem 26d: Determine the oxidation number of the underlined atoms in K₂Cr₂O₇.
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Problem 27: Calculate the molarity of C₉H₈O₄ if 85.0g dissolves in 250mL of solution.
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Problem 28: Describe the preparation of 250mL of 0.1M NaOH from solid NaOH and water.
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Problem 29a: Determine the number of electrons represented by n = 5, ml = 0.
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Problem 29b: Determine the number of electrons represented by n = 4, l = 2, ms = ½.
Additional Problems (Page 6)
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Problem 30: Calculate the grams of solute in 125mL of a 0.0036M MgCO₃ solution.
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Problem 31: Calculate the molarity of a solution made by dissolving 4.6g of (NH₄)₃PO₄ in 1.65L of water.
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Problem 32: Identify the type of thermochemical reaction represented by C₃H₈ + 5O₂ → 3CO₂ + 4H₂O + heat.
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Problem 33: Write all possible sets of quantum numbers for an outer-shell electron of Cs.
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Problem 34: Calculate the mass of BaSO₄ produced when 100mL of 0.100M BaCl₂ is mixed with excess Fe₂(SO₄)₃.
Additional Problems (Page 7)
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Problem 35: Determine the polarity of CCl₄, CH₃CH₂OH, CH₂Cl₂, and NH₃.
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Problem 36: Answer questions about the Lewis structure, electron pair shape, molecular shape, bond types, and orbital hybridization of XeF₄.
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Problem 37: Calculate the new pressure of a 3.00L sample of Ar gas at 725mmHg when the volume increases to 9.15 L, assuming constant temperature and moles.
Additional Problems (Page 8)
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Problem 38: Calculate the pressure exerted by 1.9 x 10²g of N₂ in a 2-liter gas cylinder at 22°C.
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Problem 39: Calculate the volume of H₂ produced at STP from 250.9mL of 6.0 mol/L HCl.
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Problem 40: Name the compounds CuBr, Mg₃N₂, CCl₄, and CS₂O
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Problem 41: Calculate ΔH for the process Mn(s) + O₂(s) → MnO₂(s) .
Additional Problems (Page 9)
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Problem 42: Calculate ∆H for C(s) + ½O₂(g) → CO(g) using given data.
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Problem 43: Calculate the heat given off when ½ mole of liquid water cools from 100.0°C to 10.0°C.
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Problem 44: Calculate ∆H for the dissolving of CaCl₂ in 100g of water, given the temperature change.
Additional Problems (Page 10)
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Problem 45: Calculate the amount of H₂O formed when 28.0mL of 0.250M HNO₃ and 53.0mL of 0.320M KOH are mixed.
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Problem 46: Write the net ionic equation for the reaction NaOH(aq) + FeCl₃(aq) → 3NaCl(aq) + Fe(OH)₃(s) and identify spectator ions.
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Description
This quiz covers essential work problems in Chemistry 111, focusing on conversions, significant figures, and calculations related to mass and volume. Students will apply their knowledge to convert temperature, mass, and volume as well as analyze atomic structure through various problems. Test your understanding of these fundamental concepts!
