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Practice Test
: Chapter 3
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Matching
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Limiting reactant (limiting reagent)
Mole
Theoretical yield
Stoichiometric Mixture
Molecular formula
Actual Yield vs. Percent Yield
Counting by Weighing
The reactant that runs out first and thus limits the amounts of products that can form. To find, compare mole ratio of balanced equations with mole ratio of reactants actually present
Count atoms as if they were all identical. Simply need to know the average mass of the objects. Can determine the number of atoms in a given sample by finding its mass.
The number equal to the number of carbon atoms in exactly 12 grams of pure C-12. Used for counting atoms. The mole is defined such that a sample of a natural element with a mass equal to the element's atomic mass expressed in grams contains 1 mole of atoms
Actual yield / theoretical yield x 100% = percent yield
One that contains the relative amounts of reactants that match the numbers in the balanced equation. All reactant consumed to form products
Exact formula of the molecule involved. Must know molar mass
Amount of a product formed when the limiting reagent is completely consumed. Maximum amount of compound that can be produced
Short Answer
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Average Atomic Mass
Modern system for atomic masses based on C-12
Chemical reaction
Molar mass
Mass Spectrometer
Multiple Choice
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Determining the formula of a compound
To find formula, use weighed sample of compound and decompose it into its elements or react it with oxygen to produce other substances
Actual yield / theoretical yield x 100% = percent yield
The number equal to the number of carbon atoms in exactly 12 grams of pure C-12. Used for counting atoms. The mole is defined such that a sample of a natural element with a mass equal to the element's atomic mass expressed in grams contains 1 mole of atoms
2 ways of describing composition of a compound. 1. Numbers of constituent atoms. 2. Percentages (by mass) of its elements
Percent composition of compounds
Molecular formula equivalent, for ionic compounds
Smallest whole-number ratio
The mass in grams of one mole of the compound
2 ways of describing composition of a compound. 1. Numbers of constituent atoms. 2. Percentages (by mass) of its elements
Chemical Stoichiometry
One that contains the relative amounts of reactants that match the numbers in the balanced equation. All reactant consumed to form products
Smallest whole-number ratio
Quantities of materials consumed and produced in chemical reactions
Chemical change involves a reorganization of the atoms in one or more substances. Bonds have been broken and new ones have been formed. Atoms neither created nor destroyed. Gives 2 types of information. 1) Nature of reactants and products. 2) Relative numbers of each
Empirical formula
Molecular formula equivalent, for ionic compounds
C-12 = exactly 12 atomic mass units (amu)
Smallest whole-number ratio
The reactant that runs out first and thus limits the amounts of products that can form. To find, compare mole ratio of balanced equations with mole ratio of reactants actually present
One that contains the relative amounts of reactants that match the numbers in the balanced equation. All reactant consumed to form products
Formula Unit
To find formula, use weighed sample of compound and decompose it into its elements or react it with oxygen to produce other substances
Atomic weight given on the periodic table an average value of all the isotopes of given element. Percentages based on commonality in nature
The mass in grams of one mole of the compound
Count atoms as if they were all identical. Simply need to know the average mass of the objects. Can determine the number of atoms in a given sample by finding its mass.
Molecular formula equivalent, for ionic compounds
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Practice Test: Chapter 3