The document discusses several key concepts in chemistry:
1. It defines atoms and their subatomic particles (protons, neutrons, electrons), isotopes, relative atomic mass, and relative molecular mass.
2. It explains that matter is made up of elements, compounds, and mixtures and defines these terms. Atoms combine to form molecules or ions that make up compounds.
3. It introduces the mole as a unit containing 6.022x10^23 elementary entities that is used to relate the amount of a substance to its mass in grams.
This presentation talks about the application of Law of Conservation of Mass to Chemical Equations. It has a step-by-step process of balancing equations with a bit of mole-mass conversions.
This presentation talks about the application of Law of Conservation of Mass to Chemical Equations. It has a step-by-step process of balancing equations with a bit of mole-mass conversions.
Laws of chemical combinations, prepared by Saliha RaisSaliha Rais
The presentation "Laws of chemical combinations" is prepared for grade 9, for educational purpose. the topics include all the four Laws of Chemical Combination.
Easy way to understand moles. 1 mole has the same number of particles present in 12 grams of Carbon-12. Carbon-12 is an isotope of carbon which is taken as standard. Mass of 1 mole of atoms = Atomic mass, Mass of 1 mole of molecules = molecular mass.
Postsecondary lesson for pre-u students or form 6th students on mole concept, stoichiometry, limiting reagent, spectrometry and percent yield and percent purity.
Laws of chemical combinations, prepared by Saliha RaisSaliha Rais
The presentation "Laws of chemical combinations" is prepared for grade 9, for educational purpose. the topics include all the four Laws of Chemical Combination.
Easy way to understand moles. 1 mole has the same number of particles present in 12 grams of Carbon-12. Carbon-12 is an isotope of carbon which is taken as standard. Mass of 1 mole of atoms = Atomic mass, Mass of 1 mole of molecules = molecular mass.
Postsecondary lesson for pre-u students or form 6th students on mole concept, stoichiometry, limiting reagent, spectrometry and percent yield and percent purity.
Attacking the TEKS: Focus on Atomic Theory presented by Jane Smith, ACT2 2010
This session will expose you to the new TEKS and College Readiness Standards. Ideas for sequencing and planning the unit will be shared along with tips for appropriate demos, labs, and assessments. The intended audience is for teachers with 3 or less years of experience or anyone who wants to delve deeper into the new standards.
JMeter webinar - integration with InfluxDB and GrafanaRTTS
Watch this recorded webinar about real-time monitoring of application performance. See how to integrate Apache JMeter, the open-source leader in performance testing, with InfluxDB, the open-source time-series database, and Grafana, the open-source analytics and visualization application.
In this webinar, we will review the benefits of leveraging InfluxDB and Grafana when executing load tests and demonstrate how these tools are used to visualize performance metrics.
Length: 30 minutes
Session Overview
-------------------------------------------
During this webinar, we will cover the following topics while demonstrating the integrations of JMeter, InfluxDB and Grafana:
- What out-of-the-box solutions are available for real-time monitoring JMeter tests?
- What are the benefits of integrating InfluxDB and Grafana into the load testing stack?
- Which features are provided by Grafana?
- Demonstration of InfluxDB and Grafana using a practice web application
To view the webinar recording, go to:
https://www.rttsweb.com/jmeter-integration-webinar
UiPath Test Automation using UiPath Test Suite series, part 4DianaGray10
Welcome to UiPath Test Automation using UiPath Test Suite series part 4. In this session, we will cover Test Manager overview along with SAP heatmap.
The UiPath Test Manager overview with SAP heatmap webinar offers a concise yet comprehensive exploration of the role of a Test Manager within SAP environments, coupled with the utilization of heatmaps for effective testing strategies.
Participants will gain insights into the responsibilities, challenges, and best practices associated with test management in SAP projects. Additionally, the webinar delves into the significance of heatmaps as a visual aid for identifying testing priorities, areas of risk, and resource allocation within SAP landscapes. Through this session, attendees can expect to enhance their understanding of test management principles while learning practical approaches to optimize testing processes in SAP environments using heatmap visualization techniques
What will you get from this session?
1. Insights into SAP testing best practices
2. Heatmap utilization for testing
3. Optimization of testing processes
4. Demo
Topics covered:
Execution from the test manager
Orchestrator execution result
Defect reporting
SAP heatmap example with demo
Speaker:
Deepak Rai, Automation Practice Lead, Boundaryless Group and UiPath MVP
State of ICS and IoT Cyber Threat Landscape Report 2024 previewPrayukth K V
The IoT and OT threat landscape report has been prepared by the Threat Research Team at Sectrio using data from Sectrio, cyber threat intelligence farming facilities spread across over 85 cities around the world. In addition, Sectrio also runs AI-based advanced threat and payload engagement facilities that serve as sinks to attract and engage sophisticated threat actors, and newer malware including new variants and latent threats that are at an earlier stage of development.
The latest edition of the OT/ICS and IoT security Threat Landscape Report 2024 also covers:
State of global ICS asset and network exposure
Sectoral targets and attacks as well as the cost of ransom
Global APT activity, AI usage, actor and tactic profiles, and implications
Rise in volumes of AI-powered cyberattacks
Major cyber events in 2024
Malware and malicious payload trends
Cyberattack types and targets
Vulnerability exploit attempts on CVEs
Attacks on counties – USA
Expansion of bot farms – how, where, and why
In-depth analysis of the cyber threat landscape across North America, South America, Europe, APAC, and the Middle East
Why are attacks on smart factories rising?
Cyber risk predictions
Axis of attacks – Europe
Systemic attacks in the Middle East
Download the full report from here:
https://sectrio.com/resources/ot-threat-landscape-reports/sectrio-releases-ot-ics-and-iot-security-threat-landscape-report-2024/
UiPath Test Automation using UiPath Test Suite series, part 3DianaGray10
Welcome to UiPath Test Automation using UiPath Test Suite series part 3. In this session, we will cover desktop automation along with UI automation.
Topics covered:
UI automation Introduction,
UI automation Sample
Desktop automation flow
Pradeep Chinnala, Senior Consultant Automation Developer @WonderBotz and UiPath MVP
Deepak Rai, Automation Practice Lead, Boundaryless Group and UiPath MVP
Builder.ai Founder Sachin Dev Duggal's Strategic Approach to Create an Innova...Ramesh Iyer
In today's fast-changing business world, Companies that adapt and embrace new ideas often need help to keep up with the competition. However, fostering a culture of innovation takes much work. It takes vision, leadership and willingness to take risks in the right proportion. Sachin Dev Duggal, co-founder of Builder.ai, has perfected the art of this balance, creating a company culture where creativity and growth are nurtured at each stage.
LF Energy Webinar: Electrical Grid Modelling and Simulation Through PowSyBl -...DanBrown980551
Do you want to learn how to model and simulate an electrical network from scratch in under an hour?
Then welcome to this PowSyBl workshop, hosted by Rte, the French Transmission System Operator (TSO)!
During the webinar, you will discover the PowSyBl ecosystem as well as handle and study an electrical network through an interactive Python notebook.
PowSyBl is an open source project hosted by LF Energy, which offers a comprehensive set of features for electrical grid modelling and simulation. Among other advanced features, PowSyBl provides:
- A fully editable and extendable library for grid component modelling;
- Visualization tools to display your network;
- Grid simulation tools, such as power flows, security analyses (with or without remedial actions) and sensitivity analyses;
The framework is mostly written in Java, with a Python binding so that Python developers can access PowSyBl functionalities as well.
What you will learn during the webinar:
- For beginners: discover PowSyBl's functionalities through a quick general presentation and the notebook, without needing any expert coding skills;
- For advanced developers: master the skills to efficiently apply PowSyBl functionalities to your real-world scenarios.
PHP Frameworks: I want to break free (IPC Berlin 2024)Ralf Eggert
In this presentation, we examine the challenges and limitations of relying too heavily on PHP frameworks in web development. We discuss the history of PHP and its frameworks to understand how this dependence has evolved. The focus will be on providing concrete tips and strategies to reduce reliance on these frameworks, based on real-world examples and practical considerations. The goal is to equip developers with the skills and knowledge to create more flexible and future-proof web applications. We'll explore the importance of maintaining autonomy in a rapidly changing tech landscape and how to make informed decisions in PHP development.
This talk is aimed at encouraging a more independent approach to using PHP frameworks, moving towards a more flexible and future-proof approach to PHP development.
Slack (or Teams) Automation for Bonterra Impact Management (fka Social Soluti...Jeffrey Haguewood
Sidekick Solutions uses Bonterra Impact Management (fka Social Solutions Apricot) and automation solutions to integrate data for business workflows.
We believe integration and automation are essential to user experience and the promise of efficient work through technology. Automation is the critical ingredient to realizing that full vision. We develop integration products and services for Bonterra Case Management software to support the deployment of automations for a variety of use cases.
This video focuses on the notifications, alerts, and approval requests using Slack for Bonterra Impact Management. The solutions covered in this webinar can also be deployed for Microsoft Teams.
Interested in deploying notification automations for Bonterra Impact Management? Contact us at sales@sidekicksolutionsllc.com to discuss next steps.
Connector Corner: Automate dynamic content and events by pushing a buttonDianaGray10
Here is something new! In our next Connector Corner webinar, we will demonstrate how you can use a single workflow to:
Create a campaign using Mailchimp with merge tags/fields
Send an interactive Slack channel message (using buttons)
Have the message received by managers and peers along with a test email for review
But there’s more:
In a second workflow supporting the same use case, you’ll see:
Your campaign sent to target colleagues for approval
If the “Approve” button is clicked, a Jira/Zendesk ticket is created for the marketing design team
But—if the “Reject” button is pushed, colleagues will be alerted via Slack message
Join us to learn more about this new, human-in-the-loop capability, brought to you by Integration Service connectors.
And...
Speakers:
Akshay Agnihotri, Product Manager
Charlie Greenberg, Host
1. Chapter 1 : Matter 1.1 Atoms and molecules # I dentify and describe protons, electrons and neutrons as sub-atomic particles. # Define proton number, nucleon number and isotopes and write isotope denotation. # Define relative atomic mass and relative molecular mass based on the C-12 scale. Objectives : LECTURE 1
2. What is matter? 1. Matter is made up of elements, compounds and mixtures 2. The basic building block of matter is called atom . 3. An element consists of same kind of atoms e.g. Fe Anything that occupies space and possesses mass is called matter. Example : air, earth, animals, trees, atoms,… The three states of matter are solid, liquid and gas
3. 3. A compound is made up of 2 or more kinds of atoms chemically bonded in a definite proportion e.g. NaCl, CO 2 . 4. A compound may consist of molecules or ions. E.g. NH 3 , K + Br - . 5. A molecule is made up of 2 or more atoms of the same or different element/s bonded covalently to form a discrete unit.e.g. O 3 , H 2 O. 6. An ion is an atom/group of atoms either gained electron/s (anion) or lost electron/s(kation). E.g. S 2- , Cu + , SO 4 2- .
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7. e.g. 23 Na + 11 Total charge on the ion = 1+ nucleon no., A = No. of (p+ n) = 23 proton no., Z = no. of p = 11 no. of n in nucleus of = A - Z = 23 – 11= 12 No. of e - = Z – charge = 11- (+1) = 10 Find: the no. of I) proton, ii) neutron, iii) electron?
8. Example 1.1.2: Give the number of protons, neutrons and electrons in each atom of the following species: (a) b) 2+ 2+ 2 2 No. of Symbol charge 2- 1 10 9 8 2+ 2 78 120 80 atom e n p
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10. Ex. 2 Give the isotopes’ names of hydrogen and oxygen.and write their respective atomic denotation. Ans: H: protium, deuterium and tritium O : oxygen- 16, oxygen-17 and oxygen -18 1 2 3 H H H 1 1 1 16 17 18 O O O 8 8 8
11. Complete the following table: 40 18 ----- Ca ---- ----- f. 80 125 82 e. 23 26 56 d. 32 18 *32 16 c. 24 Mg 2+ 12 b. 35 18 18 17 35 17 35 Cl - 17 a. Atomic mass No. of e - No. of n No. of p A Z Symbol notation No.
12. 40 18 20 20 40 20 40 2+ ----- Ca ---- 20 ----- f. 207 80 125 82 207 82 207 Pb 2+ 82 e. 56 23 30 26 56 26 56 Fe 3+ 26 d. 32 18 16 16 *32 16 32 S 2- 16 c. 24 12 - 2 = 10 12 12 24 12 24 Mg 2+ 12 b. 35 18 18 17 35 17 35 Cl - 17 a. Atomic mass No. of e No. of n No. of p A Z Symbol notation No.
13. RELATIVE MASS <>Isotope Carbon-12 as a reference or standard for comparing the masses of other atoms. Definition: Relative atomic mass => mass of 1atom of an element(a.m.u.) 1/12 mass of 1 atom of C-12 isotope(a.m.u.) e.g. Relative atomic mass of Na = mass of 1atom Na 1/12 mass of 1 atom 12 C isotope = 23 a.m.u ./1.0 a.m.u = 23
14. Relative molecular mass Definition: Sum of all the relative atomic masses of all atoms present in a molecule. e.g. : Molecular formula of sulphuric acid is H 2 SO 4 , determine its relative molecular mass. [ RAM: H=1.00; S=32.0; O=16.0] Ans: RMM H 2 SO 4 = 2X1.00 + 32.0 + 4X16.0 = 98.0
15. 1. For each of the substances:: i) Na 2 CO 3 ii. MgO. [ Mg=24.0; O= 16.0; Na=23.0; C=12.0] Find its relative molecular mass Exercise: .2. .Determine the relative atomic mass of an element X if the ratio of the atomic mass of X to carbon-12 is 0.75 3. The relative atomic mass of chlorine atom is 35.5 Explain why this no. is not a whole no.. 4. Relative atomic mass of bromine atom is 80. What is the mass of Br compared to carbon-12 atom? Ans: 9.00 Ans: 6.7
16. The mass spectrometer is used to : i. determine the atomic mass and molecular mass of substances. ii. reveal the presence of isotopes of elements and its relative abundance. MASS SPECTROMETRY Who invented the mass spectrometer?
17. Vaporisation chamber Acceleration chamber (Electric field) Magnetic field Ionization chamber Ion detector vacuum Figure : Diagramatic representation of Mass Spectrometer A B
18. Vaporisation Chamber Sample of the element is vaporised into gaseous atom Ionisation Chamber A gaseous sample (atom or molecule) is bombarded by a stream of high-energy electrons that are emitted from a hot filament. Collisions between the electrons and the gaseous atom (or molecule) produce positive ions by dislodging an electron from each atom or molecule M + e M + + e + e
19. Acceleration Chamber (Electric field) The positive ions are accelerated by an electric field towards the two oppositely charged plates. The electric field is produced by a high voltage between the two plates. The emerging ions are of high and constant velocity Magnetic field The positive ions are separated and deflected into a circular path by a magnet according to its mass/charge ( m/e) ratio . Positive ions with small m/e ratio are deflected most and appear near A. Ions with large m/e ratio are deflected least and appear near B
20. Ion detector The numbers of ions and types of isotopes are recorded as a mass spectrum . In practice, the ion detector is kept in a fixed position. The magnetic field is varied so that the positive ions of different masses arrive at the detector at different times
21. Mass spectrum : The horizontal axis = m/e ratio or nucleon number or isotopic mass or relative atomic mass of the ions entering the detector. The vertical axis= the abundance or detector current or relative abundance or ion intensity or percentage abundance of the ions. The height is proportional to the amount of each isotope present.
22. Relative abundance 63 8.1 9.1 0 24 25 26 m/e The mass spectrum of magnesium shows that naturally occurring magnesium consists of three isotopes: 24 Mg, 25 Mg and 26 Mg. The height of each line is proportional to the abundance of each isotope. In this example, 24 Mg is the most abundance of the three isotopes
23. A r Mg = (24 a.m.u. x 63) + (25 a.m.u. x 8.1) + (26 a.m.u x 9.1) (63 + 8.1 + 9.1) = 24.33 A r = where Q = the abundance of an isotope of the element = the percentage of the isotope found in the naturally occurring element m = the relative isotopic mass of the element General formula for A r
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25. Eg.: Boron comprises of 2 isotopes, i.e. 14.6 % 10 B dan 85.4 % 11 B with their isotopic masses of 10.01294 dan 11.00931 respectively. Calculate the relative atomic mass of B. Ans: RAM Boron = % 10 B x A r + % 11 B x A r 100 % = 14.6 x 10.01294 + 85.4 x 11.00931 % 100% = 10.8
26. 1. The atomic masses of 6 Li and 7 Li are 6.0151 amu and 7.0160 amu respectively. What is the relative abundance of each isotope if the relative atomic mass of lithium is 6.941 amu? Ans:(92.95%, 7.05 %) 2. Naturally occurring iridium, Ir is composed of 2 isotopes and in the ratio of 5:8. The relative isotopic mass of and are 191.021 and 193.025 respectively. Calculate the relative atomic mass of iridium. Ans:(192.254) Exercise your mind:
27. Objectives: #1 . Write chemical formulae of ionic compounds #2 Define mole in term of mass #2. Relate the no. of mole with Avogadro constant #3. perform calculation involving converting : i. Mole to mass ii. mass to mole #4. Relate the number of particles to mass through Avogadro ‘s constant, N A LECTURE 2
28. Chemical formulae of ionic compounds: Ionic compounds consists of : Cation(+ve ion) and anion(-ve ion) chemically bonded together by ionic bond. types : I. between monoatomic cation and anion e.g K + Cl - 2 . Monoatomic cation and polyatomic anion e.g. Mg 2+ CO 3 2- 3. Polyatomic cation and monoatomic anion e.g. ( NH 4 +) 2 S 2- 4. Polyatomic cation and anion e.g. . NH 4 + NO 3 - 5. Other combinations.
29. IUPAC names of some common anions & caions -ve Ion +ve Ion Chromate CrO 4 2- Chromium(III) Cr 3+ Carbonate CO 3 2- Manganese (II) Mn 2+ Sulphate SO 4 2- Manganese(IV) Mn 4+ Permanganate MnO 4 - Iron(III) Fe 3+ Nitrate NO 3 - Iron(II) Fe 2+ Hydroxide OH - Aluminium Al 3+ Nitride N 3- Barium Ba 2+ Sulphide S 2- Ammonium NH 4 + Bromide Br - Potassium K +
30. IUPAC names of some common anions & caions -ve Ion +ve Ion Phosphate PO 4 3- Lead(IV) Pb 4+ Oxide O 2- Lead(II) Pb 2+ Sulphite SO 3 2- Tin(IV) Sn 4+ Cyanide CN - Zinc Zn 2+ Nitrite NO 2 - Barium Ba 2+ Chlorite ClO 2 - Cobalt (II) Co 2+ Chlorate ClO 3 - Silver Ag + peroxide O 2 - Copper (I) Cu + Chloride Cl - Hydrogen H +
31. Writing chemical formulae of ionic compounds e.g. Potassium sulphite: . K + SO 3 2- 2- 1+ X2 =2 x2 K 2 SO 3 Steps: : i. write symbol of cation followed by that of anion. ii. Combine the 2 , make sure their total charge = 0 e.g. 2K + + SO 3 2- = (2+) + (2-) = 0 Hence the chemical formula for potassium sulphite is K 2 SO 3
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33. 2. Name the following compounds using IUPAC Nomenclature: i. K 2 CrO 4 ii. Na 2 Cr 2 O 7 iii. Ca(OH) 2 iv. ZnSO 4 v. Al 2 (CO 3 ) 3 vi. HNO 3 vii. MgS viii. MgSO 4 .7H 2 O
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36. MOLAR MASS: Is the mass of 1 mole of an element or compound. E.g. 1 mole of copper,Cu , contains 6.022045 x 10 23 atoms and weighs 63.5 g . What is the molar mass of Cu? Ans: 63.5 g mol -1 Unit used = g mol -1 Mass of Cu atom = 63.5 amu ( from mass spectrometry) 1 mole Cu atoms ≡ 6.022 x 10 23 atoms mole -1 Cu x 63.5 a.m..u/atom Cu Since 1 a.m.u. = 1.6605 x 10 -24 g (from Std.atomic mass of 12 C scale) Hence molar mass of Cu, M Cu =( 3.824 x 10 25 a.m.u. mol -1 x 1.66505 x 10 -24 g / 1 a.m.u.) = 63.5 g mol -1 molar mass is taken as the mass with value of the relative atomic mass , A r or molecular mass, M r in unit g mole -1
37. MOLAR MASS OF ATOM (a) 30.97 g mole -1 Exercise 2: (a) What is the molar mass of phosphorus with Its relative atomic mass of 30.97? (b) 0.50 mole of K weighs 19.50 g. What is its molar mass? (b) 39.0 g mole -1 MOLAR MASS OF a molecule/compound Is the sum of atomic masses of the elements in 1 mole of the molecule or compound. e.g. Find the molar mass of Cl 2 Ans: Molar mass of Cl 2 , M Cl = 2 x M Cl = 2 x 35.5 g mole -1 = 70.0 g mole -1 2
38. MOLAR MASS OF a molecule/compound Exercise 3: Find the molar mass of SO 2. [Given A r of : S = 32.0, O = 16.0] Ans : 64.0 g mole -1 Relate mass to mole of a substance Relate mole to mass to become quantity we can measure, ie. That can be weighed. Mass (g) = moles(n) x molar mass(g mole -1 ) i.e. m = n x M
39. e.g.1. . What is the mass of 2.50 moles of iron, Fe? [ Fe = 56.0] From m = n x M, Hence mass of Fe, m = 2.50 moles x 56.0 g mole -1 = 140.0 g e.g. 2 : How may mole of N 2 contained in 1.40 g of N 2 (g)? . From m = n x M, I.e. n = m / M Ans: Mole of N 2 , n = 1.40 g / 28.0 g mole -1 = 0.050 mole
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41. no. of particles = n x N A e.g. 1. Find the no. of ion in 0.80 mole of O 2- Ans: No. of ion O 2- = 0.80 mole x 6.022 x 10 23 ions mole -1 = 4.48 x 10 24 ions Relate mole to no. of elementary particles e.g. Find the amount(moles) in 6.022 x 10 24 atoms of Na? Ans: n = 6.022 x 10 24 atoms = 10.00 moles 6.022 x 10 23 atoms mole -1
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43. Summary/review #1 Mole is an amount of substance containing the same no. of elementary. particles as that of 12 C atoms in 12.00g of 12 C. #2 molar mass of different substances contain the same no. of elementary particles. e.g. the no. of : Na atoms in 23.0 g = CO 2 molecules in 44.0g #3 Molar mass Ξ 1 mole Ξ 6.022 x 10 23 ( i.e.N A ) #4 Molar atomic mass obtained by expressing the A r in g mole -1 #5 Molar molecular mass = sum of molar atomic masses of all elements in molecule.
44. Relate mole to mass and no. of particles. Summary/review # 1 Convert mole to mass: m = n x M #2 Convert mass to mole: n = m / M #3 Convert mole to no. of elementary particles: no. of particles = m x N A #4 Convert no of elementary particles to mole: n = no. of particles / N A #5 Relate mole to no. of elementary particles No. of particles(atom/ ion/molecule) = n x N A #6 Relate no. of elementary particles to mole n = No. of particles / N A
45. THE MOLE CONCEPT Objectives: #1 . Perform calculation involving converting i. mass to No. of elementary particles ii. no. of particles to mass #2. Relate mole with molar volume of gases #4. Relate volume of a gas to quantity in moles at : i. STP ii. room condition LECTURE 3
46. Convert mass to No. of elementary particles mass mole No. of particles e.g. How many molecules are found in 34.0 g of NH 3 ? Ans: molar mass of NH 3 = 14.0 + 3.00 = 17.0 g mole -1 moles of NH 3 , n = m / M = 34.0 g / 17.0 g mole -1 = 2.00 mole No. of NH 3 molecules = 2.00 mole x 6.022 x 10 23 molecules mole -1 = 1.20 x 10 24 molecules i.e. No. of particles = m x N A M
47. Convert no. of particles to mass No. of particles mole mass i.e. m = no. of particles x M N A e.g. What is the mass of 1.807 x 10 25 formula units of sodium hydroxide, NaOH ? Ans: molar mass, M NaOH = 23.0+16.0+1.00 = 40.0 g mole -1 Hence mass of NAOH, m NaOH = 1.807 x 10 24 f-units x 40.0 g mole -1 6.022 x 10 23 f-units mole -1 = 1200 g
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49. Relate mole with molar volume of gases Molar volume of any gases at STP, V m = 22.4 L mole -1 STP =standard temperature and pressure Where T = 273.15 K P = 1 atm @ 760 mm Hg Amount of gas at STP, n = V gas (L) V m (22.4 L mole -1 ) e.g. How many moles are there in 6.5 L oxygen at STP ? n = 6.5 L O 2 x 1 mole O 2 = 0.29 mole 22.4 L O 2
50. Relate volume with molar volume of gases Molar volume of any gases at STP, V m = 22.4 L mole -1 STP =standard temperature and pressure Where T = 273.15 K P = 1 atm @ 760 mm Hg Amount of gas at STP, n = V gas (L) Vm (22.4 L mole -1 ) e.g. How many moles are there in 6.5 L oxygen at STP ? n = 6.5 L O 2 x 1 mole O 2 = 0.29 mole 22.4 L O 2
51. Relate volume of a gas to quantity in moles Molar volume of any gases at STP, V m = 22.4 L mole -1 STP =standard temperature and pressure Where T = 273.15 K P = 1 atm @ 760 mm Hg At STP V gas (L) = n x V m (22.4 L mol -1 ) e.g. Find volume of 0.25 mole of HCl gas at STP ? ANS: V HCl = 0.25 mol HCl x 22.4 L mol -1 = 5.6 L
52. Exercise/e.g: Calculate the mass of 4.80 L of hydrogen gas at room conditions. Solution: using V gas (L) = n x V m (24 L mol -1 ) n = ( 4.80 / 24 ) mol mass of hydrogen = ( 4.80 / 24 ) mol x 2.00 g mol -1 = 0.40 g Molar volume of any gases at room conditions, V m = 24L mole -1 Room temperature & pressure Where T = 25 0 [email_address] K P = 1 atm @ 760 mm Hg
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54. Summary/review #1 Relate mass to No. of elementary particles : No. of particles = m x N A M where m = mass of substance M = its molar mass; NA = 6.022 x 1022 #2 Relate mole with molar volume of gases Amount of gas at STP, n = Vgas (L) V m (22.4 L mol -1 ) Amount of gas at room conditions, n = Vgas (L) V m (24 L mol -1 )
55. THE MOLE CONCEPT Objectives: #1 . Define i. Empirical formula ii. Molecular formula of a chemical compound. #2. Determine the empirical formula and molecular formula of a compound from it’s a) mass composition, b) combustion data. #3 Determine the % composition by mass of a chemical compound.
56. Chemical Formula Empirical Formula indicates which elements are present and the simplest whole-number ratio of their atoms in a molecule. Molecular Formula shows the exact number of atoms of each element in the smallest unit of a substance. molecula r formula = (empirical formula) n Molecules Empirical formula Molecular Formula n Water H 2 O H 2 O 1 Hydrogen peroxide HO H 2 O 2 2 Benzene CH C 6 H 6 6 Ethyne CH C 2 H 2 2
57. Which 2 compounds have same empirical formula and molecular formula ? Give 2 molecules that might have different molecular formulae but the same empirical formula 1. Calculating the empirical formula from the masses of constituents E.g. 18.3 g sample of hydrated compound contained 4.0 g of calcium, 7.1 g of chlorine and 7.2 g of water only. Calculate its empirical formula.
58. Empirical formula = CaCl 2 . 4H 2 O Constituent Ca Cl H 2 O Mass/g 4.0 7.1 7.2 Amount/mol = 0.10 = 0.20 = 0.40 Simplest ratio of relative amount = 1.0 = 2.0 = 4.0 1 2 4
59. Exercise 50.0 g of phenol. A general disinfectant, has 38.29g C, 3.21 g H ang 8.50 g O. Determine its empirical formula. Ans: C 6 H 6 O Calculating the empirical formula from percentage composition by mass Example : Ascorbic acid (vitamin C) cures scurvy and may help prevent the common cold. It is composed of 40.92% carbon, 4.58% hydrogen and 54.50% oxygen by mass. The molar mass of ascorbic acid is 176 g mol 1 . Determine its empirical formula and molecular formula
60. Empirical formula = C 3 H 4 O 3 n = = = 2 Molecular formula = (C 3 H 4 O 3 ) n = (C 3 H 4 O 3 ) 2 = C 6 H 8 O 6 Element C H O Mass/g 40.92 4.58 54.50 Amount/mol = 3.41 = 4.58 = 3.41 Simplest ratio = 1 = 1.33 = 1 1x3 1.33x3 1x3 3 4 3
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62. Calculating the empirical formula from elemental analysis data (Combustion data) E.g 1.00 g sample of compound A was burnt in excess oxygen producing 2.52 g of CO 2 and 0.443 g of H 2 O. Determine the empirical formula of the compound 1 mol CO 2 contains 1 mol C & 1 mol H 2 O 2 mol H = 0.688
63. the mass of oxygen = m sample – (m C + m H ) = 1.00 g – (0.688 g + 0.0492 g) = 0.263 g O Element C H O Mass/g 0.688 0.0492 0.263 Amount/mol = 0.0573 = 0.0492 = 0.0164 Simplest ratio of relative amount = 3.49 = 3.00 = 1.00 3.49x2 3.00x2 1.00x2 7 6 2
64. Empirical formula = C 7 H 6 O 2 Exercise 1. 0.535 g sample of thiophene, a carbon-hydrogen-sulphur compound used in manufacturing of pharmaceuticals, is burned completely in excess oxygen to yield 1.119 g CO 2 , 0.229 g H 2 O, and 0.407 g SO 2 . Determine empirical formula of thiopene.
65. Percentage composition from formula For an element in a compound = atoms of element x RAM x 100 Relative formula mass e.g. Calculate the % composition of hydrogen in C 12 H 22 O 11 Where RFM C 12 H 22 O 11 = 342.0 ANS: % C = 22(1.0) X 100 = 6.4 % 342.0 Exercise: Calculate the % of nitrogen, by mass, in Ca(NO 3 ) 3 Ans: 17.1