Chemistry June Exam Notes Quantities in Chemical Reactions Molecular and formula mass o The mass of one unit of a compound (a molecule or a formula unit) o The sum of the mass of all the atoms in a compound o With knowledge of the mass of each individual atom‚ the percentage composition by mass can be determined The Mole (mol) o A counting unit‚ one mole refers to 6.02 x 1023 particles of any given substance o Known as Avogadro’s Constant and given the symbol NA Molar Mass o The
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atom (F‚ O or N) of another molecule. THERMAL ENERGY Thermal energy is the energy of a body arising from motion of its atoms or molecules. It is directly proportional to the temperature of the substance. THE GAS LAWS Boyle’s Law At constant temperature‚ the pressure of a fixed amount of gas is inversely proportional to its volume. P1V1 = P2V2 Each curve corresponds to a different constant temperature and is known
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Contents ------------------------------------------------------------------------ I. Introduction………………………………………......3 II. Thermodynamics Properties………...….……………5 III. Thermodynamic Laws……………………………….6 IV. Compression Cycles…………………………………7 V. Ideal Positive Displacement Compressor Cycle……………8 VI. Ideal Dynamic Compressor Cycle.......………………9 VII. Compressor Types……………………………...……9 VIII. Centrifugal Compressor……………………...….…..9 IX. Centrifugal Compressor Types……………………...10 X. Compressors
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The Gas Laws The Gas Laws 1. Boyle’s Law – P-V Relationship the pressure of a fixed amount of gas maintained at constant temperature is inversely proportional to the volume of the gas. The Gas Laws 2. Charles’ Law – T-V Relationship the volume of a fixed amount of gas maintained at constant pressure is directly proportional to absolute temperature of the gas. The Gas Laws 3. Gay-Lussac’s Law – P-T Relationship the pressure of a fixed amount of gas maintained
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produced‚ applying Dalton’s Law and the Ideal Gas Equation along with the application of the stoichiometric ratio between the electron and the gases‚ the fundamental electronic charge will be determined. THEORY H+ ions will join together at the cathode (the negative electrode) to produce H Atoms‚ and the H atoms will join to form molecules of H2 gas. At the positive electrode (the anode)‚ H20 molecules will decompose to replace the H+ ions lost and release O2 gas. The reactions appear below
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moles-stoichiometry-practice-problems Now you’re ready to use what you know about conversion factors to solve some stoichiometric problems in chemistry. Almost all stoichiometric problems can be solved in just four simple steps: 1.Balance the equation. 2.Convert units of a given substance to moles. 3.Using the mole ratio‚ calculate the moles of substance yielded by the reaction. 4.Convert moles of wanted substance to desired units. These "simple" steps probably look complicated at first
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Object The object of this experiment is to find the relation between pressure and volume for the expansion of air in a pressure vessel – this expansion is a thermodynamic process. Introduction The expansion or compression of a gas can be described by the polytropic relation ‚ where p is pressure‚ v is specific volume‚ c is a constant and the exponent n depends on the thermodynamic process. In our experiment compressed air in a steel pressure vessel is discharged to the atmosphere
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Nailea Rosales Chemistry THE GAS LAWS LAB LAB 1 Pressure in kPa Volume in ml Dataset 1 30 90 Dataset 2 35 80 Dataset 3 40 75 Dataset 4 45 70 Dataset 5 50 60 Dataset 6 60 50 LAB 2 New temp. in Celsius New Volume in ml Dataset 1 5 47 Dataset 2 10 48 Dataset 3 15 49 Dataset 4 20 50 Dataset 5 25 51 Dataset 6 30 52 1. Describe the relationship that you observed between pressure and volume in this lab. Refer to your data and/or graph to help support your answer. I observed that the higher the pressure
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transferred to a 1.1-L flask at 25°C‚ what will be the gas pressure in the flask? 2. A balloon has temperature of 28°C. What will be the final temperature of the gas if the volume is reduced to half of the original under isobaric condition? 3. Calculate the volume occupied by 4.23 kg of methane gas at STP. 4. Dry ice is useful in maintaining frozen foods because it vaporizes to CO2 (g) rather than melting to a liquid. How many liters of CO2 gas‚ measured at STP‚ will be produced by the vaporization
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between molecules‚ as was HYPERLINK http//en.wikipedia.org/wiki/Isaac_NewtonIsaac Newtons conjecture‚ but due to HYPERLINK http//en.wikipedia.org/wiki/Collisioncollisions between molecules moving at different velocities. While the particles making up a gas are too small to be visible‚ the jittering motion of pollen grains or dust particles which can be seen under a microscope‚ known as HYPERLINK http//en.wikipedia.org/wiki/Brownian_motionBrownian motion‚ results directly from collisions between the particle
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