We think you have liked this presentation. If you wish to download it, please recommend it to your friends in any social system. Share buttons are a little bit lower. Thank you!
Presentation is loading. Please wait.
Published byKailey Hucke
Modified about 1 year ago
Welcome to SimpleChemConcepts.com The PowerPoint will auto-run by itself and it takes about 2 min to complete.
Video 1: Rate of Reaction Rate of Reaction affected by 5 factors: ↑ in Temperature ↑ in Rate of Rxn ↑ in Pressure (for gas) ↑ in Rate of Rxn ↑ in Conc. (for soln) ↑ in Rate of Rxn ↑ in Surface A. (for solid) ↑ in Rate of Rxn Addition of Catalyst ↑ in Rate of Rxn ©SimpleChemConcepts.com
Question from Top School ©SimpleChemConcepts.com Graph I: It shows the reaction between 1.0g of magnesium ribbon and excess 0.1M dilute hydrochloric acid at 25oC On the same axes, draw and label the following: GraphsFor reaction between IIReaction btw 0.5g of Mg ribbon & excess 0.1M dilute HCl @ 25 o C IIIReaction btw 1.0g of Mg powder & excess 0.1M dilute HCl @ 25 o C IVReaction btw 1.0g of Mg ribbon & excess 0.05M dilute HCl @ 25 o C VReaction btw 1.0g of Mg ribbon & excess 0.1M dilute HCl @ 15 o C Mass of H 2 gas / g t / s
Graph 1: Reaction btw 1.0g of Mg ribbon & excess 0.1M dilute HCl @ 25 o C Analysis: Reaction Products: MgCl 2 salt + H 2 gas Mg determines the mass of H 2 gas produced Point where graph plateaus or levels off Mg has been used up Extrapolation to Y-axis Max. amount of H 2 gas produced Extrapolation to X-axis Time when rxn stops Mass of H 2 gas / g t / s Conditions: 1.0g of Mg ribbon Excess 0.1M dilute HCl @ 25 o C ©SimpleChemConcepts.com
Graph Ⅱ : Reaction btw 0.5g of Mg ribbon & excess 0.1M dilute HCl @ 25 o C Conditions: O.5g of Mg ribbon Excess 0.1M dilute HCl @ 25 o C Analysis: All conditions same except half of Mg ribbon used Mass of H 2 gas produced to be half of Graph Ι Rxn stops/plateaus faster than Graph Ι Mass of H 2 gas / g t / s ©SimpleChemConcepts.com
Graph Ⅲ : Reaction btw 1.0g of Mg powder & excess 0.1M dilute HCl @ 25 o C Conditions: 1.0g of Mg powder Excess 0.1M dilute HCl @ 25 o C Analysis: All conditions same except Mg powder used Mass of H 2 gas produced to be same as Graph Ι Surface Area of solid reactant Rate of Reaction Initial gradient is steeper & slope plateaus off earlier Mass of H 2 gas / g t / s ©SimpleChemConcepts.com
Graph Ⅳ : Reaction btw 1.0g of Mg ribbon & excess 0.05M dilute HCl @ 25 o C Conditions: 1.0g of Mg ribbon Excess 0.05M dilute HCl @ 25 o C Analysis: All conditions same except conc. of excess HCl is halved Mass of H 2 gas produced to be same as Graph Ι Reactant particles per unit volume of solution ↓ Rate of Reaction ↓ Initial gradient is gentler & slope plateaus off later Mass of H 2 gas / g t / s ©SimpleChemConcepts.com
Graph Ⅴ : Reaction btw 1.0g of Mg ribbon & excess 0.1M dilute HCl @ 15 o C Conditions: 1.0g of Mg ribbon Excess 0.1M dilute HCl @ 15 o C Analysis: All conditions same except Temp. is reduced by 10 o C Mass of H 2 gas produced to be same as Graph Ι General Rule: Every 10 o C Doubles Rate of Rxn Rate of Rxn ↓ by half Take twice the amount of time for Rxn to stop Initial gradient is gentler & slope plateaus off much later Mass of H 2 gas / g t / s ©SimpleChemConcepts.com
Final Answer Mass of H 2 gas / g t / s ©SimpleChemConcepts.com
For more Chemistry Tips & Strategies, Visit Us @ www.SimpleChemConcepts.com ©SimpleChemConcepts.com
Rates of Reaction. Familiar with factors which affect reaction rate ◦ Temperature ◦ Particle Size / surface area ◦ Concentration ◦ Catalyst Average.
© Boardworks Ltd of 49 KS4 Chemistry Rates of Reaction.
6.1 - Expressing Reaction Rates Reaction Rate – The change in amount of reactants or products over time. Rate of Reaction = Amount of A final – Amount.
Calculation of excess In an excess calculation you will be given the quantities of two reactants.
Rate Of Reaction Investigation D. Crowley, Rate Of Reaction Investigation Your task is to investigate what affects the rate of reaction between.
RATES OF REACTION A guide for GCSE students 2010 SPECIFICATIONS KNOCKHARDY PUBLISHING.
Rates of Reaction To revise the 4 factors that affect rates To revise methods of measuring rates.
Calderglen High School
Calcium carbonate (marble) hydrochloric acid carbon dioxide.
Higher Chemistry Unit 1(a) Identifying a reactant in excess.
Problems from end of chapter 11. Chapter 11 Slide 2 of A weather balloon has a volume of 750 mL when filled with helium at 8 o C at a pressure.
Rates of Reactions Teacher Version. Rate measures how fast or slow a chemical reaction occurs Who cares about rates of reactions? ◦ Chemical engineers.
Kinetics - graphs Sketch volume-time graphs for: 1.hydrogen produced during a magnesium and hydrochloric acid reaction both reactants are in stoichiometric.
04/24/2016 Topic 5 – Chemical Reactions. 04/24/201604/24/16 Endothermic and exothermic reactions Step 1: Energy must be SUPPLIED to break bonds: Step.
Factors Affecting the Rate of a Chemical Reaction 1. temperature 2. concentration 3. pressure (gases) 4. surface area 5. orientation (molecules must collide.
How can I slow the rate of this reaction down? Starter: What does rate mean?
IGCSE CHEMISTRY SECTION 4 LESSON 3. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.
Reaction Rates Speed matters! *Watch a Video!*. Reaction Rate Decrease in concentration of reactants with time or Increase in concentration of products.
Chapter 12: Chemical Kinetics Kinetics and Graphs.
Factors Affecting the Rate of a Chemical Reaction The following events must occur before a reaction can proceed: 1.The reactant particles must collide.
Unit 1 rates. Go to question d. A small rise in temperature produces a large increase in the reaction rate. An experiment was carried.
TOPIC 2 Speed of Reactions A chemical reaction can be represented by a Chemical Equation. A chemical reaction can be represented by a Chemical Equation.
Speed of Reactions A chemical reaction can be represented by a Chemical Equation. The starting chemicals are called Reactants and the new ones made the.
1 of 39© Boardworks Ltd of 39 © Boardworks Ltd of 39 What does rate of reaction mean? The speed of different chemical reactions varies.
Higher Chemistry Unit 1(a) Collision Theory and Particle Size.
Chemistry 2 Lesson 4.2 Collision Theory AQA Additional Science.
Rates of Reaction In this unit you will investigate what makes chemical reactions go faster. At the end of the unit you will have a 2 hour practical test.
Chemistry ( ) Rates of Reaction © SSER Ltd..
Rate Of Reaction & Temperature Noadswood Science, 2012.
Topic 6 Kinetics Rates of reaction Collision theory.
TOPIC A FACTORS AFFECTING RATES OF REACTION. Factors that influence the rate of a chemical reaction. Each factor has a noticeable effect on the microscopic.
Topic 06 – Kinetics 6.1: Rates of Reaction IB Chemistry T06D01.
EOC Chemistry Review II. Which is an empirical formula? A. C 2 H 2 B. H 2 0 C. H 2 O 2 D. C 6 H 12 O 6.
Final Jeopardy Subterm 2 Gases* Solutions* Equilibrium* Acids & Bases* Thermochemistry* Nuclear Chemistry*
Collision Theory Factors affecting rate Particle size affects rate.
Section 12.2 Factors that Affect Gas Pressure. After reading section 12.2, you should know: How the amount of gas and the volume of the container affect.
Factors affecting Reaction Rates Press the left mouse key to move on on each page.
Chapter 1: Rate of Reaction Rate of Reaction. Which reaction is faster?
A solution is a homogeneous mixture that is the same all the way throughout. Water and Soda is an example of a homogeneous mixture. Homogeneous mixtures.
Wednesday 5/2/12 Pick up the Reaction Rate Note Packet off the front green demo table and date it.
Temperature and the Rate of Reaction L.O: To understand the effect of temperature on the rate of a reaction.
© Use your knowledge about chemical reactions to answer the questions. 1.
Physical Science Chapter 15 Solubility. Solution: A homogeneous mixture, in which the particles are evenly distributed throughout.
Integrated Rate Equation Volumemeasurement Colorimetry Physical Method Physical Chemistry: Chemical Kinetics C. Y. Yeung (CHW, 2009) AL CHEM REVIEW Chemical.
Expressing and Measuring Reaction Rates SCH 4U. Expressing Reaction Rates Understanding the rate of a reaction can be very important to understanding.
Topic 4. Collision theory Chemical reactions only occur when reacting particles collide with each other with sufficient energy. The minimum amount of.
Title: Lesson 3 Rate Law and Reaction Order Learning Objectives: – Know that rate law can only be derived from experimental data – Understand the concept.
© 2017 SlidePlayer.com Inc. All rights reserved.