with the atomic theory‚ which states that all substances are composed of a large number of very small particles (molecules or atoms). In principle‚ the observable properties of gas (pressure‚ volume‚ temperature) are the consequence of the actions of the molecules making up the gas. The Kinetic Molecular Theory of Gases begins with five postulates that describe the behavior of molecules in a gas. These postulates are based upon some simple‚ basic scientific notions‚ but they also involve some simplying
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Avogadro’s Law? Yes 4. Based on the calculated number of moles in one 1 atm of gas‚ how many molecules are in 1 atm of gas? (There are 6.022 x 1023 molecules/mole) Since all 3 gases have the same number of moles I will calculate 1 formula for all 3. 0.0062mol (6.022 x 1023 molecules/mol)= 0.0373364 →3.73 x 1022 molecules for each gas are in 1atm. 5. Even though the number of molecules in 1 atm of gas at constant pressure and temperature is identical‚ the number of atoms in the gas
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able to: Mole Concept • Calculate formula mass. • Convert representative particles to moles and moles to representative particles. (Representative particles are atoms‚ molecules‚ formula units‚ and ions.) • Convert mass of atoms‚ molecules‚ and compounds to moles and moles of atoms‚ molecules‚ and compounds to mass. • Convert representative particles to mass and mass to representative particles. • Convert moles to volume and volume to moles at STP. • Calculate
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(Jan 2012) (a) Identify polar group(s) in molecule A & write down the chemical formula(s) (b) Redraw the molecule A; the answer the following questions: (i) Label chiral centre(s) using (*) (ii) Label & identify type(s) of hybridization of all carbons in molecule A (iii) Identify 2 bonds in the molecule containing π bonds. 4. Consider the compound below:
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1 mole of any substance can be defined as: Amount of a substance that contains as many particles (atoms‚ molecules or ions) as there are atoms in 12 g of the 12C isotope Avogadro number or Avogadro constant (NA); equal to 6.022 × 1023 particles Example − 1 mole of oxygen atoms = 6.022 × 1023 atoms 1 mole of carbon dioxide molecules = 6.022 × 1023 molecules 1 mole of sodium chloride = 6.022 × 1023 formula units of sodium chloride Molar mass of a substance can be defined as: Mass of one mole
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bonds with water molecules. A hydrate is a compound that incorporates water molecules into its crystalline lattice structure (McGraw-Hill Ryerson‚ 2014). Identifying a compound as hydrated or anhydrous is important as the mass of the compound increases if it contains water molecules. In nature‚ hydrates exist with a fixed ratio of water molecules bound to each formula unit. These salts are able to release water to become anhydrous‚ or the anhydrous compound can absorb water molecules into their ionic
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What is the empirical formula of a compound that contains 75% Ag and 25% Cl by mass? AGCL Calculate the approximate number of molecules in a drop of water with a mass of 0.10 g. 3 x 1021 molecules What is the percentage composition of CaSO4? 29.44% Ca‚ 23.55% S‚ 47.01% O What mass of calcium bromide is needed to prepare 150.0 mL of a 3.50 M solution? (Assume that the molecular weight of CaBr2 is 200.618 g/mol) 105 g Nitrous oxide (N2O)‚ or laughing gas‚ is commonly used as an anesthetic
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to have sufficient volatility. The theory behind the mass spectrometer is to use the difference in mass-to-charge ratio (m/e) of ionized atoms or molecules to separate them from each other. Mass spectrometry is therefore useful for quantitation of atoms or molecules and also for determining chemical and structural information about molecules. Molecules have distinctive fragmentation patterns that provide structural information to identify structural components. The combination of the gas chromatograph
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apart as possible. Though there is some structural diversity in ionic compounds‚ covalent compounds present us with a world of structural possibilities. From simple linear molecules like H2 to complex chains of atoms like butane (CH3CH2CH2CH3)‚ covalent molecules can take on many shapes. To help decide which shape a polyatomic molecule might prefer we will use Valence
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Chapter 1 Carbon Compounds and Chemical Bonds. (Covered material: 1.1 - 1.8; 1.12 - 1.17) 1. Structural Theory – most fundamental theory of Organic Chemistry (developed independently by A. Kekule‚ A. Couper and A. Butlerov between 1858 and 1861). Organic Compounds – compounds of carbon and hydrogen. Other elements frequently found in organic compounds are: oxygen‚ nitrogen and halogens (F‚ Cl‚ Br‚ I); less frequently found are: sulfur and phosphorus. Review Periodic Table for determining valence
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