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- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Chemistry_Basics/Gay-Lussac's_LawIf water is 88.9% O, 11.1% H, what is the atomic mass of O in terms of H (if you assume H is 1.00)? To answer, you need the formula: H 2 O (2 H atoms for 1 O atom) (11.1)/2 = 5.55 → (88.9)/5.55 = 16.0...If water is 88.9% O, 11.1% H, what is the atomic mass of O in terms of H (if you assume H is 1.00)? To answer, you need the formula: H 2 O (2 H atoms for 1 O atom) (11.1)/2 = 5.55 → (88.9)/5.55 = 16.0 (this is the atomic weight of O, assuming H is ~1) Gay-Lussac's law describes how increasing the temperature of a gas with a fixed volume and a constant number of "particles" will result in a similar increase in the pressure of the gas, and vice versa.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.01%3A_Avogadro's_NumberThis page explains Avogadro's number, 6.02×1023, which quantifies the number of representative particles in a mole, allowing chemists to measure atoms and molecules. It discusses the mol...This page explains Avogadro's number, 6.02×1023, which quantifies the number of representative particles in a mole, allowing chemists to measure atoms and molecules. It discusses the mole as the SI unit for substance amount, with representative particles being atoms for elements and molecules for compounds. Additionally, it mentions National Mole Day, celebrating this key chemistry concept.
- 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/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Chemical_Reactions/Stoichiometry/Amounts_of_SubstancesThe stoichiometric relationships among reactants and products may be complicated in units of g, but much simpler relationships are seen if we deal with units of moles or natural units of atoms and mol...The stoichiometric relationships among reactants and products may be complicated in units of g, but much simpler relationships are seen if we deal with units of moles or natural units of atoms and molecules. The number of moles of a substance in a sample is the mass in g divided by the molar mass, which gives the amount in moles.
