Vapor-Liquid Equilibria

Size: px
Start display at page:

Download "Vapor-Liquid Equilibria"

Transcription

1 31 Introduction to Chemical Engineering Calculations Lecture 7. Vapor-Liquid Equilibria

2 Vapor and Gas Vapor A substance that is below its critical temperature. Gas A substance that is above its critical temperature (but below the critical pressure). For the same pressure, a vapor is more easily condensed while a gas is normally non-condensable. 2

3 The PT Diagram 3

4 Definition of Terms Vapor Pressure Pressure of the vapor when the vapor and liquid of a pure component are in equilibrium. Also referred to as saturated pressure. Saturated Temperature Temperature at which the vapor and liquid will co-exist at a given pressure. Commonly referred to as the boiling or condensation point. Dew Point The temperature when the vapor starts to condense. Bubble Point The temperature when the liquid starts to vaporize. 4

5 Definition of Terms Saturated Vapor and Saturated Liquid Vapor and liquid at the saturated P and saturated T. Subcooled Liquid A liquid that is below its saturated T at a given pressure. Compressed Liquid A liquid that is above its saturated P at a given temperature. Superheated Vapor A vapor that is above its saturated T at a given pressure. Quality For a saturated mixture, quality refers to the mass fraction of the vapor in the mixture. 5

6 The PT Diagram 6

7 The PT Diagram 7

8 Saturated and Superheated Steam Tables 8

9 Properties of Saturated Mixture For a saturated mixture, V ˆ (1 x) V ˆ (x) Vˆ l g mixture H ˆ (1 x) H ˆ (x) Hˆ l g mixture U ˆ (1 x) U ˆ (x) Uˆ l g mixture where x = mass fraction of vapor in the mixture. 9

10 Example 7/8-1. Vapor-Liquid Properties of Water For each of the conditions of temperature and pressure listed below for water, state whether the water is a solid, liquid, saturated mixture, or superheated vapor. If it is a saturated mixture, calculate the quality. State P (kpa) T (K) V (m 3 /kg)

11 Example 7-1. Vapor-Liquid Properties of Water Using the saturated steam table, State P (kpa) T (K) Phase Liquid Vapor Vapor Saturated 11

12 Example 7-1. Vapor-Liquid Properties of Water From the saturated steam pressure table, By 2-point linear interpolation, properties at P = can be estimated: V ˆ m / kg and V ˆ m / kg l 3 3 g 12

13 Example 7-1. Vapor-Liquid Properties of Water If x is the quality of the saturated mixture, then m m m 1 x x kg kg kg Solving for x, x =

14 Change of Vapor Pressure with Temperature Many functional forms have been proposed to predict vapor pressure (p*) from temperature. One of these functions is the Antoine equation: B ln (p*) A C T Where p* = vapor pressure of the substance, mmhg T = temperature, K A, B, C = constants for each substance 14

15 Change of Vapor Pressure with Temperature The Clapeyron equation is another function relating vapor pressure p* and temperature T: dp* ĤV dt T(Vˆ V ˆ ) g l Where p* = vapor pressure of the substance T = temperature H V = latent heat of vaporization V g, V l = specific molar volumes of vapor and liquid, respectively 15

16 Change of Vapor Pressure with Temperature Simplifications of the Clapeyron equation: 1. Specific molar volume of liquid is very small compared to specific molar volume of the vapor, such that (Vˆ V ˆ ) Vˆ g l g 2. The vapor is assumed to behave ideally. ˆV g RT P * 16

17 Change of Vapor Pressure with Temperature The Clapeyron equation then becomes, dp* dt P* Hˆ RT 2 V Separating the variables and integrating to yield the Clausius-Clapeyron equation, dp* ĤV dt 2 P* R T Ĥ ln(p*) RT V B 17

18 Example 7-2. Estimation of Normal BP Using the Antoine Equation Determine the % error if the Antoine equation is used to estimate the normal boiling point of benzene. From literature value, the normal boiling point of benzene is K. Solution: For benzene, values of the constants for the Antoine equation are: A = B = C =

19 Example 7-2. Estimation of Normal BP Using the Antoine Equation Using the Antoine equation, ln (760 mmhg) T Solving for temperature, T = K The percent error is, K 353.3K % error % K 19

20 Example 7-3. Clausius-Clapeyron Equation The vapor pressure of benzene is measured at two temperatures, with the following results: T 1 = C T 2 = C P* 1 = 40 mm Hg P* 2 = 60 mm Hg Calculate the latent heat of vaporization and the parameter B in the Clausius-Clapeyron equation and then estimate P* at C using this equation. 20

21 Example 7-3. Clausius-Clapeyron Equation The Clausius-Clapeyron is a linear equation with: Solving for slope, m: 1 x y ln(p*) T Ĥ R V m b B m ĤV y ln(p* 2) ln(p* 1) T1 T2 ln(p* 2 /P* 1) R x 1 1 T1 T2 T2 T 1 21

22 Example 7-3. Clausius-Clapeyron Equation Using absolute values for temperature: T 1 = K and T 2 = K The slope is computed as: m m 60 mmhg K K ln ˆ 40 mmhg R K K HV Ĥ R V 4213K 22

23 Example 7-3. Clausius-Clapeyron Equation And the latent heat of vaporization is: J ĤV 4213K R 4213K , 030 molk J mol The intercept b (b = B) can be determined as follows: Hˆ B ln(p* ) ln(p* ) Hˆ V V 1 2 RT1 RT B ln(40)

24 Example 7-3. Clausius-Clapeyron Equation The Clausius-Clapeyron equation for benzene can now be written as: 4213 ln(p*) T At T = C = K, the vapor pressure of benzene is 4213 ln(p*) P* exp mmhg 24

25 Vapor-Liquid Equilibrium for Multi-component Systems Consider a binary mixture with components A and B. Vapor Y A (P A ) Y B (P B ) Liquid X A0 X B0 Heating Liquid X A X B Note: X, Y = mole fractions of the component in the vapor and liquid phases, respectively. 25

26 Vapor-Liquid Equilibrium for Multi-component Systems For multi-component systems, P i = f(x i ) This functional relationship is given by 1. Raoult s Law generally used when x i is close to Henry s Law generally used when x i is close to 0. 26

27 Vapor-Liquid Equilibrium for Multi-component Systems Henry s Law: P i = x i H i where P i x i H i = partial pressure of component i in the vapor phase. = y i P T (if the vapor behaves ideally) = mole fraction of component i in the liquid phase. = Henry s law constant 27

28 Vapor-Liquid Equilibrium for Multi-component Systems Raoult s Law: P i = x i P* i where P i x i P T = partial pressure of component i in the vapor phase. = y i P T (if the vapor behaves ideally) = mole fraction of component i in the liquid phase. = total pressure 28

29 Vapor-Liquid Equilibrium for Multi-component Systems If the vapor behaves ideally, the Raoult s law becomes Rearranging the equation, y i P T = x i P* i y x i i P * P T i K i where K i is the V-L equilibrium constant. 29

30 Example 7-4. Vapor-Liquid Equilibrium Calculation Suppose that a liquid mixture of 4.0% n-hexane (A) in n-octane (B) is vaporized. What is the composition of the first vapor formed if the total pressure is 1.00 atm? Values of the Antoine constants for n-octane are: A = B = C =

31 Example 7-4. Vapor-Liquid Equilibrium Calculation Solution: Assuming the vapor behaves ideally, the composition of the vapor is determined using the Raoult s law: y y A B P * P T P * P T A B x x A B 31

32 Example 7-4. Vapor-Liquid Equilibrium Calculation Upon formation of the first vapor, the composition of the liquid is essentially the same as the initial composition. Hence, x A = and x B = 1 x A =0.960 The vapor pressures of A and B are calculated using the Antoine equation: B ln (P*) A C T 32

33 Example 7-4. Vapor-Liquid Equilibrium Calculation For n-hexane: P* A exp T For n-octane: P* B exp T Since vaporization temperature is not given, the next step in the calculation is to determine its value. 33

34 Example 7-4. Vapor-Liquid Equilibrium Calculation For the vapor mixture, Using Raoult s Law, P T = P A + P B P T = P* A x A + P* B x B = 1.00 atm = 760 mmhg Using the expressions for the vapor pressures as defined by the Antoine equation T 63.63T e e

35 Example 7-4. Vapor-Liquid Equilibrium Calculation The last equation is a non-linear equation. To find the value of T, Newton s method is used by defining f(t) as: T 63.63T f(t) = 0.040e 0.960e Similar to example 6-4, the temperature value that will satisfy this equation is determined using the following iteration formula: T k1 Tk f (T k ) f '(T ) k 35

36 Example 7-4. Vapor-Liquid Equilibrium Calculation Differentiating f(t): f '(T) T 63.63T e e = T T Any value for the temperature may be used as initial guess. For this example, the following initial guess is used: T 0 = 1000 K 36

37 Example 7-4. Vapor-Liquid Equilibrium Calculation Step T K (K) f(t) f'(t) T K+1 (K) E

38 Example 7-4. Vapor-Liquid Equilibrium Calculation For T = K, the vapor pressures of n-hexane and n-octane are: P* A = mm Hg P* B = mm Hg And the composition of the first vapor formed is: y y A B

39 Vapor-Liquid Equilibrium for Multi-component Systems Consider a mixture of a vapor (A) and a non-condensable gas (B). Gas Mixture Y A (P A ) Y B (P B ) Cooling Vapor Y A (P A ) Y B (P B ) Liquid X A 39

40 Vapor-Liquid Equilibrium for Multi-component Systems (Terms and symbols in parenthesis refer specifically to air-water system.) Relative Saturation (Relative Humidity) PV sr hr 100 P * Absolute Saturation (Absolute Humidity) V s a h a mass of vapor PVMWV massof vapor-free gas P P MW T V G Molal Saturation (Molal Humidity) s m h m moles of vapor PV molesof vapor-free gas P P T V 40

41 Example 7-5. Humidity of Air Humid air at 75 0 C, 1.1 bar, and 30% relative humidity is fed into a process unit at a rate of 1000 m 3 /h. Determine: a. the molar flow rates of water, dry air, and oxygen entering the process unit. b. the molal humidity and absolute humidity. c. the dew point. Assume ideal gas behavior. 41

42 Example 7-5. Humidity of Air Solution for (a): Determine the mole fraction of water: y P 2 H2O H O PT The partial pressure of water is calculated from relative humidity: P P* H2O h 100 r H2O 42

43 Example 7-5. Humidity of Air At T = 75 0 C, P* H2O = 289 mm Hg And the partial pressure of water is, P H2O = (289 mm Hg)(0.3) = 86.7 mm Hg For a total pressure of 1.1 bar = 825 mm Hg, the mole fraction of water is, 86.7 mm Hg mol H2O yh2o mm Hg mol HA 43

44 Example 7-5. Humidity of Air Determine the molar flow rate of humid air: 3 1.1bar 1000 m / h P V kmol na RT m bar h K kmol K The molar flow rate of water can now be obtained: kmol HA 0.105kmolH2O kmol H2O n H2O h kmol HA h 44

45 Example 7-5. Humidity of Air The molar flow rate of dry air: kmol kmol DA kmol DA n DA h kmol HA h The molar flow rate of O 2 : kmol DA 0.21kmol O kmol O n O h kmol DA h

46 Example 7-5. Humidity of Air Solution for (b): The absolute humidity (h a ): T H2O DA PH2O MWH2O kg H2O ha P P MW kg DA The molal humidity (h m ): PH2O 86.7 mol H2O hm P P mol DA T H2O 46

47 Example 7-5. Humidity of Air Solution for (c): At the dew point, P H2O = P* H2O = 86.7 mmhg From vapor pressure data for water, this vapor pressure of water occurs at: T = C This is the dew point since at this temperature, water will start to condense. 47

vap H = RT 1T 2 = 30.850 kj mol 1 100 kpa = 341 K

vap H = RT 1T 2 = 30.850 kj mol 1 100 kpa = 341 K Thermodynamics: Examples for chapter 6. 1. The boiling point of hexane at 1 atm is 68.7 C. What is the boiling point at 1 bar? The vapor pressure of hexane at 49.6 C is 53.32 kpa. Assume that the vapor

More information

Phase Equilibrium: Fugacity and Equilibrium Calculations. Fugacity

Phase Equilibrium: Fugacity and Equilibrium Calculations. Fugacity Phase Equilibrium: Fugacity and Equilibrium Calculations (FEC) Phase Equilibrium: Fugacity and Equilibrium Calculations Relate the fugacity and the chemical potential (or the partial molar Gibbs free energy)

More information

Chem 338 Homework Set #5 solutions October 10, 2001 From Atkins: 5.2, 5.9, 5.12, 5.13, 5.15, 5.17, 5.21

Chem 338 Homework Set #5 solutions October 10, 2001 From Atkins: 5.2, 5.9, 5.12, 5.13, 5.15, 5.17, 5.21 Chem 8 Homework Set #5 solutions October 10, 2001 From Atkins: 5.2, 5.9, 5.12, 5.1, 5.15, 5.17, 5.21 5.2) The density of rhombic sulfur is 2.070 g cm - and that of monoclinic sulfur is 1.957 g cm -. Can

More information

Thermodynamics. Chapter 13 Phase Diagrams. NC State University

Thermodynamics. Chapter 13 Phase Diagrams. NC State University Thermodynamics Chapter 13 Phase Diagrams NC State University Pressure (atm) Definition of a phase diagram A phase diagram is a representation of the states of matter, solid, liquid, or gas as a function

More information

Thermodynamics of Mixing

Thermodynamics of Mixing Thermodynamics of Mixing Dependence of Gibbs energy on mixture composition is G = n A µ A + n B µ B and at constant T and p, systems tend towards a lower Gibbs energy The simplest example of mixing: What

More information

Everest. Leaders in Vacuum Booster Technology

Everest. Leaders in Vacuum Booster Technology This article has been compiled to understand the process of Solvent Recovery process generally carried out at low temperatures and vacuum. In many chemical processes solute is to be concentrated to high

More information

CHAPTER 14 THE CLAUSIUS-CLAPEYRON EQUATION

CHAPTER 14 THE CLAUSIUS-CLAPEYRON EQUATION CHAPTER 4 THE CAUIU-CAPEYRON EQUATION Before starting this chapter, it would probably be a good idea to re-read ections 9. and 9.3 of Chapter 9. The Clausius-Clapeyron equation relates the latent heat

More information

So T decreases. 1.- Does the temperature increase or decrease? For 1 mole of the vdw N2 gas:

So T decreases. 1.- Does the temperature increase or decrease? For 1 mole of the vdw N2 gas: 1.- One mole of Nitrogen (N2) has been compressed at T0=273 K to the volume V0=1liter. The gas goes through the free expansion process (Q = 0, W = 0), in which the pressure drops down to the atmospheric

More information

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790. CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

More information

Chapter 7 : Simple Mixtures

Chapter 7 : Simple Mixtures Chapter 7 : Simple Mixtures Using the concept of chemical potential to describe the physical properties of a mixture. Outline 1)Partial Molar Quantities 2)Thermodynamics of Mixing 3)Chemical Potentials

More information

CHEM 36 General Chemistry EXAM #1 February 13, 2002

CHEM 36 General Chemistry EXAM #1 February 13, 2002 CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show

More information

Sample Test 1 SAMPLE TEST 1. CHAPTER 12

Sample Test 1 SAMPLE TEST 1. CHAPTER 12 13 Sample Test 1 SAMPLE TEST 1. CHAPTER 12 1. The molality of a solution is defined as a. moles of solute per liter of solution. b. grams of solute per liter of solution. c. moles of solute per kilogram

More information

Distillation vaporization sublimation. vapor pressure normal boiling point.

Distillation vaporization sublimation. vapor pressure normal boiling point. Distillation Distillation is an important commercial process that is used in the purification of a large variety of materials. However, before we begin a discussion of distillation, it would probably be

More information

= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm

= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular

More information

6. 2. Unit 6: Physical chemistry of spectroscopy, surfaces and chemical and phase equilibria

6. 2. Unit 6: Physical chemistry of spectroscopy, surfaces and chemical and phase equilibria 6. 2 Phase equilibria Many industrial processes involve several phases in equilibrium gases, liquids, solids and even different crystalline forms of the solid state. Predicting the number of phases present

More information

ORGANIC LABORATORY TECHNIQUES 10 10.1. NEVER distill the distillation flask to dryness as there is a risk of explosion and fire.

ORGANIC LABORATORY TECHNIQUES 10 10.1. NEVER distill the distillation flask to dryness as there is a risk of explosion and fire. ORGANIC LABORATORY TECHNIQUES 10 10.1 DISTILLATION NEVER distill the distillation flask to dryness as there is a risk of explosion and fire. The most common methods of distillation are simple distillation

More information

a) Use the following equation from the lecture notes: = ( 8.314 J K 1 mol 1) ( ) 10 L

a) Use the following equation from the lecture notes: = ( 8.314 J K 1 mol 1) ( ) 10 L hermodynamics: Examples for chapter 4. 1. One mole of nitrogen gas is allowed to expand from 0.5 to 10 L reversible and isothermal process at 300 K. Calculate the change in molar entropy using a the ideal

More information

Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline

Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline Gases and Kinetic-Molecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he Volume-Pressure

More information

ES-7A Thermodynamics HW 1: 2-30, 32, 52, 75, 121, 125; 3-18, 24, 29, 88 Spring 2003 Page 1 of 6

ES-7A Thermodynamics HW 1: 2-30, 32, 52, 75, 121, 125; 3-18, 24, 29, 88 Spring 2003 Page 1 of 6 Spring 2003 Page 1 of 6 2-30 Steam Tables Given: Property table for H 2 O Find: Complete the table. T ( C) P (kpa) h (kj/kg) x phase description a) 120.23 200 2046.03 0.7 saturated mixture b) 140 361.3

More information

Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.

Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion. Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.

More information

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g) CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26

More information

Experiment 12E LIQUID-VAPOR EQUILIBRIUM OF WATER 1

Experiment 12E LIQUID-VAPOR EQUILIBRIUM OF WATER 1 Experiment 12E LIQUID-VAPOR EQUILIBRIUM OF WATER 1 FV 6/26/13 MATERIALS: PURPOSE: 1000 ml tall-form beaker, 10 ml graduated cylinder, -10 to 110 o C thermometer, thermometer clamp, plastic pipet, long

More information

Gases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random)

Gases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random) Gases States of Matter States of Matter Kinetic E (motion) Potential E(interaction) Distance Between (size) Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large

More information

Lecture 9 Solving Material Balances Problems Involving Non-Reactive Processes

Lecture 9 Solving Material Balances Problems Involving Non-Reactive Processes CHE 31. INTRODUCTION TO CHEMICAL ENGINEERING CALCULATIONS Lecture 9 Solving Material Balances Problems Involving Non-Reactive Processes Component and Overall Material Balances Consider a steady-state distillation

More information

48 Practice Problems for Ch. 17 - Chem 1C - Joseph

48 Practice Problems for Ch. 17 - Chem 1C - Joseph 48 Practice Problems for Ch. 17 - Chem 1C - Joseph 1. Which of the following concentration measures will change in value as the temperature of a solution changes? A) mass percent B) mole fraction C) molality

More information

Calorimetry: Heat of Vaporization

Calorimetry: Heat of Vaporization Calorimetry: Heat of Vaporization OBJECTIVES INTRODUCTION - Learn what is meant by the heat of vaporization of a liquid or solid. - Discuss the connection between heat of vaporization and intermolecular

More information

Final Exam CHM 3410, Dr. Mebel, Fall 2005

Final Exam CHM 3410, Dr. Mebel, Fall 2005 Final Exam CHM 3410, Dr. Mebel, Fall 2005 1. At -31.2 C, pure propane and n-butane have vapor pressures of 1200 and 200 Torr, respectively. (a) Calculate the mole fraction of propane in the liquid mixture

More information

EXERCISES. 16. What is the ionic strength in a solution containing NaCl in c=0.14 mol/dm 3 concentration and Na 3 PO 4 in 0.21 mol/dm 3 concentration?

EXERCISES. 16. What is the ionic strength in a solution containing NaCl in c=0.14 mol/dm 3 concentration and Na 3 PO 4 in 0.21 mol/dm 3 concentration? EXERISES 1. The standard enthalpy of reaction is 512 kj/mol and the standard entropy of reaction is 1.60 kj/(k mol) for the denaturalization of a certain protein. Determine the temperature range where

More information

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,

More information

Chemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES

Chemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES Chemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES The learning objectives of this experiment are to explore the relationship between the temperature and vapor pressure of water. determine the molar

More information

Lecture 1: Physical Equilibria The Temperature Dependence of Vapor Pressure

Lecture 1: Physical Equilibria The Temperature Dependence of Vapor Pressure Lecture 1: Physical Equilibria The Temperature Dependence of Vapor Pressure Our first foray into equilibria is to examine phenomena associated with two phases of matter achieving equilibrium in which the

More information

4-1 Copyright Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014)

4-1 Copyright Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014) Balances on Multiphase Systems A B, B C A feedstock, B desired product, C byproduct (waste) B(v) to purification and packaging Distillation Column A(g) A(g) A(g),B(g),C(g) B(l), C(l) 80 o F 900 o F 700

More information

CHAPTER 12. Gases and the Kinetic-Molecular Theory

CHAPTER 12. Gases and the Kinetic-Molecular Theory CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids

More information

We will study the temperature-pressure diagram of nitrogen, in particular the triple point.

We will study the temperature-pressure diagram of nitrogen, in particular the triple point. K4. Triple Point of Nitrogen I. OBJECTIVE OF THE EXPERIMENT We will study the temperature-pressure diagram of nitrogen, in particular the triple point. II. BAKGROUND THOERY States of matter Matter is made

More information

AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1

AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1 Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example

More information

The Ideal Solution. ChemActivity T15

The Ideal Solution. ChemActivity T15 ChemActivity T15 The Ideal Solution Focus Question: An equi-molar mixture of benzene and toluene is prepared. What will be the composition of the vapor in equilibrium with this solution? Model 1: Benzene

More information

Chapter 13. Properties of Solutions

Chapter 13. Properties of Solutions Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. A.P. Chemistry Practice Test: Ch. 11, Solutions Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Formation of solutions where the process is

More information

AP CHEMISTRY 2009 SCORING GUIDELINES (Form B)

AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) Question 3 (10 points) 2 H 2 O 2 (aq) 2 H 2 O(l) + O 2 (g) The mass of an aqueous solution of H 2 O 2 is 6.951 g. The H 2 O 2 in the solution decomposes completely

More information

F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.

F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7. Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.

More information

Chapter 7 Energy and Energy Balances

Chapter 7 Energy and Energy Balances CBE14, Levicky Chapter 7 Energy and Energy Balances The concept of energy conservation as expressed by an energy balance equation is central to chemical engineering calculations. Similar to mass balances

More information

Chem 420/523 Chemical Thermodynamics Homework Assignment # 6

Chem 420/523 Chemical Thermodynamics Homework Assignment # 6 Chem 420/523 Chemical hermodynamics Homework Assignment # 6 1. * Solid monoclinic sulfur (S α ) spontaneously converts to solid rhombic sulfur (S β ) at 298.15 K and 0.101 MPa pressure. For the conversion

More information

Molar Mass of Butane

Molar Mass of Butane Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures

More information

THE HUMIDITY/MOISTURE HANDBOOK

THE HUMIDITY/MOISTURE HANDBOOK THE HUMIDITY/MOISTURE HANDBOOK Table of Contents Introduction... 3 Relative Humidity... 3 Partial Pressure... 4 Saturation Pressure (Ps)... 5 Other Absolute Moisture Scales... 8 % Moisture by Volume (%M

More information

Performing Multi - Phase Mass and Energy Balances

Performing Multi - Phase Mass and Energy Balances Performing Multi-Phase Mass and Energy Balances (Separations) Performing Multi - Phase Mass and Energy Balances Using thermodynamics in mass / energy balance problems means that additional equations are

More information

CHEMISTRY GAS LAW S WORKSHEET

CHEMISTRY GAS LAW S WORKSHEET Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is

More information

The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10

The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10 Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force

More information

QUESTIONS THERMODYNAMICS PRACTICE PROBLEMS FOR NON-TECHNICAL MAJORS. Thermodynamic Properties

QUESTIONS THERMODYNAMICS PRACTICE PROBLEMS FOR NON-TECHNICAL MAJORS. Thermodynamic Properties QUESTIONS THERMODYNAMICS PRACTICE PROBLEMS FOR NON-TECHNICAL MAJORS Thermodynamic Properties 1. If an object has a weight of 10 lbf on the moon, what would the same object weigh on Jupiter? ft ft -ft g

More information

Chapter 12 - Liquids and Solids

Chapter 12 - Liquids and Solids Chapter 12 - Liquids and Solids 12-1 Liquids I. Properties of Liquids and the Kinetic Molecular Theory A. Fluids 1. Substances that can flow and therefore take the shape of their container B. Relative

More information

Thermodynamics. Thermodynamics (Th)

Thermodynamics. Thermodynamics (Th) Thermodynamics (Th) Thermodynamics Thermodynamics can be used to make the number of necessary measurements smaller, or to make the type of measurement easier. It turns out that volumetric flowrates are

More information

Chemistry 13: States of Matter

Chemistry 13: States of Matter Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties

More information

Rusty Walker, Corporate Trainer Hill PHOENIX

Rusty Walker, Corporate Trainer Hill PHOENIX Refrigeration 101 Rusty Walker, Corporate Trainer Hill PHOENIX Compressor Basic Refrigeration Cycle Evaporator Condenser / Receiver Expansion Device Vapor Compression Cycle Cooling by the removal of heat

More information

The first law: transformation of energy into heat and work. Chemical reactions can be used to provide heat and for doing work.

The first law: transformation of energy into heat and work. Chemical reactions can be used to provide heat and for doing work. The first law: transformation of energy into heat and work Chemical reactions can be used to provide heat and for doing work. Compare fuel value of different compounds. What drives these reactions to proceed

More information

Answer, Key Homework 6 David McIntyre 1

Answer, Key Homework 6 David McIntyre 1 Answer, Key Homework 6 David McIntyre 1 This print-out should have 0 questions, check that it is complete. Multiple-choice questions may continue on the next column or page: find all choices before making

More information

FUNDAMENTALS OF ENGINEERING THERMODYNAMICS

FUNDAMENTALS OF ENGINEERING THERMODYNAMICS FUNDAMENTALS OF ENGINEERING THERMODYNAMICS System: Quantity of matter (constant mass) or region in space (constant volume) chosen for study. Closed system: Can exchange energy but not mass; mass is constant

More information

Physical Chemistry Laboratory I CHEM 445 Experiment 6 Vapor Pressure of a Pure Liquid (Revised, 01/09/06)

Physical Chemistry Laboratory I CHEM 445 Experiment 6 Vapor Pressure of a Pure Liquid (Revised, 01/09/06) 1 Physical Chemistry Laboratory I CHEM 445 Experiment 6 Vapor Pressure of a Pure Liquid (Revised, 01/09/06) The vapor pressure of a pure liquid is an intensive property of the compound. That is, the vapor

More information

Gibbs Free Energy and Chemical Potential. NC State University

Gibbs Free Energy and Chemical Potential. NC State University Chemistry 433 Lecture 14 Gibbs Free Energy and Chemical Potential NC State University The internal energy expressed in terms of its natural variables We can use the combination of the first and second

More information

Review of Chemical Equilibrium Introduction

Review of Chemical Equilibrium Introduction Review of Chemical Equilibrium Introduction Copyright c 2016 by Nob Hill Publishing, LLC This chapter is a review of the equilibrium state of a system that can undergo chemical reaction Operating reactors

More information

= 800 kg/m 3 (note that old units cancel out) 4.184 J 1000 g = 4184 J/kg o C

= 800 kg/m 3 (note that old units cancel out) 4.184 J 1000 g = 4184 J/kg o C Units and Dimensions Basic properties such as length, mass, time and temperature that can be measured are called dimensions. Any quantity that can be measured has a value and a unit associated with it.

More information

Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1

Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1 Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0

More information

PHYSICAL-CHEMICAL PROCESSES OF CLOUD ACTIVATION STUDIED WITH A DESKTOP CLOUD MODEL

PHYSICAL-CHEMICAL PROCESSES OF CLOUD ACTIVATION STUDIED WITH A DESKTOP CLOUD MODEL PHYSICAL-CHEMICAL PROCESSES OF CLOUD ACTIVATION STUDIED WITH A DESKTOP CLOUD MODEL Stephen E. Schwartz ses@bnl.gov Brookhaven National Laboratory Upton NY USA 11973 6th International Conference Air-Surface

More information

Problem Set 4 Solutions

Problem Set 4 Solutions Chemistry 360 Dr Jean M Standard Problem Set 4 Solutions 1 Two moles of an ideal gas are compressed isothermally and reversibly at 98 K from 1 atm to 00 atm Calculate q, w, ΔU, and ΔH For an isothermal

More information

Thermodynamics of Adsorption

Thermodynamics of Adsorption CTI_CHAPTER_21.qxd 6/7/24 3:31 PM Page 243 CHAPTER 21 Thermodynamics of Adsorption ALAN L. MYERS 1 Introduction The attachment of molecules to the surface of a solid by adsorption is a broad subject. This

More information

Air Water Vapor Mixtures: Psychrometrics. Leon R. Glicksman c 1996, 2010

Air Water Vapor Mixtures: Psychrometrics. Leon R. Glicksman c 1996, 2010 Air Water Vapor Mixtures: Psychrometrics Leon R. Glicksman c 1996, 2010 Introduction To establish proper comfort conditions within a building space, the designer must consider the air temperature and the

More information

Kinetic Theory of Gases

Kinetic Theory of Gases Kinetic Theory of Gases Physics 1425 Lecture 31 Michael Fowler, UVa Bernoulli s Picture Daniel Bernoulli, in 1738, was the first to understand air pressure in terms of molecules he visualized them shooting

More information

Figure 56. Simple mixing process with process specification for the outlet stream.

Figure 56. Simple mixing process with process specification for the outlet stream. Flowsheet Analysis One of the most useful functions of process simulators is the ability to manipulate and analyze the different design variables to determine the required value or study its effect on

More information

Why? Intermolecular Forces. Intermolecular Forces. Chapter 12 IM Forces and Liquids. Covalent Bonding Forces for Comparison of Magnitude

Why? Intermolecular Forces. Intermolecular Forces. Chapter 12 IM Forces and Liquids. Covalent Bonding Forces for Comparison of Magnitude 1 Why? Chapter 1 Intermolecular Forces and Liquids Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water?

More information

LECTURE I-UNITS OF CONCENTRATION

LECTURE I-UNITS OF CONCENTRATION LECTURE I-UNITS OF CONCENTRATION Chemical concentration is one of the most important determinants in almost all aspects of chemical fate, transport and treatment in both environmental and engineered systems.

More information

Chemistry B11 Chapter 4 Chemical reactions

Chemistry B11 Chapter 4 Chemical reactions Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl

More information

CHEM 120 Online Chapter 7

CHEM 120 Online Chapter 7 CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases

More information

THERMODYNAMICS. TUTORIAL No.8 COMBUSTION OF FUELS. On completion of this tutorial you should be able to do the following.

THERMODYNAMICS. TUTORIAL No.8 COMBUSTION OF FUELS. On completion of this tutorial you should be able to do the following. THERMODYNAMICS TUTORIAL No.8 COMBUSTION OF FUELS On completion of this tutorial you should be able to do the following.. Let's start by revising the basics. Write down combustion equations. Solve the oxygen

More information

μ α =μ β = μ γ = =μ ω μ α =μ β =μ γ = =μ ω Thus for c components, the number of additional constraints is c(p 1) ( ) ( )

μ α =μ β = μ γ = =μ ω μ α =μ β =μ γ = =μ ω Thus for c components, the number of additional constraints is c(p 1) ( ) ( ) Phase Diagrams 1 Gibbs Phase Rule The Gibbs phase rule describes the degrees of freedom available to describe a particular system with various phases and substances. To derive the phase rule, let us begin

More information

Gases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6

Gases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6 Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000A 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,

More information

States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.

States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided. CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas

More information

5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C

5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C 1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

Stoichiometry. Lecture Examples Answer Key

Stoichiometry. Lecture Examples Answer Key Stoichiometry Lecture Examples Answer Key Ex. 1 Balance the following chemical equations: 3 NaBr + 1 H 3 PO 4 3 HBr + 1 Na 3 PO 4 2 C 3 H 5 N 3 O 9 6 CO 2 + 3 N 2 + 5 H 2 O + 9 O 2 2 Ca(OH) 2 + 2 SO 2

More information

Phase diagram of water. Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure.

Phase diagram of water. Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure. Phase diagram of water Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure. WATER Covers ~ 70% of the earth s surface Life on earth

More information

13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects

13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects Week 3 Sections 13.3-13.5 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects 13.4 Ways of Expressing Concentration Mass Percentage, ppm, and ppb Mole Fraction,

More information

Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).

Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse

More information

4. Introduction to Heat & Mass Transfer

4. Introduction to Heat & Mass Transfer 4. Introduction to Heat & Mass Transfer This section will cover the following concepts: A rudimentary introduction to mass transfer. Mass transfer from a molecular point of view. Fundamental similarity

More information

k 2f, k 2r C 2 H 5 + H C 2 H 6

k 2f, k 2r C 2 H 5 + H C 2 H 6 hemical Engineering HE 33 F pplied Reaction Kinetics Fall 04 Problem Set 4 Solution Problem. The following elementary steps are proposed for a gas phase reaction: Elementary Steps Rate constants H H f,

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55

More information

Distillation Principles

Distillation Principles Distillation Principles Definition of distillation, Types of columns, Simple Distillation methods (Flash, batch, Steam), Basic distillation Equipment and operation, Column internal, Reboilers, Distillation

More information

Chemistry 110 Lecture Unit 5 Chapter 11-GASES

Chemistry 110 Lecture Unit 5 Chapter 11-GASES Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all

More information

HAVE A BLAST FINDING MOLAR MASS An Ideal Gas Experiment. Contents:

HAVE A BLAST FINDING MOLAR MASS An Ideal Gas Experiment. Contents: EXPERIMENT 4 HAVE A BLAST FINDING MOLAR MASS An Ideal Gas Experiment Contents: Pages 2-8: Teachers Guide Pages 9-11: Student Handout ACKNOWLEDGEMENTS The creation of this experiment and its support materials

More information

Experiment 1: Colligative Properties

Experiment 1: Colligative Properties Experiment 1: Colligative Properties Determination of the Molar Mass of a Compound by Freezing Point Depression. Objective: The objective of this experiment is to determine the molar mass of an unknown

More information

Popcorn Laboratory. Hypothesis : Materials:

Popcorn Laboratory. Hypothesis : Materials: Popcorn Laboratory Problem: Popcorn kernels explode into delightful, edible parcels because of a build-up of pressure inside the kernel during heating. In this experiment you will try to calculate the

More information

Fugacity, Activity, and Standard States

Fugacity, Activity, and Standard States Fugacity, Activity, and Standard States Fugacity of gases: Since dg = VdP SdT, for an isothermal rocess, we have,g = 1 Vd. For ideal gas, we can substitute for V and obtain,g = nrt ln 1, or with reference

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008

Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008 Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid

More information

1.3 Saturation vapor pressure. 1.3.1 Vapor pressure

1.3 Saturation vapor pressure. 1.3.1 Vapor pressure 1.3 Saturation vaor ressure Increasing temerature of liquid (or any substance) enhances its evaoration that results in the increase of vaor ressure over the liquid. y lowering temerature of the vaor we

More information

CHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry

CHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,

More information

Standard Test Method for Vapor Pressure 1

Standard Test Method for Vapor Pressure 1 Designation: E 1194 01 Standard Test Method for Vapor Pressure 1 This standard is issued under the fixed designation E 1194; the number immediately following the designation indicates the year of original

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Given: 4 NO2(g) + O2(g) 2 N2O5(g) ΔH = -110.2 kj find ΔH for N2O5(g) 2 NO2(g) + 1/2 O2(g).

More information

VAPOR PRESSURE AS A FUNCTION OF TEMPERATURE. This laboratory covers material presented in section 11.8 of the 9 th Ed. of the Chang text.

VAPOR PRESSURE AS A FUNCTION OF TEMPERATURE. This laboratory covers material presented in section 11.8 of the 9 th Ed. of the Chang text. VAPOR PRESSURE AS A FUNCTION OF TEMPERATURE Objectives: (1) Observe and measure the change in the vapor pressure (dependent variable) as a function of temperature (independent variable). (2) Analyze the

More information

Where the exp subscripts refer to the experimental temperature and pressure acquired in the laboratory.

Where the exp subscripts refer to the experimental temperature and pressure acquired in the laboratory. Molar Volume of Carbon Dioxide Reading assignment: Julia Burdge, Chemistry 3rd edition, Chapter 10. Goals To determine the molar volume of carbon dioxide gas and the amount of sodium carbonate in a sample.

More information

1-1 Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014)

1-1 Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014) Air Conditioner Sizing Exercise On an uncomfortable summer day, the air is at 87 o F and 80% relative humidity. A laboratory air conditioner is to deliver 1000 ft 3 /min of air at 55 o F in order to maintain

More information

Chemistry 101 Generating Hydrogen Gas

Chemistry 101 Generating Hydrogen Gas Chemistry 101 Generating Hydrogen Gas Objectives To experimentally verify the molar volume of hydrogen gas at STP To gain experience in collecting gas over water Discussion The molar volume of a gas is

More information