'Convert mass' diaporamas de présentation

The Mole Concept

The Mole Concept. For chemists, a mole is NOT a small furry animal. A mole is the SI unit for amount of substance. This is a dozen eggs - that's an amount. A mole is like a dozen - only MORE. One gram bar of gold. Today, gold is selling for $$$ per gram.

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Atoms, Molecules, and Ions

Atoms, Molecules, and Ions. Chapter 2. 2.6 Molecules, Compounds, and Formulas. A molecule is the smallest identifiable unit into which a pure substance can be divided and still retain the composition and chemical properties of the substance. Molecules, Compounds, and Formulas.

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Highland Science Department Ideal Gas Law

Highland Science Department Ideal Gas Law. Highland Science Department Ideal Gas Law Avogadro's Law: equal volumes of all ideal gases at the same temperature and pressures contain the same number of molecules. Highland Science Department Ideal Gas Law

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Unit 4: Stoichiometry

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Moles (n) Weight (w) molecule count (N)

Multiply Down to weight and molecule count. Moles (n) Weight (w) molecule count (N). MW. 6.02*10 23. Divide up to moles.

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Formula of a Hydrate

Formula of a Hydrate. What is a hydrate?. An ionic compound that contains water molecules in its structure The formula states how many mol of water molecules per one mol of ionic compound Example: CuSo 4 ? 5 H 2 0 Copper sulfate pentahydrate. What is an anhydrate?.

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Things to definitely know for your exAM ?

Things to definitely know for your exAM ?. Periodic Trends. The names of the four we looked at How to explain at least one of your own choosing. Chemical Reactions. Classifying the main types: synthesis, single displacement, double displacement, decomposition, combustion

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6.10 Calculating Empirical Formulas

6.10 Calculating Empirical Formulas. The empirical formula gives the lowest whole-number ratio of the atoms of the elements in a compound. It tells the kinds and relative count (atoms or moles of atoms) in molecules or formula units of a compound.

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4.6 Empirical and Molecular Formulas

4.6 Empirical and Molecular Formulas. Empirical and Molecular Formulas. How do we find a chemical formula for and unknown substance? Identify elements & # of atoms of each element D etermine % composition by mass Convert mass values ? moles Formula = empirical formula

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The Gas Laws

The Gas Laws. The density of a gas decreases as its temperature increases. Ideal Gas Law. PV = nRT. Brings together gas properties. Can be derived from experiment and theory . Ideal Gas Law.

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Skills for this lab:

Skills for this lab: Find the molar mass of a substance (grams per mole)- add up all the elements average atomic mass using the periodic table ex: H 2 0 = H = 1 x 2 = 2 0 = 16 x 1= 16 H 2 0 is 18g/mol Convert mass to moles ? divide by the molar mass How many moles in 56g of water?

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