Lecture 10.2a- Mole Mass Conversions
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The document discusses converting between moles, number of particles, and mass for various substances. It provides examples of calculating the mass of substances like magnesium and arsenic given a number of moles. The key steps shown are using the molar mass from the periodic table to convert between moles and mass, and using Avogadro's number to convert between number of particles and moles.
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1) The document discusses moles, Avogadro's number, and molar mass. It defines a mole as 6.02 x 1023 particles, such as atoms, ions, or molecules.
2) To convert between moles and particles, atoms, or molecules, you must multiply or divide by Avogadro's number. Molar mass is the mass in grams of one mole of a substance and is used to convert between moles and grams.
3) Examples are provided for calculating molar mass and for converting between moles, grams, and number of particles using molar mass and Avogadro's number.
Chem m16 stoichiometry
This chemistry module discusses stoichiometry and the mole concept. It contains 4 lessons:
1) Defining a mole and the mole-particle relationship.
2) Exploring the mole-mass relationship through examples and activities.
3) Relating the mass of reactants and products in chemical equations using moles.
4) Calculating mass percent composition of elements in compounds.
The module aims to teach students how to use moles to relate mass, number of particles, and chemical equations.
The mole
- A mole represents 6.02 x 10^23 particles of a substance, whether atoms, molecules, ions, etc. This number is known as Avogadro's number.
- Common examples are given to illustrate just how large Avogadro's number is, such as the number of atoms needed to cover the Earth's surface.
- The document provides examples of calculating the number of particles and moles of different substances.
2016 topic 01 part 1
This document discusses quantitative chemistry concepts including the mole, Avogadro's constant, molar mass, and using moles to calculate the number of particles and mass of substances. Some key points covered are:
- A mole is a unit used to count fundamental particles and represents 6.02x1023 particles.
- The mole allows converting between large numbers of particles and more manageable units like grams.
- Molar mass relates the mass of a sample of a substance to the number of moles it contains.
- Problems use molar mass to calculate moles, particles, or mass given any two of those quantities.
Chapter 7.3 : Using Chemical Formulas
This document discusses calculating formula masses, molar masses, and percentage compositions of chemical compounds. It provides examples of calculating the formula mass of compounds by adding the atomic masses of each element. Molar mass is defined as the mass of one mole of a compound and is numerically equal to formula mass. The document demonstrates using molar mass to convert between mass and moles of a compound. It also gives examples of calculating the percentage by mass of each element in compounds like copper(I) sulfide and sodium carbonate decahydrate.
Chapter_3_Mass_Relationships.ppt
1. The document discusses mass relationships in chemical reactions including atomic mass, molar mass, molecular mass, formula mass, and percent composition.
2. It defines the mole as the amount of a substance containing 6.022x1023 elementary entities, such as atoms or molecules. Molar mass is the mass in grams of one mole of a substance.
3. Examples are provided for calculating the number of atoms, moles of substances, and masses involved in chemical reactions using molar mass and mole ratios from balanced chemical equations.
Lecture 10.1- The Mole
The document discusses the mole, which is used to measure the quantity of particles in chemical reactions. A mole is defined as 6.02 x 1023 particles and represents atoms, molecules, or formula units that are involved in a balanced chemical equation. The mass of one mole of an element or compound, known as its molar mass, is equal numerically to the atomic/formula mass and given in grams. The mole allows chemists to quantitatively relate the masses of reactants and products in chemical reactions.
Concept of mole
1. A mole is defined as the amount of substance containing 6.02 x 1023 particles and can refer to atoms, molecules, or ions.
2. The mole is the unit for quantifying amount of substance, with the symbol "mol".
3. The number of particles in a given number of moles can be calculated by multiplying the moles by Avogadro's number, and the moles for a given number of particles is calculated by dividing the particles by Avogadro's number.
Moles
The document discusses the mole, which relates the number of particles in a substance to its mass in grams. It defines one mole as 6.02 x 10^23 particles, known as Avogadro's number. It provides examples of calculating moles, mass, and number of particles using molar mass and unit conversion with moles. Key relationships discussed are mass=moles×molar mass and number of particles=moles×Avogadro's number.
Chapter 10 The Mole
The document discusses the concept of the mole in chemistry. It defines a mole as 6.02 x 1023 representative particles, which can be atoms, molecules, or formula units. It provides examples of calculating the number of moles and mass of different substances. It also explains that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure. Key terms discussed include molar mass, percent composition, empirical formula, and molecular formula.
Mole Concept.pptx (Grade 9, second quarter)
The document discusses the mole concept in chemistry. It defines the mole as the amount of substance that contains as many elementary units (atoms, molecules, ions) as there are atoms in exactly 12 grams of carbon-12. The number of elementary units in one mole is Avogadro's number, which is approximately 6.022x1023. Examples are given to illustrate that one mole of any substance will contain this number of particles, though the masses in grams will vary depending on the molar masses of the substances. The mole can be used to convert between the number of particles, moles, and mass in grams for calculations involving chemical substances.
CHEMISTRY 10 UNIT 1.pptx
A) Molecular formula of butane is C4H10
Molecular weight = (4 x 12) + (10 x 1) = 58 g/mol
B) 0.25 mol x 58 g/mol = 14.5 g
C) 2.9 g x 1 mol/58 g = 0.05 mol = 5 x 1022 molecules
D) 1.5 x 1022 molecules x 58 g/mol = 87 g
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SHS STEM General Chemistry 1: Atoms, Moles, Equations, Stoichiometry
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Chapter 3 and 5 lecture- Ecology & Population Growth
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1) The levels of ecological organization from lowest to highest are individual, population, community, ecosystem, biome, and biosphere.
2) Energy enters ecosystems mainly through photosynthesis by producers like plants and algae. It is then transferred as heterotroph consumers eat producers or other consumers.
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1. Reproduction in seed plants occurs within flowers or cones through a process called alternation of generations. In this process, haploid gametophytes are produced from diploid sporophytes and fuse during fertilization to form a new diploid sporophyte.
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Chapter 22- Plant Diversity
Plants are multicellular eukaryotes that have cell walls made of cellulose and carry out photosynthesis. They go through life cycles of alternating diploid and haploid generations. Early plants evolved from multicellular green algae and the first plants were similar to modern mosses. Bryophytes like mosses reproduce using sperm and eggs that require water, while vascular plants like ferns have specialized tissues to transport water and nutrients throughout the plant.
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Chapter 37- Circulatory and Respiratory Systems
The circulatory system transports blood throughout the body via the heart and blood vessels. The heart has four chambers and uses valves to pump oxygenated blood from the lungs and deoxygenated blood to the lungs. Blood flows through arteries, capillaries, and veins. The respiratory system exchanges gases through the nose, pharynx, trachea, bronchi, and alveoli in the lungs. Breathing is controlled by the medulla oblongata and diaphragm. Smoking damages lungs and increases risk of diseases like cancer, emphysema, and bronchitis.
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Fredrick Griffith discovered that heat-killed pneumonia bacteria could transform harmless bacteria into deadly disease-causing bacteria when mixed together and injected into mice. This led researchers like Oswald Avery to determine that DNA was the molecule responsible for transformation. Further experiments by Hershey and Chase showed that the genetic material of viruses that infect bacteria is DNA. Together, these findings established DNA as the genetic material that gets passed from parents to offspring and controls inheritance.
Chapter Eleven- Intro to Genetics
1. Gregor Mendel was an Austrian monk who studied inheritance patterns in pea plants and is considered the founder of genetics.
2. He conducted breeding experiments with pea plants involving both self-pollination and cross-pollination to study inherited traits like plant height, seed texture, flower color and more.
3. Through his experiments, Mendel discovered that traits are passed from parents to offspring through discrete units later known as genes, and that some genes are dominant while others are recessive.
Chapter Ten Lecture- Mitosis
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Chapter Eight- Photosynthesis
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Lecture 10.2a- Mole Mass Conversions
- 2. Converting between moles and number of particles involves multiplying or dividing by 6.02 x 10 23
- 3. Converting between moles and mass involves multiplying or dividing by the molar mass of the substance
- 4. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh?
- 5. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh? 3.75 moles Mg
- 6. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh? 3.75 moles Mg X
- 7. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh? 3.75 moles Mg X 24.305 grams 1 mole Mg
- 8. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh? 3.75 moles Mg X 24.305 grams 1 mole Mg = 91.1 grams Mg
- 9. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh? 3.75 moles Mg X 24.305 grams 1 mole Mg = 91.1 grams Mg WHERE THE HECK DID THIS COME FROM?!?
- 10. Convert from moles to mass How much does 3.75 moles of magnesium metal weigh? 3.75 moles Mg X 24.305 grams 1 mole Mg = 91.1 grams Mg WHERE THE HECK DID THIS COME FROM?!? The periodic table!
- 11. 10.5 Moles to grams 9.45 mol Al 2 O 3 x ___________ = 964g Al 2 O 3 1 mol Al 2 O 3 102g Al 2 O 3 2 Al = 54g 3 O = 48 g 102g
- 12. Grams to moles
- 16. Mole Review huge # of particles 6 x 10 23 6 x 10 23 (g) grams (mass) molar mass molar mass Use the periodic table! Use the mole banner!
Editor's Notes
- These aluminum satellite dishes at the National Radio Astronomy Observatory near Soccoro, New Mexico are naturally protected from corrosion by the formation of a thin film of aluminum oxide (Al 2 O 3 ).
- Rust weakens an iron chain.