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Questions and Answers
What is the molar mass of C6H12O6?
What is the molar mass of C6H12O6?
- 164.10 g
- 78.01 g
- 180.18 g (correct)
- 261.35 g
How would you find the percent composition of an element in a compound?
How would you find the percent composition of an element in a compound?
- Calculate the total mass of all elements in the formula.
- Divide the atomic mass of the element by the total number of atoms.
- Add the masses of all elements together.
- Divide the contribution of each element's mass by the total molar mass and multiply by 100. (correct)
What is the empirical formula of glucose (C6H12O6)?
What is the empirical formula of glucose (C6H12O6)?
- C6H12O6
- C3H6O3
- C2H4O2
- CH2O (correct)
What is the formula mass of Ca(NO3)2?
What is the formula mass of Ca(NO3)2?
Which step is NOT part of calculating the percent composition of a compound?
Which step is NOT part of calculating the percent composition of a compound?
What is the percent composition of Hydrogen in C6H12O6?
What is the percent composition of Hydrogen in C6H12O6?
How is the contribution of each element's mass calculated in a compound?
How is the contribution of each element's mass calculated in a compound?
What is the percent composition of Barium in Ba(NO3)2?
What is the percent composition of Barium in Ba(NO3)2?
What is the empirical formula of phosgene, given its composition of 12.1% C, 16.2% O, and 71.7% Cl?
What is the empirical formula of phosgene, given its composition of 12.1% C, 16.2% O, and 71.7% Cl?
In determining the molecular formula, what is the first step after calculating the empirical formula mass?
In determining the molecular formula, what is the first step after calculating the empirical formula mass?
Given a 10.150 g sample containing only P and O, with 4.433 g of P, what is the empirical formula?
Given a 10.150 g sample containing only P and O, with 4.433 g of P, what is the empirical formula?
If the empirical formula of a compound is C2H6O and its molar mass is 62 g/mol, what is the molecular formula?
If the empirical formula of a compound is C2H6O and its molar mass is 62 g/mol, what is the molecular formula?
Which of the following represents the method for calculating the empirical formula from mass percent composition?
Which of the following represents the method for calculating the empirical formula from mass percent composition?
How do you determine the number of empirical formula units in an actual molecule?
How do you determine the number of empirical formula units in an actual molecule?
Which characteristic distinguishes a molecular formula from an empirical formula?
Which characteristic distinguishes a molecular formula from an empirical formula?
What does the molecular weight of a compound signify in relation to the empirical formula weight?
What does the molecular weight of a compound signify in relation to the empirical formula weight?
What is the empirical formula for a compound composed of 79.8% copper and 20.2% sulfur?
What is the empirical formula for a compound composed of 79.8% copper and 20.2% sulfur?
Which empirical formula corresponds to a compound with 36.8% nitrogen and 63.2% oxygen?
Which empirical formula corresponds to a compound with 36.8% nitrogen and 63.2% oxygen?
For the empirical formula Na₂S₂O₃, what would be the molecular formula if its molecular weight is 270.4 g/mol?
For the empirical formula Na₂S₂O₃, what would be the molecular formula if its molecular weight is 270.4 g/mol?
Which of the following compounds has an empirical formula of C₆H₁₂O₆ based on its molecular weight of 180 g/mol?
Which of the following compounds has an empirical formula of C₆H₁₂O₆ based on its molecular weight of 180 g/mol?
Based on the law of multiple proportions, which two compounds featuring carbon can be compared for their mass ratios?
Based on the law of multiple proportions, which two compounds featuring carbon can be compared for their mass ratios?
In a sample of carbon suboxide weighing 2.500 g that contains 1.32 g of carbon and 1.18 g of oxygen, which principle is demonstrated?
In a sample of carbon suboxide weighing 2.500 g that contains 1.32 g of carbon and 1.18 g of oxygen, which principle is demonstrated?
What empirical formula corresponds to a compound with 38.9% chlorine and 61.2% oxygen?
What empirical formula corresponds to a compound with 38.9% chlorine and 61.2% oxygen?
Which of the following empirical formulas is correctly paired with its corresponding compound mass composition?
Which of the following empirical formulas is correctly paired with its corresponding compound mass composition?
Flashcards
Empirical Formula
Empirical Formula
Simplest whole number ratio of atoms in a compound.
Formula Mass
Formula Mass
The sum of the atomic masses of all atoms in a chemical formula.
Mole Ratio
Mole Ratio
Ratio of moles of elements in a compound expressed as whole numbers.
Molar Mass
Molar Mass
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Molecular Formula
Molecular Formula
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Percent Composition
Percent Composition
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Molar Mass
Molar Mass
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Empirical Formula
Empirical Formula
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Calculating Formula Mass
Calculating Formula Mass
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Empirical Formula Calculation
Empirical Formula Calculation
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Percent Composition Calculation
Percent Composition Calculation
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Calculating Moles
Calculating Moles
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Calculating Empirical Formula
Calculating Empirical Formula
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Molecular Formula Calculation
Molecular Formula Calculation
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Mass Percent Analysis
Mass Percent Analysis
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% composition equation
% composition equation
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Empirical Formula
Empirical Formula
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Molecular Formula
Molecular Formula
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Law of Multiple Proportions
Law of Multiple Proportions
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Percentage Composition
Percentage Composition
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Hydrocarbons
Hydrocarbons
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Carbon Suboxide
Carbon Suboxide
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Mass of carbon in benzene
Mass of carbon in benzene
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Mass of carbon in ethane
Mass of carbon in ethane
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Study Notes
Compounds
- A compound is a substance composed of two or more elements held together by chemical bonds.
- Elements in compounds combine in specific ratios.
- Examples: Water (H₂O), Sodium Chloride (NaCl)
Lewis Dot Symbols
- Lewis dot symbols represent atoms using their element symbol surrounded by dots.
- The dots represent valence electrons.
- Main group metals use the number of dots to indicate the number of valence electrons.
- Second period elements use dots to represent the number of bonds the atom can form.
Ionic Compounds and Bonding
- Ionic bonding involves electrostatic attraction between oppositely charged ions.
- Ionic compounds form from the interaction of a metal and a non-metal.
- Lattice energy is the energy required to convert a mole of an ionic solid to its gaseous ions.
- Lattice energy correlates with the stability and melting point of the compound.
Covalent Bonding and Molecules
- Covalent bonding involves sharing of electrons between non-metal atoms.
- Atoms form covalent bonds to achieve a noble gas configuration.
- A molecule is formed by two or more atoms joined together by covalent bonds.
Naming Ions and Ionic Compounds
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Law of Definite Proportions
- Different samples of the same compound contain the same elements in the same proportions by mass.
Law of Multiple Proportions
- If two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in a ratio of small whole numbers.
Molecular and Formula Mass
- Molecular mass is the sum of the atomic masses of all atoms in a molecule.
Percent Composition of Compounds
- Percent composition refers to the percentage by mass of each element present in a compound.
- The percent by mass of an element can be calculated by dividing the total mass of an element by the total molar mass of the compound then multiplying by one hundred.
Molar Mass
- Molar mass is the mass of one mole of a substance in grams.
- This is equal to the sum of the atomic masses of the elements in the compound.
Empirical Formula
- Empirical formula is the simplest whole-number ratio of atoms in a compound
Molecular Formula
- Molecular formula represents the actual number of atoms in a molecule.
- It's a multiple of the empirical formula.
Hydrates
- Hydrates are compounds with a specific number of water molecules within their crystal structures.
- This water can be driven off by heating, forming an anhydrous compound
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