# Stoichiometry Flashcards

Stoichiometry Flashcards
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Define the term: chemical formula
The precise composition of a substance, giving the exact number of each type of atom in a molecule.
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Define the term: excess reactant
If you finish all of one reactant in a chemical reaction, and you have leftovers of the other reactant, the one you have left over is the excess reactant.
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Define the term: limiting reactant
If you finish all of one reactant in your reaction, and you still have leftovers of the other reactant, the one you finished first is the limiting reagent.
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Define the term: molar volume
One mole of gas will fill 22.4 L of volume at standard temperature and pressure.
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Define the term: Standard Temperature and Pressure (STP)
0 degrees Celsius (273 Kelvins) and 1 atmosphere of pressure
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Define the term: Coefficient
The number we put in front of an element or compound to say how many atoms or molecules we have of it.
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What it means to balance a chemical equation
Add coefficients to a product or a reactant so that we have the same number of atoms of each element on both sides of the equation.
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How many atoms should appear in the 'products' side of a balanced chemical reaction
The same number of atoms as there were in the 'reactants' side
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## Flashcard Content Overview

In these flashcards, students can test their knowledge of stoichiometry. The cards cover the basic principle of what a balanced chemical equation means. Students can learn the difference between a chemical formula and an empirical formula.

This flashcard set also teaches you about the necessary calculations when working with limiting reactants and excess reactants. And you can test your memory of actual yield, theoretical yield, and percent yield. Finally, you'll be able to review key concepts for working with gases in chemical equations, such as molar volume and Standard Temperature and Pressure (STP).

Front
Back
How many atoms should appear in the 'products' side of a balanced chemical reaction
The same number of atoms as there were in the 'reactants' side
What it means to balance a chemical equation
Add coefficients to a product or a reactant so that we have the same number of atoms of each element on both sides of the equation.
Define the term: Coefficient
The number we put in front of an element or compound to say how many atoms or molecules we have of it.
Define the term: Standard Temperature and Pressure (STP)
0 degrees Celsius (273 Kelvins) and 1 atmosphere of pressure
Define the term: molar volume
One mole of gas will fill 22.4 L of volume at standard temperature and pressure.
Define the term: limiting reactant
If you finish all of one reactant in your reaction, and you still have leftovers of the other reactant, the one you finished first is the limiting reagent.
Define the term: excess reactant
If you finish all of one reactant in a chemical reaction, and you have leftovers of the other reactant, the one you have left over is the excess reactant.
Define the term: chemical formula
The precise composition of a substance, giving the exact number of each type of atom in a molecule.
Define the term: empirical formula
A simplified formula that shows only the ratio/proportions of elements to each other in a given compound.
How to determine the limiting reactant in a chemical reaction.
Calculate how many moles of Reactant B you need, to react with all of Reactant A. If you have more B than that, A is the limiting reactant. If you have less, B is the limiting reactant.
Define the term: mole ratio
The ratio of the number of moles of one substance to another in a balanced chemical reaction
How to determine the volume of a gaseous product of a chemical reaction, if conditions are not at STP
Use the Ideal Gas Law (PV=nRT).
Conditions for multiplying 'moles of product' by 22.4 L to calculate the volume of product
The product must be a gas at 1 atm pressure and 0 degrees Celsius (273 Kelvins)
Define this term: theoretical yield of a chemical reaction
The biggest possible amount of product you would get from a given amount of reactants, if the reaction worked perfectly.
Define the term: actual yield of a chemical reaction
The amount of product you really got, when you measured the result of your reaction.
How to calculate percent yield
(Actual yield / theoretical yield) * 100%

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