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What is stoichiometry?
What is stoichiometry?
The calculation of quantities in chemical reactions is a subject of chemistry.
What is a mole ratio?
What is a mole ratio?
A conversion factor derived from coefficients of a balanced chemical equation interpreted in terms of moles.
What is a limiting reagent?
What is a limiting reagent?
The reagent that determines the amount of product that can be formed by a reaction.
What is an excess reagent?
What is an excess reagent?
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What is theoretical yield?
What is theoretical yield?
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What is actual yield?
What is actual yield?
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What is percent yield?
What is percent yield?
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How do chemists use balanced chemical equations?
How do chemists use balanced chemical equations?
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What quantities can you interpret from a balanced chemical equation?
What quantities can you interpret from a balanced chemical equation?
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In a chemical reaction, mass is conserved.
In a chemical reaction, mass is conserved.
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In mole to mole conversions: Amount of given substance A in moles multiplied by mole ratio from balanced equation equals amount of unknown substance B in moles. A (in moles) x ____ = B (in moles)
In mole to mole conversions: Amount of given substance A in moles multiplied by mole ratio from balanced equation equals amount of unknown substance B in moles. A (in moles) x ____ = B (in moles)
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In mole to mass conversions: Amount of given substance A in moles multiplied by #1: Mole ratio from balanced equation multiplied by #2 Molar Mass from periodic table equals amount of unknown substance B in grams. A (in moles) x #1 x #2 = B (in grams)
In mole to mass conversions: Amount of given substance A in moles multiplied by #1: Mole ratio from balanced equation multiplied by #2 Molar Mass from periodic table equals amount of unknown substance B in grams. A (in moles) x #1 x #2 = B (in grams)
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In mass to mole conversions: Amount of given substance A in grams multiplied by #2 Molar mass from periodic table multiplied by #1 Mole ratio from balanced equation equals amount of unknown substance B in moles. A (in grams) x #2 x #1 = B (in moles)
In mass to mole conversions: Amount of given substance A in grams multiplied by #2 Molar mass from periodic table multiplied by #1 Mole ratio from balanced equation equals amount of unknown substance B in moles. A (in grams) x #2 x #1 = B (in moles)
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In mass to mass conversions: Amount of given substance A in grams multiplied by #2 Molar mass from periodic table multiplied by #1 Mole ratio from balanced equation multiplied by #3 Molar mass from periodic table equals amount of unknown substance B in grams. A (in grams) x #2 x #1 x #3 = B (in grams)
In mass to mass conversions: Amount of given substance A in grams multiplied by #2 Molar mass from periodic table multiplied by #1 Mole ratio from balanced equation multiplied by #3 Molar mass from periodic table equals amount of unknown substance B in grams. A (in grams) x #2 x #1 x #3 = B (in grams)
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How do you convert grams of substance A to molecules of substance B?
How do you convert grams of substance A to molecules of substance B?
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Given the reaction N₂ + 3F₂ → 2NF₃, how many molecules of nitrogen are needed to produce 3.17g of nitrogen trifluoride?
Given the reaction N₂ + 3F₂ → 2NF₃, how many molecules of nitrogen are needed to produce 3.17g of nitrogen trifluoride?
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Given the reaction N₂(g) + 3H₂(g) → 2NH₃ (g), if 14.5 liters of hydrogen gas is used, how many liters of ammonia would be produced?
Given the reaction N₂(g) + 3H₂(g) → 2NH₃ (g), if 14.5 liters of hydrogen gas is used, how many liters of ammonia would be produced?
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Identify the limiting and excess reactants in the reaction Mg + 2H₂O → Mg(OH)₂ + H₂ when 16.2 g Mg are reacted with 12.0g H₂O.
Identify the limiting and excess reactants in the reaction Mg + 2H₂O → Mg(OH)₂ + H₂ when 16.2 g Mg are reacted with 12.0g H₂O.
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What does the percent yield of a reaction measure?
What does the percent yield of a reaction measure?
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Calculate the percent yield given that the actual yield is 46.3 g KCl and the theoretical yield is 49.4 g KCl.
Calculate the percent yield given that the actual yield is 46.3 g KCl and the theoretical yield is 49.4 g KCl.
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Study Notes
Stoichiometry Basics
- Stoichiometry involves calculating quantities in chemical reactions.
- A mole ratio is derived from the coefficients in a balanced chemical equation, used as a conversion factor.
Key Concepts
- The limiting reagent is the reactant that limits the amount of product formed in a reaction.
- An excess reagent is the reactant that remains unreacted after the reaction completes.
- The theoretical yield represents the maximum possible product yield from given reactants, while actual yield is the product amount obtained in practice.
- Percent yield is the ratio of actual yield to theoretical yield, expressed as a percentage.
Application of Balanced Equations
- Chemists utilize balanced chemical equations for determining reactant quantities needed and product amounts generated.
- A balanced equation provides insight into numbers of atoms, molecules, or moles along with their mass and volume conversions.
Conservation of Mass Principle
- In chemical reactions, mass conservation means that matter cannot be created or destroyed.
Conversion Processes
- Mole to Mole: Use mole ratios to convert amount of one substance in moles to another.
- Mole to Mass: Multiply moles by mole ratio and then by the molar mass to find mass in grams.
- Mass to Mole: Use grams multiplied by molar mass and mole ratio to determine moles.
- Mass to Mass: Combine grams, mole ratios, and molar masses to convert between masses of two substances.
- Mass to Molecules: Convert grams to molecules or vice versa.
Examples
- Mass to Molecules Conversion: To find the number of molecules of nitrogen needed for 3.17g of nitrogen trifluoride, the result is 1.33 x 10²² molecules of N₂.
- Volume to Volume Conversion Example: From 14.5 L of hydrogen gas, 9.67 L of ammonia can be produced under STP conditions.
Limiting Reactants Example
- Given the reaction Mg + 2H₂O → Mg(OH)₂ + H₂, with 16.2g of Mg and 12.0g of H₂O:
- Limiting reagent: 12.0g H₂O
- Excess reagent: 16.2g Mg
Percent Yield Calculation
- Percent yield measures a reaction's efficiency:
- Given actual yield of 46.3g KCl and theoretical yield of 49.4g KCl, the calculation is:
- % yield = (46.3g / 49.4g) x 100.
Studying That Suits You
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Description
Test your knowledge of stoichiometry with these flashcards that cover key concepts such as mole ratio, limiting reagent, and more. Perfect for students looking to enhance their understanding of chemical quantities and reactions.
