Jennifer Jiang Dr. Iobst Chemistry I Honors 11 March 2013 Molar Mass of Butane: Applying the Gas Laws 1. Water bath temperature: 17.7° C or 291 K Celsius to Kelvin temperature conversion: 17.7° C + 273 = 290.7 Kelvin (rounded to SF= 291 K) 2. 1 atm 1 atm 10 mm 10 mm 2.54 cm 2.54 cm According to the digital barometer our teacher provided‚ the barometric pressure in the lab is 29.77 in Hg‚ which will need to be converted to atmospheric pressure. 760 mm Hg 760 mm Hg 1 cm
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Chemistry 1110 Molar Mass of Butane Materials * Butane Lighter * Plastic Tube * 100 ml Graduated Cylinder * 2 Thermometers * Barometer * Sink Full of Water Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton’s Law of Partial Pressures and the ideal gas law. Hypothesis My hypothesis is that as we complete the experiment‚ we will be able to correctly use the air and water temperatures‚ volume of gas‚ and barometric
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09/17/13 Che 102L Lab # 4 Molar Mass by Freezing Point in Anti-Freeze. Objective: to determine the freezing point of pure naphthalene‚ determine the molar mass of an unknown by measuring the freezing point depression of a solution of the unknown in naphthalene. Materials: Beakers 600 mL‚ 2-250 mL‚Crystal Ice‚20 g of NaCl‚Stirring Rod‚Thermometer‚Foil‚ Water‚ 10 mL‚ Cylinder‚ 25 mL 100 mL Dropper‚ 2 Test Tubes. Procedure: Filled 600 mL beaker with ice‚ took temperature until it got
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the making of the solution. Using the volume and concentration of the solution‚ I was able to calculate the moles of the solution (concentration x volume). Using the periodic table I was able to calculate the molar mass of sodium carbonate which was 106‚ from this I could calculate the mass of the sodium carbonate I needed to make the solution (moles x Mr). After making the solution I cleaned the apparatus
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Discussion In this experiment‚ the molar mass of two volatile liquids – methanol and an unknown liquid – were calculated for through the Dumas Method. Initially‚ the sets of Erlenmeyer flasks with aluminum foil and rubber bands were weighed. Next‚ volatile liquids were placed in 125mL Erlenmeyer flasks and covered with aluminum foil‚ but small holes were made into the foil. The flask was then heated in a water bath until all of the liquid evaporated. The flask was then removed‚ and weighed again
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Experiment 19 Molar Mass Determination y Depression of the Freezing Point Introduction: The most commonly used liquid is water. In this experiment we study the equilibria that can exist between pure water and an aqueous solution‚ and ice‚ the solid form of water. The heat will transfer from a higher temperature to a lower temperature. In order for water to change states of matter‚ it takes a certain amount of kinetic energy or heat. The shift from ice to water (solid to a liquid) is called the
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College Preparatory Academy A mole is a scientific unit developed by chemist that measures large quantities of very small things‚ such as atoms‚ molecules‚ and other particles. There are three types of molar conversions; moles to particles or particles to moles‚ moles to mass or mass to moles‚ and moles to volume or volume to moles. The number of units in a mole is 6.02 × 1023. This number is called Avogadro’s number in honour of Amedeo Avogadro. Full name‚ Lorenzo Romano Amedeo Carlo Avogadro
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Determining the Molar Mass of an Unknown Solute by Freezing Point Depression Introduction: Colligative properties of solutions are only influenced by the concentration of solute particles and are independent of the nature of the solute. Some examples of colligative properties are boiling point elevation‚ vapor pressure lowering‚ and freezing point lowering (depression) (Brown‚ 542). For a substance to freeze‚ the kinetic energy of the particles must be low enough for the
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Practical 6 -Determining the Gas Constant Aim: To verify the gas constant as 8.31 J/mol/K ( ) and to calculate the molar mass of butane. Theory: The ideal gas law‚ PV=nRT‚ is used to model an ideal gas‚ which is a gas with no intermolecular forces other than those of collisions‚ perfectly spherical and elastic particles. Although an ideal gas is a theoretical model and so cannot exist in practice‚ most gases behave fairly similarly to an ideal gas. Gases behave more like an ideal gas when they are
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