...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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...objective of this lab experiment is to measure the material in the gas phase and to see how the ideal gas experiment could apply to the physical. In this the material we used was, a sip-lock plastic bag, a large plastic beaker, thermometry, dry ice, water, and butane lighter. Introduction In this lab, the experiment focused on the relationship between the temperature and pressure of an ideal gas that was dry ice inside the closed container. Therefore, the volume remains constant because the ideal gas was in a closed container. Experiment Procedure First, all the materials were collected. After collecting all the materials was prepared, we started measuring the mass of the beaker and plastic zip-lock bag on the loading balance. After that, about 50 g of dry ice was transferred into the plastic bag and weighted the total mass and calculate the mass of carbon dioxide transferred. After that, the plastic bag was collected to inflate fully and the temperature of the gas was recorded. This was due to carbon dioxide present in the dry ice and after that we removed all the gas in the bag; mass of the bag and ice was measured again. The next lab experiment helps to determine the molecular weight of the gas. After obtaining the materials required, and the group member’s filled out the burette with water and inverted it. Then the room temperature and water temperature were recorded. A tube was then attached to butane lighter outlet and burette. The volume of the gas was inside the...
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...Lab Session 12, Experiment 11: Valence, the Combining Capacity of Elements and Molecules One molar mass of an element or compound that produces or reacts with 1.008 grams of hydrogen has a valence of I. It follows that the same quantity producing or reacting with 2.016 grams of hydrogen is valence II, and producing or reacting with 3.024 grams of hydrogen is valence III, etc. In this experiment, the magnesium metal will be reacted with concentrated hydrochloric acid to produce hydrogen gas according to the following chemical equation: Mg (sol) + x HCl (aq) → MgCl x (aq) + x H2 (gas) 2 The hydrogen gas produced will be collected, its volume measured, and the mass in grams calculated using the ideal gas law: PV = nRT When using this equation, the units of the gas constant (R) must be consistent with the units used for the other quantities in the equation. The Handbook of Chemistry and Physics lists the value of R as R = 0.08206 L × atm × mol –1 –1 ×K Thus, pressure (P) must be expressed in atmospheres, volume (V) in liters, and temperature (T) in Kelvin. 11A Experiment A sample of magnesium metal with an approximate mass of 0.24 grams will be reacted with excess hydrochloric acid. The hydrogen gas produced will be collected, its volume measured, and finally its mass in grams will be calculated. Chemicals Required: 6M hydrochloric acid Note: 12M HCl(aq) must be diluted. Apparatus Required: 500 mL Florence flask Glass tubing Watch...
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...Boyle's Law Examples in Real Life Boyle's Law Explained In 1662, Robert Boyle discovered that when held at a constant temperature, the volume and pressure of a gas are inversely proportionate. Put simply, when the volume goes up, pressure drops, and vice versa. The mathematic equation is equally as simple: PV=K where P=Pressure, V=Volume, and K is simply a constant. This has become a basic principle in chemistry, now called "Boyle's law" and is included as a special case into the more general ideal gas law. Spray paint uses a real life application of Boyle's law to work its magic. Spray Paint While there are a couple different types of aerosol cans, one being a little more elaborate than the other, they both operate off of the same basic principle: Boyle's law. We'll examine the more elaborate of the two, since it's far more popular. We know that before you spray a can of paint you are supposed to shake it up for a while, listening as a ball bearing rattles around inside. There are two substances inside the can, one being your product (paint for example), and the other being a gas that can be pressurized so much that it retains a liquid state even when it is heated past its boiling point. This liquefied gas will be a substance that has a boiling point far below room temperature. The can is sealed, preventing this gas from boiling and turning into a gaseous state. That is, until you push down the nozzle. The moment the...
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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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... Anid Ideal Gas Law Equation Group Members: Lazaro Tovar Corbin Mayer Alex Saint-Hailaire Objectives: To take data from the user and perform the calculations necessary to use the Ideal Gas Law, including Boyle’s Law, Charles’s Law, Gay-Lussac’s Law, and the Combined Gas Law. The user will answer a series of questions to have the program “determine” what equation will be necessary. The computer will then ask for the input variables and perform the calculations getting the answer. A series of prompt dialogue boxes will be used to help determine the user’s need. He will answer accordingly, and upon entering all pertinent data, the program will give an answer to the question. Background: Gasses have neither a defined shape nor volume, and as such are very sensitive to temperature and pressure. To relate these, there is a law of Chemistry called the Ideal Gas Law. “A gas is said to be “idea” if it behaves exactly as predicted”. This is expressed as PV=nRT, relating pressure, volume, number of moles, a constant value, and the temperature. It was built from several preceding laws. These would be Boyle’s Law, P1V1 = P2V2, Charles’s Law, V1/T1 = V2/T2 , Guy-Lussac’s Law, P1/T1 = P2/T2 , and the Combined Gas Law, P1V1 / T1= P2V2 / T2 . These helped pave the way for the Ideal Gas law, stated before. The Ideal Gas Law and corresponding laws are helpful for determining...
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...characteristics because it does not exactly follow the ideal gas law. In the ideal gas law, gas molecules are considered to have negligible volume and negligible intermolecular interactions (Averill and Eldredge, 2006). The ideal gas equation of state is not sufficient to describe the pressure, volume and temperature behavior of most real gases but real gases shows significant deviations from the behavior of an ideal gas. For real gases or non-ideal gases, the most common equation of states are shown below: Van der Waals: Berthelot: Redlich-Kwong: Dietirici: Virial: There are other equations of state that can be used to predict non-ideal gas behaviour and to incorporate a compression factor is another one. Compression factor, also known as compressibility factor is the ratio between molar volumes of a gas to the molar volume of a perfect gas. A perfect gas has a compression factor equal to 1 in all conditions so real gases deviates from that value. Another equation for compression factor is Fugacity is function of pressure and temperature where Φ is the fugacity coefficient, a dimensionless quantity that depends on the temperature, pressure and identity of a gas. Getting Φ from the equation would result to the ratio of the fugacity and the effective pressure. The fugacity coefficient approaches the value of 1 when the gas behaves like an ideal gas, so it is also a measure of non-ideality such as compression...
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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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...------------------------------------------------- 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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...Test 2 – AF202 Prep |Basic Anatomy Gas Laws | |Part 61 Certification Pilots, Flight Instructors and Ground Instructors | |.14—Refusal to submit to a drug or alcohol test | |.15—Offenses involving alcohol or drugs | |.16—Refusal to submit to an alcohol test or to furnish test results | |.23—Medical certificates: Requirement and duration | |.31g—Additional training required for operating pressurized aircraft capable of operating at high altitudes | |.53—Prohibition on operations during medical deficiency | |Part 67 Medical Standards & Certification | |Part 91 ...
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...CHM 1101 Introductory Chemistry Dawn Fox Medeba Uzzi August, 2007 Compiled and edited by Medeba Uzzi Authors’ Note This document is an initiative by the authors in an attempt to deal with what they think may be one of the reasons contributing to the relatively high failure rate in the introductory Chemistry course (CHM 1101) at the University of Guyana. It was brought to our attention that many first year students taking CHM 1101 are unable to efficiently cope with the frenetic pace of the Semester system and even less able to deal comprehensively with the large content in CHM 1101. It is hoped that by providing this paper, students will not need to make lots of notes in lectures and so they can focus on grasping the concepts taught. The document is meant to be a guide to the topics covered in CHM 1101 and is by no means exhaustive. Students are still required to attend classes regularly and punctually and to engage meaningfully in lectures and tutorials. Further, supplemental reading of these topics in any good General Chemistry text is expected. Dawn Fox Medeba Uzzi 2 SECTION 1 – Modules A – D: section deals with the foundation for chemistry. It introduces students to matter & its classification, Atom & its structure, Periodic table and chemical rxns. Introduction to Science and Measurement What is Chemistry? – Chemistry is the study of matter and its transformations Natural sciences refer to the systematic study of the natural world (our...
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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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...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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...CHEMISTRY 1031 (CHILDS) – STUDY GUIDE FOR EXAM II Tuesday October 14 BE 160 Exam II will cover the material I lectured on from chapters 4 and 5. You are also expected to retain material from chapters 1, 2, and 3. Everything covered in lecture is fair game for the exam. You will be provided with a periodic table, solubility rules, conversion factors and constants (similar to those at the back of the chapter.) The exam will contain a mixture of multiple choice questions similar to those assigned as homework and at the end of each chapter in the textbook. (The Practice Examples are within the chapter, the problems appear at the end of the chapter.) Students must have their Temple photo ID card during lecture exams. TU-ID Numbers must be correctly and completely filled in on exams to ensure your score is properly recorded. Students are not allowed to have cell phones and other PDA devices on their persons while taking an exam. Cell phones/PDAs are to be placed in bags/backpacks which will be kept at the back of the lecture hall. Students may leave cell phones/PDAs on the front bench of the lecture hall. Students who are caught using cell phones/PDAs during an exam will be ejected from the exam and will receive a score of zero. This violation will be reported to the Dean and the Vice-Provost who will then take the appropriate disciplinary action. Only pens/pencils and scientific calculators (non-programmable and non-graphing) are allowed to be with students during...
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