...The ideal gas law is where the product of the pressure and the volume of one gram molecule of an ideal gas is equal to the product of the absolute temperature of the gas and the universal gas constant. This is represented by PV = nRT, where R is the ideal gas constant of 0.08206 L*atm/mol*k and is a relationship of energy to quantity of matter at any given temperature. An ideal gas has no definite volume or mass, unlike real gas. Pressure is also higher in ideal gas compared to real gas. Dalton's law of partial pressures states that the total pressure exerted by a mixture of gases is the sum of partial pressure of each individual gas present. Each gas is also assumed to be an ideal gas. The reaction Mg + 2HCl = H2 + MgCl2 is used to compare the ideal gas law constant in order to complete the objective of this experiment, which is to verify the ideal gas law constant. Results:...
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...COMBINED GAS LAW SUMMARY The combined gas law is a gas law which combines Charles's law, Boyle's law, and Gay-Lussac's law. This law states: “The ratio between the pressure-volume product divided by the temperature of a system remains constant.” This can be stated mathematically as:  Where: p is the pressure, V is the volume, T is the temperature measured in kelvins, and k is a constant (with units of energy divided by temperature). Reminder: 1atm= 760 torr = 101.3 kPa & Celsius to Kelvin= add 273 and Kelvin to Celsius= subtract 273 For comparing the same substance under two different sets of conditions, the law can be written as:  If the problem does not state which unit to give the result in, then make sure that temperature is converted into Kelvin and for the Pressure and Volume just make sure you stay constant and use the same unit on both sides of the equation. Combination of 3 Laws: Boyle's Law states that the pressure-volume product is constant:  In other words as external pressure on a gas increases the volume decreases, and vice versa. Charles's Law shows that the volume is proportional to absolute temperature:  In other words as temperature increases the volume increases, and vice versa. Gay-Lussac's Law says that the pressure is proportional to the absolute temperature:  In other words as temperature increases the pressure increases, and vice versa. Where P is the pressure, V the volume and T the absolute temperature and of an ideal gas. By combining...
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...Marigona Krasniqi 15 October 2015 Contemporary Science: Chemistry Lab assignment Gas Laws Lab Part 1 – The effect of temperature on gas volume Problem: Which gas law describes these results (Paper assignment)? Observation/ Research: Charles’s Law According to Jacques Charles, “if the temperature of the gas increases, the volume of the gas also will be increased or other way around.” (Charles). This statement describes Charles Law. According to this law, “the Volume and Temperature are directly proportional and pressure is held constant” (Charles). This shows that V/T = k, where k is constant. So, the formula of this law is: V1/T1 = V2/T2 (Charles’s Law) Hypothesis: If the temperature of the gas within the syringe is decreased, then the...
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...Gas laws apply in many everyday activities and daily necessities including air travel and recreation. Air medical services use gas laws in order to understand how the changes in altitude affect people, equipment and the internal environment of the aircraft. Several laws affect air travel including Boyle’s law, Henry’s law, Dalton’s law and Graham’s Law. Boyle’s law is relevant as it explains how pressure changes allow the gas to expand (Monroney, 2013). Dalton’s law transfers oxygen molecules from a person’s lungs to their bloodstream depending on the pressure gradient. Henry’s Law relates to the pressure of a gas over liquid (solubility). Within humans physiology the three physiological zones within the atmosphere are utilised to control conditions. Between sea level and 3 048 metres above sea level...
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...In the 2015 AFC Championship football game, opponents Indianapolis Colts and New England Patriots went head to head for the title and bling. With the New England Patriots earning the title, later became allegations against the Patriots for the deflation of eleven out of twelve footballs. In my opinion the deflation of the footballs has relation to the Ideal Gas Law. Footballs contain volume and pressure, the pressure in the ball helps the player to grip the ball, the volume helps the ball travel through the air. With a little less pressure the ball would be easy to grip or catch, even throw. An ideal gas law describes the relationship between ideal gases. “the volume of a gas depends solely on the number of moles of its molecules, not on the...
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...Character Count: Hours Dedicated: Federal Law - Federal Leasing In order for the Department of Interior (DOI) to decide which public lands will become available for oil and gas leasing the Bureau of Land Management (BLM), an agency within the DOI must conduct a Resource Management Plan (RMP) guide the BLM in deciding how to best use federal lands. An employee of the BLM known as the “Field Manager” is tasked with preparing the plan. The steps to create and finalize a RMP are: * Use input from the public, Federal agencies, State & local governments and Indian tribes to identify potential issues. * Develop the criteria for the plan, which the BLM will make public before it is approved for used in the planning process. * Collect data and information relevant to the plan goals. * Analyze data to provide the basis for formulating reasonable land use alternative, including the types of resources to be developed or protected. * Formulate and estimate the effects of reasonable resources management alternatives. * The Field Manager will then evaluate and identify a preferred alternative, which will then be submitted to the State Director for approval, publication and filing with the EPA. The draft will also be submitted for comment to various federal, state and local agencies and governments of the affected area as well as the Governor of the state involved. * The Field Manager then evaluates all comments and submits to the State Director a proposed...
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...------------------------------------------------- Submitted to: ------------------------------------------------- Waperi,Evelyn P. ------------------------------------------------- ------------------------------------------------- My Learning Log 3rdGrading Period On November- December we tackle all about changes in matter and Gases. First we discuss about skill 2.1 convert number of roles to mass or vice versa and to the number of particles (atoms, ions, molecules) or vice versa. Second on Nov. 18, 2013 we tacle about skill 2.2 Derive the chemical formula of a compound given the mass ratio and the atomic masses of the elements present. Third on Nov. 19, 2013 we discuss about skill 2.3 Explain the law of conservation of mass. ( Empirical formula, Molecular formula and mass, mole, g/mole). Next on Nov.26, 2013 we discuss about determining the formula from percentage composition. And then on Nov. 26,2013 we discuss types of Chemical Reaction which is Combination, Decomposition, Single replacement and Double replacement . and we discuss also about explain the implied information derived from balanced equation. After we discuss all about changes in matter, we discuss all about changes, energy, and time. First discuss is all about Differentiate exothermic and endothermic reactions, which is the exothermic process ( releases beat while the endothermic process absorbs heat. ...
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...constant-volume gas thermometer, T L L0 T V V0 T in kelvins (17.4) linear thermal expansion for solids volume thermal expansion for liquids of mass m (17.6) (17.12) (17.13) (17.18) (17.20) Q mc T Q nC T heat required for temperature change T heat required for temperature change of n moles heat transfer in a phase change Σ������ ������������ = 0 for an isolated system. Q mL H T T dQ kA H C dt L heat current in conduction ������ = ������ Σ (������ /������ ) when there are several layers. ������ ������ ������ Δ������ H Ae T 4 heat current in radiation (17.25) H net Ae T 4 Ae Ts 4 Ae T 4 Ts 4 (17.26) Copyright © 2012 Pearson Education, Inc. Page 1 of 7 Chapter 18 mtotal nM total mass, number of moles, and molar mass pV nRT (18.2) (18.3) (18.8) ideal-gas equation M NAm molar mass, Avogadro’s number, and mass of a molecule K tr 3 nRT 2 average translational kinetic energy of n moles of ideal gas 3 kT 2 (18.14) 1 m 2 2 av average translational kinetic energy of a gas molecule root-mean-square speed of a gas molecule (18.16) rms 2 av 3kT 3RT m M (18.19) tmean V 4 2r 2 N mean free path of a gas molecule (18.21) CV 3 R 2 ideal gas of point particles (18.25) CV 5 R 2 diatomic gas, including...
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...73, 75 & 82. Gas Properties 1. 2. 3. 4. Gases are highly compressible where liquids and solids are not. Gases occupy full volume of the container. Gases always form homogenous mixtures. In gases, there is spaces between gaseous molecules. 5. 1 Pressure Pressure = Force - N Area – m2 in Pascals (SI units) Pressure is measured using pressure gauges or diaphragm gauges. Atmospheric Pressure at sea level is 1 atm = 760 mm = 760 torr = 1.01 x 105 Pascals 5.2 The Gas Laws of Boyle, Charles, and Avogadro Boyle’s Law Measured pressure vs. volume. Pressure and Volume are indirectly proportional P = K 1/V At constant temperature, following relationship can be written as P1V1 = P2V2 P1V1 = P2V2 Charle’s Law Measured volume vs. temperature. Volume and temperature are directly proportional. V = K T where temperature is in Kelvin At constant pressure, following relationship can be written as V1 = V2 T1 T2 If you extrapolate the linear relationship between temp and volume down to volume equals to zero, you’ll get T = -273 oC also known as Absolute Zero equivalent to Zero Kelvin. The Effects of Increasing the Temperature of a Sample of Gas at Constant Pressure Avogadro’s Law Equal number of molecules occupy equal volumes at same temperature and pressure. V = K. n where n is number of moles At constant temperature and pressure, following relationship can be written as V1 = V2 n1 n2 These Balloons Each Hold 1.0 L of Gas at 25 Celsius and...
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...Titlle: Evaluation of Gas Law Constant. Objective: To experimentally determine the value of the universal gas constant , R. Theory / Background : The ideal gas law equation is expressed as PV=nRT and is used in most problems dealing with changes situations involving gases. This law can be used to approximate the behaviour of various gases under many situations with a few limitations. The term PV = nRT is also called the compression factor and is a measure of the ideality of the gas. An ideal gas will always equal 1 when plugged into this equation. The greater it deviates from the number 1, the more it will behave like a real gas rather than an ideal. A few things should always be kept in mind when working with this equation are: * Pressure is directly proportional to number of molecule and temperature. (Since P is on the opposite side of the equation to n and T) * Pressure, however, is indirectly proportional to volume. (Since P is on the same side of the equation with V) In this experiment, we will be using this law to evaluate R, the gas law constant. If R is to be determined in this experiment, the other parameters of P, V, n and T must also be available in this experiment. From this experiment known amount of Magnesium used and the stoichimometry of reaction the number of moles of hydrogen can be calculated. Mg(s) + 2 HCl MgCl2 + H2 Hydrogen collected in the eudiometer tube. So, the gas pressure in the tube after the reaction ceased...
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...Ideal gas behaviour (PV = nRT) Boyle’s Law, Charles’s Law, Dalton’s Law, Avogadro’s Law Real gases and its deviation Kinetic molecular theory of gases 1 2 THREE STATES OF MATTER Chapter Scopes Liquid States Kinetic-molecular theory (melting, vaporization & vapor pressure) 3 General Properties of Gases Properties of Gases • There is a lot of “free” space in gases • Gases can be expanded infinitely • Gases occupy containers uniformly & completely • Gases diffuse & mix rapidly Gas properties can be modeled using math which depends on: • V = volume of the gas (L or dm3) • T = temperature (K) • n = amount (mol) • P = pressure (atm) 5 FHSC1114 Physical Chemistry 4 6 1 Centre for Foundation Studies, UTAR Boyle’s Law Unit of Pressure & Volume • Unit of Pressure: The effect of pressure on gas volume 1 atm = 760 mm Hg = 101325 Pa (Nm-2) = 101.325 kPa = 1.013 bar = 760 torr P 1 V inversely proportional PV constant • Unit of Volume: PV1 P V2 1 2 1 dm3 = 1 L 1 m3 = 103 dm3 = 106 cm3 at constant n and T 7 Example 1: Boyle’s Law 8 Solution: A sample of CO2 has a pressure of 55 mm Hg in a volume of 125 mL. The sample is compressed to the new pressure 78 mm Hg. What is the new volume? Boyle’s Law: P1V1 P2V2 at cons tan t n and T P1 = 55 mm Hg , V1 = 125 mL P2 = 78 mm Hg , V2 = ? 9 10 Charles’s Law Example 2: Charles’s Law The...
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...Avogadro's Law Chemistry Avogadro's Law Experiment 1 1. For each gas, record the following: a Name and formula b Mass of 100 mL gas (g) c Molecular weight of the gas (g/mole) d Number of moles in the 100 mL sample 2. To verify Avogadro's Law, calculate the average number of moles for the three gases along with the percent deviation for each gas, according to the formula: % deviation = |(moles of gas) - (average for all gases)| / (average for all gases) * 100% a Average number of moles in 100 mL for all three gases b % deviation for each gas c Do your results confirm Avogadro's Law? 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 * 10^23 molecules/mole) 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 at STP can vary depending on the gas. How many atoms are there in one mole of methane (CH4) 6. In this experiment, the pressure (P) was 1 atm, the temperature (T) was 295 K, the volume (V) was 0.150 L, and the number of moles (n)was 6.2 * 10^-3 moles. The ideal gas law states that P*V = n*R*T. Based on your experiment, what value do you get for R? Is your value close to the standard value for R (0.082057 L*atm/K*mol) 7. In a real gas (non-ideal gas) the molecules can interact with...
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...Experiment: Avogadro’s Law Type Your Name: Date: 11/17/13 Experiment 1 ________________________________________ 1. For each gas, record the following: Propane Butane Methane a Name and formula C3H8 C4H10 CH4 b Mass of 100 mL gas (g) 0.274g 0.361g 0.100g c Molecular weight of the gas (g/mole) 44.10g/mol 58.12g/mol 16.04g/mol d Number of moles in the 100 mL sample 0.0062mol 0.0062mol 0.0062mol Average of all 3 gases: (0.0062+0.0062+0.0062) / 3 = 0.0062 2. To verify Avogadro's Law, calculate the average number of moles for the three gases along with the percent deviation for each gas, according to the formula: % deviation = |(moles of gas) - (average for all gases)| / (average for all gases) * 100% %deviation= (0.0062 -0.0062) mol / 0.0062mol *100% % deviation= 0% a Average number of moles in 100 mL for all three gases 0.0062moles b % deviation for each gas All 3 the same: 0% c Do your results confirm 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 at STP can vary...
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... gas Pressure – continual bombardment on the walls of a container by gas molecules in rapid, random motion Two units used to measure pressure: 1. millimeters of mercury (mm Hg) 2. atmospheres (atm) 1 atm = 760 mm Hg barometer – instrument used to measure atmospheric pressure manometer – instrument used to measure pressure of a gas in a container Boyle’s Law – for a fixed mass of an ideal gas at constant temperature, the volume of the gas is inversely proportional to the applied pressure. P1V1 = P2V2 Charles’s Law – the volume of a fixed mass of an ideal gas at a constant pressure is directly proportional to the temperature in kelvins (K). V1 = V2 T1 = T2 Gay-Lussac’s Law – for a fixed mass of a gas at constant volume, the pressure is directly proportional to the temperature in kelvins (K). P1 = P2 Combined Gas Law – P1V1 = P2V2 T1 T2 Avogadro’s Law – equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. standard temperature and pressure (STP) = 0 °C (273 K) and 1 atm One mole of any gas at STP occupies a volume of 22.4 L. Ideal Gas Law: PV = nRT P = pressure of gas (atm) V = volume of gas (L) n = amount of gas (moles) T = temperature of gas (K) R = ideal gas constant (0.0821 L x atm/mole x K Dalton’s law of partial pressures: The partial pressure of a gas in a mixture is the pressure that gas would exert if it were alone...
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...Experiment 1 Avogadro’s Law Multiple Choice Questions 1. How many atm of gas did you add to the flask? A. 1 atm B. 3 atm C. 4 atm D. 2 atm 2. What was the volume of the flask? E. 100 mL F. 120 mL G. 150 mL H. 88 mL 3. How many grams of propane were there in 1 atm? Choose the closest answer. I. 0.735 g J. 0.274 g K. 0.664 g L. 0.232 g 4. How many grams of butane were there in 1 atm of gas? Choose the closest answer. M. 0.774 g N. 0.361 g O. 0.664 g P. 0.214 g 5. How many grams of methane were in 1 atm of gas? Choose the closest answer. Q. 0.244 g R. 0.337 g S. 0.637 g T. 0.100 g 6. The molecular weight of propane is 44.10 g/mol. Based on the number of grams of gas measured, how many moles is this? (moles = mass / molecular weight) Choose the closest answer. U. 6.2 * 10^-3 moles V. 9.8 * 10^-2 moles W. 5.2 * 10^-3 moles X. 4.1 * 10^-3 moles 7. The molecular weight of butane is 58.14 g/mol. Based on the number of grams of gas measured, how many moles is this? (moles = mass / molecular weight) Choose the closest answer. Y. 8.1 * 10^-4 moles Z. 9.4 * 10^-2 moles [. 6.2 * 10^-3 moles \. 5.5 * 10^-1 moles 8. The molecular weight of methane is 16.04 g/mol. Based on the number of grams of gas measured, how many moles...
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