Combined Gas Law P1V1 = P2V2 N Is Constant T Always in K No Mass Or Moles Given T1 T2

Total Page：16

File Type：pdf, Size：1020Kb

Combined Gas Law P1V1 = P2V2 N Is Constant T Always in K No Mass Or Moles Given T1 T2

Gas Laws Summary Table Definitions: P = pressure n = # of moles V = volume R = gas constant (0.0821 L•atm/mol•K); this is the most common one T = temperature (in Kelvin always for gas laws!) molar volume: 1 mol/22.4 L or 22.4L/1 mol of any gas at STP STP: standard temperature = 00C or 273 K K = 0C + 273 standard pressure = 1 atm = 760 mm Hg = 760 torr = 101.3 kPa M = Molar Mass (on Ref. Tables packet M is molarity – it is italicized!!) Name Formula Special Conditions; Special Notes Regarding Some Examples of Other information Units Key Words in or missing from word Problems Combined Gas Law P1V1 = P2V2 n is constant T always in K no mass or moles given T1 T2 Boyle’s Law P1V1 = P2V2 n and T are constant consistent units for T is constant or not PV = k inverse relationship pressure and volume mentioned; no mass or P↑V↓ and P↓V↑ moles given Charles’ Law V1 = V2 n and P are constant T always in K P is constant or not direct relationship V1/T1 = k T1 T2 consistent units for V mentioned; no mass or V↑T↑ and V↓T↓ moles given Gay-Lussac’s Law P1 = P2 n and V are constant T always in K V is constant or not direct relationship P1/T1 = k T1 T2 consistent units for P mentioned; no mass or P↑T↑ and P↓T↓ moles given Dalton’s Law of Partial Pressures PT = P1 + P2 + P3 +… sum of partial pressures consistent units for P partial pressure – sum of all gases in a fixed of them or find one of container them given PT Special Case of Dalton’s Law Patm = Pg + PH2O use for collection of a consistent units for P pressure of a dry gas gas over water collected over water Graham’s Law of Effusion rate of gas A = √M of gas B M is the molar mass NO Units – this is a ratio ratio of speed, effusion, rate of gas B √M of gas A (from periodic table) or comparison diffusion; comparison of (notice diatomics!) 2 gases Ideal Gas Law PV = nRT only R is constant units used must be moles or mass is given must use R value consistent with R; or to be found in the consistent with usually P in atm; V in L; problem pressure units T always in K! Gas Density at STP D = Molar Mass can only use at STP usually in g/L for gases find density or molar Molar Volume (standard conditions) mass when given density at STP Gas Density NOT at STP D = PM must use when usually in g/L for gases find gas density or RT conditions are not at molar mass when given STP density **Highlighted Info Given in NCDPI Reference Tables** .

Copy Link

Recommended publications

Molar Volume of a Gas
Science Enhanced Scope and Sequence – Chemistry Molar Volume of a Gas Strand Molar Relationships Topic Investigating molar volume of a gas Primary SOL CH.4 The student will investigate and understand that chemical quantities are based on molar relationships. Key concepts include a) Avogadro’s principle and molar volume; b) stoichiometric relationships. Related SOL CH.1 The student will investigate and understand that experiments in which variables are measured, analyzed, and evaluated produce observations and verifiable data. Key concepts include a) designated laboratory techniques; b) safe use of chemicals and equipment; f) mathematical and procedural error analysis; g) mathematical manipulations including SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, and dimensional analysis. CH.2 The student will investigate and understand that the placement of elements on the periodic table is a function of their atomic structure. The periodic table is a tool used for the investigations of h) chemical and physical properties. CH.3 The student will investigate and understand how conservation of energy and matter is expressed in chemical formulas and balanced equations. Key concepts include b) balancing chemical equations. CH.5 The student will investigate and understand that the phases of matter are explained by kinetic theory and forces of attraction between particles. Key concepts include a) pressure, temperature, and volume; b) partial pressure and gas laws; c) vapor pressure. Background Information Avogadro’s law says that the volume of one mole of any gas at standard temperature and pressure is 22.4 liters. This is a necessary concept for the completion of stoichiometric problems that involve the use of gases as reactants or products.
[Show full text]
Research Article Densities, Apparent Molar Volume, Expansivities, Hepler's Constant, and Isobaric Thermal Expansion Coefficien
Hindawi International Journal of Chemical Engineering Volume 2018, Article ID 8689534, 10 pages https://doi.org/10.1155/2018/8689534 Research Article Densities, Apparent Molar Volume, Expansivities, Hepler’s Constant, and Isobaric Thermal Expansion Coefficients of the Binary Mixtures of Piperazine with Water, Methanol, and Acetone at T = 293.15 to 328.15 K Qazi Mohammed Omar ,1 Jean-Noe¨l Jaubert ,2 and Javeed A. Awan 1 1Institute of Chemical Engineering and Technology, Faculty of Engineering and Technology, University of the Punjab, Lahore, Pakistan 2Université de Lorraine, Ecole Nationale Supérieure des Industries Chimiques, Laboratoire Réactions et Génie des Procédés (UMR CNRS 7274), 1 rue Grandville, 54000 Nancy, France Correspondence should be addressed to Jean-Noe¨l Jaubert; [email protected] and Javeed A. Awan; javeedawan@ yahoo.com Received 11 May 2018; Revised 26 July 2018; Accepted 2 September 2018; Published 14 November 2018 Academic Editor: Gianluca Di Profio Copyright © 2018 Qazi Mohammed Omar et al. 2is is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited. 2e properties of 3 binary mixtures containing piperazine were investigated in this work. In a first step, the densities for the two binary mixtures (piperazine + methanol) and (piperazine + acetone) were measured in the temperature range of 293.15 to 328.15 K and 293.15 to 323.15 K, respectively, at atmospheric pressure by using a Rudolph research analytical density meter (DDM 2911). 2e concentration of piperazine in the (piperazine + methanol) mixture was varied from 0.6978 to 14.007 mol/kg, and the concentration of piperazine in the (piperazine + acetone) mixture was varied from 0.3478 to 1.8834 mol/kg.
[Show full text]
The Molar Volume of a Gas
THE MOLAR VOLUME OF A GAS OBJECTIVE: To calculate the standard molar volume of a gas from accumulated data INTRODUCTION Solids, liquids and gases are called the three states of matter. In this experiment, we will examine the gaseous state. The "condition" or state of a gaseous substance is determined by four properties: volume (V), pressure (P), temperature (T), and the number of moles of the substance present (n). A change in one variable causes a change in one or more of the other variables. If any 3 of the variables are known, the fourth can be calculated using the ideal gas law: PV = nRT (1) where R is a constant determined from experiment. It is called the universal gas constant. One mole of any gas at 0.00EC (273 K) and 1.00 atm (760 torr) occupies a volume of 22.4 L. These conditions are called standard temperature and pressure, or STP, and 22.4 L is called the standard molar volume. Using this data, R can be calculated: R = PV = (1.00 atm)(22.4 L) = 0.0821 L@atm (2) nT (1.00 mol) (273 K) mol@K If the number of moles of gas is constant, another useful relationship is the combined gas law: P1V1 = P2V2 (3) T1 T2 If P, V and T are known under an initial set of conditions and 2 of the conditions change, the change in the third can be calculated. For example, if a sample of 0.0500 moles of a gas occupies a 1.42 L container at 298 K and 654 torr, the volume it will occupy at 323 K and 985 torr is: (654 torr)(1.42 L) = (985 torr)(V2) (4) 298 K 323 K V2 = (654 torr)(1.42 L)(323 K) = 1.02 (5) (985 torr)(298 K) The volume occupied by 1 mole of gas under these nonstandard conditions would be: (1.02 L) = 20.4 L/mol (6) (0.050 mol) Note: Pressure units do not have to be changed to atm, as long as the units cancel out.
[Show full text]
Simple Mixtures
Simple mixtures Before dealing with chemical reactions, here we consider mixtures of substances that do not react together. At this stage we deal mainly with binary mixtures (mixtures of two components, A and B). We therefore often be able to simplify equations using the relation xA + xB = 1. A restriction in this chapter – we consider mainly non-electrolyte solutions – the solute is not present as ions. The thermodynamic description of mixtures We already considered the partial pressure – the contribution of one component to the total pressure, when we were dealing with the properties of gas mixtures. Here we introduce other analogous partial properties. Partial molar quantities: describe the contribution (per mole) that a substance makes to an overall property of mixture. The partial molar volume, VJ – the contribution J makes to the total volume of a mixture. Although 1 mol of a substance has a characteristic volume when it is pure, 1 mol of a substance can make different contributions to the total volume of a mixture because molecules pack together in different ways in the pure substances and in mixtures. Imagine a huge volume of pure water. When a further 1 3 mol H2O is added, the volume increases by 18 cm . When we add 1 mol H2O to a huge volume of pure ethanol, the volume increases by only 14 cm3. 18 cm3 – the volume occupied per mole of water molecules in pure water. 14 cm3 – the volume occupied per mole of water molecules in virtually pure ethanol. The partial molar volume of water in pure water is 18 cm3 and the partial molar volume of water in pure ethanol is 14 cm3 – there is so much ethanol present that each H2O molecule is surrounded by ethanol molecules and the packing of the molecules results in the water molecules occupying only 14 cm3.
[Show full text]
CHEMISTRY 111 LECTURE EXAM I Material
CHEMISTRY 111 LECTURE EXAM I Material Chapter 5 (pages 178-216) I. Properties of gases II. Measurements-Review force A. Pressure = Unit area 1. Conversions: ` 1 atm= 760 mm Hg = 760 torr (exactly) 1.013 x 105 Pa= 1 atm = 14.68 psi 2. Barometer 3. Manometer B. Temperature - Kelvin K = ºC + 273 C. Volume 1. The volume of a gas is the volume of the container it occupies. 2. Units: liters or milliliters III. RELATIONSHIP BETWEEN oT, VOLUME, AND PRESSURE.-Review A. Boyle's law P & V As the pressure increases the volume decreases in the same proportion. B Charles's law ºT & V As the temperature (Kelvin) is increased the volume is increased proportionally. C Gay-Lussac's Law When temperature (K) increases pressure increases proportionally. D Avogadro’s Law: Volume and Amount (in moles, n) When the amount (moles,n) increases volumne increases proportionally. E. COMBINATION OF THE GAS LAWS-Review: P, V, and oT varying. Assume that the mass is constant. Prob: A certain mass of gas occupies 5.50 L at 34ºC and 655 mm Hg. What will its volume in liters be if it is cooled to 10.0oC and its pressure remains the same? E. GAY-LUSSAC'S LAW OF COMBINING VOLUMES-Review: At the same oT and Pressure, the volumes of gases that combine in a chemical reaction are in the ratio of small whole numbers. Page 1 F. IDEAL GAS EQUATION-Review: Derivation: KNOW: PV=nRT Where: n = moles of gas R = 0.0821 L-atm mole-K 1. What volume in liters will be occupied by 6.00 mol carbon dioxide gas at 105 mm Hg and 28ºC? G MOLAR VOLUME at Standard Temperature and Pressure-Review: At the same temperature and pressure the same number of moles of different gases have the same volume.
[Show full text]
Molar Volume of a Gas/Calculation of R Name______Lab Period ______Date______I
Molar Volume of a Gas/Calculation of R Name_____________________ Lab Period ______Date__________ I. Introduction The molar volume of a gas is defined as the volume occupied by one mole of gas at standard temperature and pressure (STP). The theoretical value for the molar volume of an ideal gas at standard conditions is 22.4 L/mol. Since this is the volume occupied by one mole, it follows that the volume contains Avogadro’s number of molecules. The mass in the molar volume would be equal to the molecular mass of the gas in grams. When magnesium metal reacts with hydrochloric acid, hydrogen is produced. The gas can be collected in a graduated cylinder where its volume may be determined. Knowing the number of moles of magnesium used, we can calculate the volume of hydrogen produced per mole of magnesium consumed. The balanced equation for this reaction allows us to determine the volume of one mole of gas at standard temperature and pressure. After completing this experiment, you should be able to determine the molar volume of a gas. You will also collect this gas by water displacement and make a standard pressure and temperature comparison to the actual value. II. Pre-Lab Disscussion 1. Write a balanced equation for the reaction between hydrochloric acid and magnesium. III. Purpose The purpose is to experimentally determine the molar volume of hydrogen gas at standard temperature and pressure using Dalton’s Law of Partial Pressure and the Combined Gas Law. IV. Materials and Equipment safety goggles thermometer hydrochloric acid (6 M HCl) 25 mL graduated cylinder magnesium ribbon (Mg) 400 mL beaker V.
[Show full text]
Determining a Molar Volume a Safer Experiment SCIENTIFIC
Determining a Molar Volume A Safer Experiment SCIENTIFIC Introduction The traditional method for calculating molar volumes involves generating oxygen gas—potassium chlorate is heated with manganese dioxide, a catalyst, to produce oxygen gas. This method is quite hazardous because large amounts of oxygen gas are produced and potassium chlorate is a powerful oxidizer of organic materials including the rubber stopper used in the set-up. In fact, potassium chlorate is a frequent source of accidents on school premises. An easier and safer method pre- sented in this laboratory activity for the calculation of molar volumes involves the use of carbon dioxide instead of oxygen gas. Concepts • Mole • Molar volume • Ideal gas law Materials 3 Dry ice, solid carbon dioxide, CO2, small piece about ⁄4 square Graduated cylinder, 500-mL Balance Rubber stopper, to fit Erlenmeyer flask Barometer Thermometer Erlenmeyer flask, Pyrex®, 125-mL Tongs or insulated gloves (Zetex™) Safety Precautions This activity requires the use of hazardous components and/or has the potential for hazardous reactions. Dry ice can cause frostbite; never touch dry ice directly with the skin; wear appropriate insulated gloves or use tongs whenever handling dry ice. Do not stopper the flask until all of the dry ice has sublimed. Failure to wait until all solid pieces are gone may cause the flask to shatter due to increased pressure. Wear chemical splash goggles, chemical-resistant gloves, and a chemical-resistant apron. Please review current Material Safety Data Sheets for additional safety, handling, and disposal information. Procedure 1. Place the stopper in the Pyrex Erlenmeyer flask and mass to the nearest 0.01 g.
[Show full text]
Gases Chapter 9
Gases Chapter 9 What parameters do we use to describe gases? pressure: force/unit area 1 atm = 101 kPa; volume: liters (L) Temperature: K Amount of gas: moles A gas consists of small particles that move rapidly in straight lines until they collide; they have enough kinetic energy to overcome any attractive forces; gas molecules are very far apart; gas molecules have very small volumes compared to the volumes of the containers they occupy; have kinetic energies that increase with an increase in temperature; collisions of the gas cause pressure (force /unit area) What is meant by % volume? In principle, the actual molecular volume of a gas is so small in comparison to the volume it will occupy that we treat gases at mathematical points. What is air pressure due to? A column of air 1 m2 has a mass of 10,300 kg, producing a pressure of 101 kPa due to gravity (14.7 pounds/in2) 1 atm = 76 cm Hg; 101 kPa Atmospheric pressure is the pressure exerted by a column of air from the top of the atmosphere to the surface of the Earth; Pressure is: about 1 atmosphere at sea level; depends on the altitude and the weather; is lower at high altitudes where the density of air is less; How do we measure pressure? A barometer measures the pressure exerted by the gases in the atmosphere indicates atmospheric pressure as the height in mm of the mercury column A water barometer would be 13.6 times taller than a mercury barometer because the density of Hg is 13.6 times as dense as water • What is the relationship between the variables used to describe gases? Boyle’s
[Show full text]
Chemistry 230 Problem Set # 11 — 11/10/99 Recommended Problems: Chapt. 9: 1-5, 8-12, 14-16, 19, 20, 29, 35, 39, 53, 63-65 1
Chemistry 230 Problem Set # 11 — 11/10/99 Recommended Problems: Chapt. 9: 1-5, 8-12, 14-16, 19, 20, 29, 35, 39, 53, 63-65 1. 4.45 g of 100% sulfuric acid is added to 82.20 g of water, and the density of the solution is found to be 1.029 g/cm3 at 25˚C and 1 atm. Treating the acid as solute, calculate (a) the weight per cent; (b) the mole fraction; (c) the mole per cent; (d) the molality; and (e) the molarity of the solution. 2. The partial molar volume ` VB of K2SO4 in aqueous solutions at 25˚C is given by ` VB (cm3/mol) = 32.280 + 18.216 m1/2 + 0.0222 m, where m is the molality of the solution. For water at this temperature, Vm = 18.068 cm3/mol. (a) Obtain an equation for the total volume V of a solution containing 1.000 kg of H2O. (b) Obtain an equation fot the partial molar volume ` VA of water. [Hint: See Problem 9.22 in Levine.] 3. The molar enthalpy of mixing for forming solid solutions of NaCl and NaBr at 25˚C as a function of the mole fraction x of NaBr is given by DHmix,m(kJ/mol) = 5.996 x – 6.761 x2 + 0.765 x3 . (a) Calculate DH for mixing 1.000 mol of each component to form 2.000 mol of solution. (b) Calculate the differential heats of solution for each component in the 50.0 mole per cent solution. 4. Benzene and hexane form nearly ideal solutions.
[Show full text]
Density and Molar Volume
Molar Volume We have already investigated the relationship between mass, mole and the number of particles. But, is there any relationship between volume and mass, or mole and number of particles? Lets investigate. Purpose: Determine if there is a mathematical relationship between the mole and molar volume. Q1. If the molar mass (g/mole) is divided by the density (g/mL), what units remain? Q2. What would be an appropriate name for measurements having units in moles per mL? DIRECTIONS FOR TI-82/83 o Clear all equations Set up the Ö EDIT table with the following data: Construct a scatter plot of density versus molar mass L1=Molar Mass (g/mol) for the elements listed below. L2=Density (g/mL) y o Plots Off Plot1 ON " Xlist=L1 Ylist=L2 q ZoomStat Substance Molar Mass Density Al 27.0 g/mol 2.7 g/mL Fe 55.9 g/mol 7.9 g/mL Cu 63.5 g/mol 8.9 g/mL Zn 65.4 g/mol 7.1 g/mL Mo 95.4 g/mol 8.6 g/mL Zr 91.2 g/mol 4.5 g/mL Ag 107.9 g/mol 11.5 g/mL Ta 181 g/mol 13 g/mL Au 197.0 g/mol 19.3 g/mL Hg 200.6 g/mol 13.6 g/mL Sketch a simple diagram of the graph into your lab report. Q3. Does the data between molar mass and the density of the various metals seem to fit an easily recognized mathematical function? DIRECTIONS FOR TI-82/83 o Clear all equations Next, examine the following data for gases and Set up the Ö EDIT table with the following data: determine if there is a mathematical relationship L1=Density (g/mL) between the density of a gas and it’s molar mass.
[Show full text]
NOTES: 10.2 - Molar Volume, Density; and the Mole “Road Map”; NOTES: 10.3 Percent Composition What Is a MOLE?
NOTES: 10.2 - Molar Volume, Density; and the Mole “Road Map”; NOTES: 10.3 Percent Composition What is a MOLE? • VIDEO CLIP! Volume ↔ Mole Conversion: ● Conversion Factor: -1 mole of any gas at STP = 22.4 L -this is known as MOLAR VOLUME -”STP” = standard temperature (0oC) and standard pressure (1 atm) Mole Volume Calculations 1 mole = 22.4 L of gas at STP STP = standard temperature and pressure (0 °C & 1 atm) 22.4 L 1 mol Volume 1 mol 22.4 L Volume Example #1: Determine the volume, in liters, of 0.600 mol of SO2 gas at STP. 0.600mol SO 22.4L 2 1 mol 13.4L SO2 Volume Example #2: Determine the number of moles in 33.6 L of He gas at STP. 33.6L He 1 mol 22.4 L 1.50 mol He DENSITY: Density = Mass / Volume When given the density of an unknown gas, one can multiply by the molar volume to find the molar mass. The molar mass can then allow for identification of the gas from a list of possibilities. Density Example (part A): The density of an unknown gas at STP is 2.054 g/L. (a) What is the molar mass? density molar volume molar mass 2.054g 22.4L 46.01 g/mol L 1mol Density Example (part B): The density of an unknown gas is 2.054 g/L. (b) Identify the gas as either nitrogen, fluorine, nitrogen dioxide, carbon dioxide, or ammonia. molar mass = 46.0 g/mol (from part a) Nitrogen = N2 = 2(14.0) = 28.0 g/mol Fluorine = F2 = 2(19.0) = 38.0 g/mol Nitrogen dioxide = NO2 = 14.0 + 2(16.0) = 46.0 g/mol Carbon dioxide = CO2 = 12.0 + 2(16.0) = 44.0 g/mol Ammonia = NH3 = 14.0 + 3(1.0) = 17.0 g/mol Density Example #2: The density of a gaseous compound containing carbon and oxygen is 1.964 g/L at STP.
[Show full text]
Molar Volume and Molecular Weight of Gasses
Molar Volume and Molecular Weight of Gasses Molar Volume General Definition of Molar Volume In chemistry, the molar volume of a substance is the volume of one mole of that substance. It can be computed as the substance's molecular (or atomic) weight divided by its density. The SI unit for volume is the cubic meter, m3. Thus, the SI unit of molar volume is cubic meters per mole (m3 mol-1). Molar volume can also be expressed in cm3 mol-1. A cubic centimeter (cm3) is a measure of volume one million times smaller than a cubic meter. Numerical Definition of Molar Volume The molar volume for an ideal gas at STP is 22.414 L mol-1 Thus, one mole of an ideal gas at STP occupies 22.414 liters. This value has been known for about 200 years. The value is actually known to several more decimal places, but three decimal places will provide sufficient precision for our calculations. Using PV = nRT, you can calculate the value for molar volume of an ideal gas. V is the unknown, and n = 1 mol. Set P and T equal to their STP values, and use R = 0.08206 L atm mol-1 K-1. The Molecular Weight of Air The physical behavior of gases is described by various laws, which have resulted from hundreds of years of experimentation. Most general chemistry textbooks describe many applications of the ideal gas equation, PV = nRT. This equation provides a very useful, general description of the physical behavior of “ideal” gases. Although real gases rarely behave in a completely “ideal” manner, this equation will provide a good basis for the investigation you are performing in the laboratory this week.
[Show full text]