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Questions and Answers
What is the term for the mass of one mole of a substance, expressed in grams per mole?
What is the term for the mass of one mole of a substance, expressed in grams per mole?
- Atomic mass
- Molar mass (correct)
- Molecular mass
- Formula mass
How many particles are there in one mole of any substance?
How many particles are there in one mole of any substance?
- 1.0 x 10^24
- 1.0 x 10^23
- 6.02 x 10^23 (correct)
- 12.04 x 10^23
Which of these elements exist as diatomic molecules in nature?
Which of these elements exist as diatomic molecules in nature?
- Phosphorus (P)
- Chlorine (Cl) (correct)
- Sodium (Na)
- Sulfur (S)
If you have 2 moles of water (H₂O), how many hydrogen atoms do you have?
If you have 2 moles of water (H₂O), how many hydrogen atoms do you have?
What type of mass is used for ionic compounds in the context of molar masses?
What type of mass is used for ionic compounds in the context of molar masses?
If you have a sample of 127.0 grams of copper, approximately how many moles of copper are present? (molar mass of copper is 63.5 g/mol)
If you have a sample of 127.0 grams of copper, approximately how many moles of copper are present? (molar mass of copper is 63.5 g/mol)
How many total atoms are present in a single molecule of sucrose (C₁₂H₂₂O₁₁)?
How many total atoms are present in a single molecule of sucrose (C₁₂H₂₂O₁₁)?
If you have 150.0g of H2O, and know its molar mass to be 18.0g/mol, what are the approximate number of moles of H2O?
If you have 150.0g of H2O, and know its molar mass to be 18.0g/mol, what are the approximate number of moles of H2O?
A compound is found to contain 0.900 g of calcium and 1.600 g of chlorine. What is its empirical formula?
A compound is found to contain 0.900 g of calcium and 1.600 g of chlorine. What is its empirical formula?
An iron oxide is found to be 78% iron. What is its empirical formula?
An iron oxide is found to be 78% iron. What is its empirical formula?
How many grams of $C_{12}H_{22}O_{11}$ are present in 1 mole?
How many grams of $C_{12}H_{22}O_{11}$ are present in 1 mole?
For a compound with the empirical formula CH and a molecular mass of 78 g/mol, what is its molecular formula?
For a compound with the empirical formula CH and a molecular mass of 78 g/mol, what is its molecular formula?
A compound contains 42.5 g of palladium and 0.80 g of hydrogen. The molar mass of the compound is 216.8 g/mol. Determine the molecular formula.
A compound contains 42.5 g of palladium and 0.80 g of hydrogen. The molar mass of the compound is 216.8 g/mol. Determine the molecular formula.
According to Avogadro's Law, what happens to the volume of a gas if the amount of gas increases at constant temperature and pressure?
According to Avogadro's Law, what happens to the volume of a gas if the amount of gas increases at constant temperature and pressure?
What is the volume occupied by one mole of any gas at Standard Temperature and Pressure (STP)?
What is the volume occupied by one mole of any gas at Standard Temperature and Pressure (STP)?
What is the percent concentration by mass of a solution containing 25 g of solute in 225 g of solution?
What is the percent concentration by mass of a solution containing 25 g of solute in 225 g of solution?
Which of the following variables is NOT directly used in the Ideal Gas Law equation?
Which of the following variables is NOT directly used in the Ideal Gas Law equation?
What is the molarity of a solution when 37 g of NaCl are dissolved in 150 mL of solution?
What is the molarity of a solution when 37 g of NaCl are dissolved in 150 mL of solution?
Which of the following statements regarding the molar volume of gases is correct?
Which of the following statements regarding the molar volume of gases is correct?
How many moles of HCl are present in 145 mL of a 2.25 M HCl solution?
How many moles of HCl are present in 145 mL of a 2.25 M HCl solution?
What is the molality of a solution that contains 8.50 g of calcium nitrate in 125 g of water?
What is the molality of a solution that contains 8.50 g of calcium nitrate in 125 g of water?
Which of the following correctly describes the relationship between the number of gas particles and pressure inside a container at a constant temperature and volume?
Which of the following correctly describes the relationship between the number of gas particles and pressure inside a container at a constant temperature and volume?
1 molecule of $C_{12}H_{22}O_{11}$ contains how many oxygen atoms?
1 molecule of $C_{12}H_{22}O_{11}$ contains how many oxygen atoms?
What does the 'n' represent in the Ideal Gas Law equation, $PV = nRT$?
What does the 'n' represent in the Ideal Gas Law equation, $PV = nRT$?
Flashcards
Mole
Mole
A unit that represents 6.02 x 10^23 particles.
Mole
Mole
A unit representing 6.02x10²³ particles of a substance.
Molar Mass
Molar Mass
The mass of one mole of a substance in grams per mole (g/mol).
1 mole of C12H22O11
1 mole of C12H22O11
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Molar Volume at STP
Molar Volume at STP
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Formula Unit
Formula Unit
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Avogadro’s Law
Avogadro’s Law
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Atomic Mass Unit (amu)
Atomic Mass Unit (amu)
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Conversions: Moles to Grams
Conversions: Moles to Grams
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Ideal Gas Law
Ideal Gas Law
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Conversions: Moles to Atoms
Conversions: Moles to Atoms
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Empirical Formula
Empirical Formula
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Gas pressure relation
Gas pressure relation
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1 Mole = Mass (g) from PT
1 Mole = Mass (g) from PT
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Calculating gas volume
Calculating gas volume
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Molecular Mass
Molecular Mass
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Molecular Formula
Molecular Formula
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Molarity (M)
Molarity (M)
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Molality (m)
Molality (m)
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Percent Concentration by Mass
Percent Concentration by Mass
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Solute
Solute
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Solution
Solution
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Study Notes
The Mole
- A mole is a unit of measurement in chemistry, representing 6.02 x 1023 particles (atoms, formula units, or molecules).
- One mole of a substance equals its mass in grams, as determined from the periodic table (PT).
Getting to Know the Terms
- Microscopic Mass: Atomic mass (amu) for atoms, molecular mass (amu) for molecules, and formula mass (amu) for ionic compounds.
- Macroscopic Mass: Molar mass (g/mol) for elements, molecular compounds, and ionic compounds.
- Key elements existing as molecules in nature are H2, O2, F2, Br2, I2, N2, Cl2, S8, and P4
Mole Relationships
- 1 mole = 6.02 x 1023 particles (atoms, formula units, or molecules).
- 1 mole = mass (grams) of the substance from the PT.
- 1 molecule = number of atoms.
- 1 formula unit = number of ions or atoms.
Mole Conversions
- Calculations between moles, mass, and numbers of particles require the use of factor labels.
- Conversions must account for the number of atoms/ions in a molecule/formula unit.
Avogadro's Law
- Equal volumes of gases at the same temperature and pressure contain an equal number of particles.
- One mole of any gas occupies 22.4 L at standard temperature and pressure (STP).
Molar Mass
- The molar mass of a substance is the mass of one mole of that substance, measured in grams.
- Molar mass does not affect the volume of a gas at constant pressure, temperature and quantity of moles.
Ideal Gas Law
- Ideal gas law describes the relationship between pressure, volume, number of moles, and temperature of a gas.
- The ideal gas law equation is PV = nRT.
Empirical Formulas
- Empirical formulas represent the smallest whole-number ratio of atoms in a compound.
- Determination of these formulas involves using experimental data, typically mass percentages.
Molecular Formulas
- Molecular formulas show the actual number of atoms of each element in a molecule.
- Molecular formula is a multiple of the empirical formula.
- The molecular formula can be calculated given the empirical formula and molar mass.
Concentration
- Percent concentration by mass = (solute/solution) x 100%
- Molarity (M) = moles of solute / liters of solution (mol/L)
- Molality (m) = moles of solute / mass of solvent (kg) (mol/kg)
Molarity or Concentration Calculations and Problems
- Standard solutions can be prepared via exact calculation and standardized instruments.
- Calculations of molarity and dilution require the use of proper formulas and unit conversions.
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