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- https://chem.libretexts.org/Courses/University_of_California_Irvine/UCI%3A_General_Chemistry_1A_(OpenChem)/119The_Gas_Laws_-_Avogadro's_Law_(OpenChem)
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/01%3A_The_Basics/1.01%3A_The_System_and_the_SurroundingsThe page discusses the Zeroth Law of Thermodynamics, emphasizing the importance of defining key terms like "system" and "surroundings." Various types of systems are identified, such as open, closed, a...The page discusses the Zeroth Law of Thermodynamics, emphasizing the importance of defining key terms like "system" and "surroundings." Various types of systems are identified, such as open, closed, and isolated systems, based on how they allow matter and energy transfer. The distinctions between homogeneous and heterogeneous systems are also outlined, along with the significance of intensive and extensive variables.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.07%3A_Conversions_Between_Moles_and_Gas_VolumeThis page discusses the measurement of gas volume in chemistry, focusing on the calculation of moles for optimal reactions. It highlights the concept of molar volume at standard temperature and pressu...This page discusses the measurement of gas volume in chemistry, focusing on the calculation of moles for optimal reactions. It highlights the concept of molar volume at standard temperature and pressure (STP), where 1mol=22.4L, and provides examples for converting gas volumes to moles and vice versa. The importance of maintaining STP conditions during these calculations is emphasized, along with practice questions for further comprehension.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/12%3A_Stoichiometry/12.08%3A_Determining_the_Limiting_ReactantThis page explains how to find the limiting reactant in a chemical reaction, illustrated by the reaction of silver and sulfur to form silver sulfide. It details steps to convert mass to moles, use a b...This page explains how to find the limiting reactant in a chemical reaction, illustrated by the reaction of silver and sulfur to form silver sulfide. It details steps to convert mass to moles, use a balanced equation for mole ratios, and identify excess reactants. In the example provided, silver is the limiting reactant, while sulfur remains in excess. Additionally, it outlines how to calculate the mass of the excess reactant left after the reaction.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.05%3A_Conversions_Between_Mass_and_Number_of_ParticlesThis page outlines Avogadro's contributions to gas laws, focusing on the connections between gas volume, particle count, and mass. It details the conversion of mass to the number of particles through ...This page outlines Avogadro's contributions to gas laws, focusing on the connections between gas volume, particle count, and mass. It details the conversion of mass to the number of particles through moles, featuring an example with 20 grams of chlorine gas (Cl2). The summary highlights the calculation methods and includes review questions to reinforce understanding of mass and particle conversions.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.02%3A_Conversions_Between_Moles_and_AtomsThis page explains conversion methods between moles, atoms, and molecules, emphasizing the convenience of moles for simplifying calculations. It provides examples on converting carbon atoms to moles a...This page explains conversion methods between moles, atoms, and molecules, emphasizing the convenience of moles for simplifying calculations. It provides examples on converting carbon atoms to moles and determining hydrogen atoms in water and sulfuric acid. The importance of knowing chemical formulas for accurate calculations is highlighted, accompanied by step-by-step calculation processes. The document concludes with review questions on the discussed concepts.
- https://chem.libretexts.org/Courses/Lakehead_University/Analytical_I/2%3A_Basic_Tools_of_Analytical_Chemistry/2.3%3A_Stoichiometric_CalculationsA balanced reaction, which gives the stoichiometric relationship between the moles of reactants and the moles of products, provides the basis for many analytical calculations.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/03%3A_Basic_Tools_of_Analytical_Chemistry/3.3%3A_Stoichiometric_CalculationsA balanced reaction, which gives the stoichiometric relationship between the moles of reactants and the moles of products, provides the basis for many analytical calculations.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.03%3A_Molar_MassThis page explains how to calculate the amount of a substance needed for a solution based on its molar mass, using carbon dioxide and calcium nitrate as examples. It highlights the relationship betwee...This page explains how to calculate the amount of a substance needed for a solution based on its molar mass, using carbon dioxide and calcium nitrate as examples. It highlights the relationship between moles and grams and underscores the importance of molar mass for accurate measurements in solution preparation. The page also includes review questions to help reinforce understanding of molar mass and its calculations.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)/04%3A_The_Mole_and_Measurement_in_Chemistry/4.S%3A_The_Mole_and_Measurements_in_Chemistry_(Summary)Because atomic masses, and the number of particles in a mole, are both based on the isotopic atomic mass of the isotope carbon-12, the mass of any substance expressed in atomic mass units is numerical...Because atomic masses, and the number of particles in a mole, are both based on the isotopic atomic mass of the isotope carbon-12, the mass of any substance expressed in atomic mass units is numerically equal to the molar mass of the substance in grams per mole.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/16%3A_Solutions/16.08%3A_MolarityThis page explains molarity as a concentration measure in solutions, defined as moles of solute per liter of solution. It contrasts molarity with percent solutions, which measure mass instead of molec...This page explains molarity as a concentration measure in solutions, defined as moles of solute per liter of solution. It contrasts molarity with percent solutions, which measure mass instead of molecular quantity. The text includes examples for calculating molarity and finding the mass of solute required for specific concentrations, underscoring the importance of accurate measurements in laboratory settings.
