IB Chemistry HL IA Rate of reaction, Chemistry lab
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The document describes an experiment to determine how different concentrations of hydrochloric acid affect the rate of reaction with copper (II) powder. A colorimeter will be used to measure the absorbance of light by solutions containing copper (II) and hydrochloric acid over three minutes. Five concentrations of hydrochloric acid will react with 20g of copper (II) powder in separate trials. Variables like temperature, volume, and light intensity will be controlled. Absorbance readings will be taken and used to calculate the order of reaction and compare how concentration impacts the rate. The experiment will be repeated three times for each concentration to collect sufficient data.
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金属イオンの定性分析
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※採用活動において「篠原凜久」を知っていただくために使用しています。よって、全ての採用担当者にはファイルの閲覧のみしか許可していません。ファイルの複製および共有、不正使用は禁止といたします。採用活動にのみ使用していただけると幸いです。
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Experiment 1 Calorimetry .docx
Experiment 1: Calorimetry
Post lab
Rawan Douar, Albert Campbell, Riley
Richardson, Christopher Cardenas
02/10/17
Instructor: Meng Chen
CHM2046L
Section: 912
Introduction
We determined the change in enthalpy to be negative, which means energy is sendoff the system and entering the environments in the form of heat.
Calorimetry is the chemical process which is used to measure heat in chemical reaction. The apparatus used is the calorimeter. A coffee cup calorimeter is not technologically advanced but it is effective in stopping heat transfer between the system and the atmosphere. Because the cup is open to the air, this is a constant pressure measurement. Per the first law of thermodynamics, the total energy of an isolated system can neither be created nor destroyed. In other words, energy is preserved in chemical reaction.
Calorimeter will consist of two nested Styrofoam coffee cups and a plastic cover. It will use a temperature sensor armed with a thermocouple probe. There will be a hole in the plastic cover of your calorimeter for insertion of the probe. In this experiment, we are going to study about the redox reactions with coffee cup and calorimeter.
Hypothesis and Objectives
Using a coffee cup calorimeter, the heat of neutralization of HCl and NaOH is measured. From this, the enthalpy change for the neutralization of one mole of HCl can be calculated.
· Introduction to the technique of calorimetry, in which the heat is evolved or absorbed by a chemical reaction is incidental by measuring temperature vicissitudes in an insulated reaction container.
· Reaction involve strong bases and acids will produce more heat.
Methods
Following are the materials that are used in experiment.
· Coffee cup calorimeter thermometer
· Lid or parafilm
· 10 mL graduated cylinder
· HCL
· NaOH
· Water
· 250 mL beaker
Procedure
1. Set up calorimeter apparatus.
2. Measuring solution temperature before mixing.
3. Adding simultaneously HCl and NaOH to the coffee cup.
4. Measure temperature change after mixing.
5. Calculate enthalpy change.
(J. Kotz, P. Treichel, J. Townsend; Chemistry & Chemical Reactivity 7th ed. 2009)
Obtain 10 ml of cold water and get the temperature, and pour it into your calorimeter. Then do the same thing for hot water. After that, measure the final temperature when it reaches equilibrium. Use the initial and the final temperatures to measure Ccal. Now gather two 50 mL beakers, one for NaOH, and one for HCl. Use the 10-mL graduated cylinder and then add the 3 mL of HCl and 7 mL of water, measure the temperature and put it into your unfilled calorimeter. Do the same for NaOH. Then put the thermometer in and measure the exact last temperature of it.
Clean up, and do the same thing aga ...
2016 topic 5.1 measuring energy changes
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. The key points are:
- Exothermic reactions release heat while endothermic reactions absorb heat.
- Enthalpy change (ΔH) is the quantity of heat released or absorbed during a chemical reaction.
- Calorimetry experiments allow calculation of ΔH by measuring the temperature change of a reaction mixture.
- Sample problems demonstrate how to use calorimetry data like mass changes and temperature differences to calculate the enthalpy change for a reaction.
Equilibrium reactions.pptx
The document discusses reversible reactions and equilibrium reactions. It provides examples of the hydration and dehydration of cobalt(II) chloride and copper(II) sulfate. The document also discusses factors that affect equilibrium positions such as concentration, temperature, pressure, and catalysts. Finally, it summarizes the Haber process for producing ammonia and the contact process for producing sulfuric acid. Both processes use typical conditions of high pressure and temperature with a catalyst to favor production of the desired products.
Lesson : Enthalpy and Calorimetry
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. It discusses key concepts like:
1) The standard enthalpy change (ΔH°) is the enthalpy change measured under standard conditions of temperature and pressure.
2) Calorimetry can be used to determine enthalpy changes by measuring the temperature change of a reaction mixture in a calorimeter.
3) Sample problems demonstrate how to use calorimetry data like temperature changes, masses, and concentrations to calculate enthalpy changes for chemical reactions.
Chapter 1 Rate of Reactions
The document discusses rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. It describes several factors that affect rate based on collision theory, including surface area, concentration, temperature, catalysts, and pressure. It gives examples of how scientific understanding of rate of reaction enhances quality of life, such as refrigeration, pressure cooking, cutting food into smaller pieces, making margarine, and burning coal.
Chapter 4 Thermochemistry
This document discusses thermochemistry and energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and how to construct energy level diagrams to represent them. Specific heats of reaction like combustion, precipitation, displacement, and neutralization are also explained. Experiments to determine various heats of reaction are described. The relationships between the heat of reaction and type of reactants, as well as the number of carbons in alcohols are also summarized.
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This document provides an overview of stoichiometry and related concepts from a YouTube chemistry lecture series. It defines stoichiometry as dealing with quantitative relationships between reactants and products in balanced chemical equations. Key points covered include mole calculations using molar mass and Avogadro's number, determining limiting and excess reactants, and calculating theoretical and percent yield of products. Worked examples are provided for several stoichiometry calculations.
LabQuest 18 Chemistry with Vernier 18 - 1 Additi.docx
LabQuest
18
Chemistry with Vernier 18 - 1
Additivity of Heats of Reaction:
Hess’s Law
In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by
three reactions. One of the reactions is the same as the combination of the other two reactions.
Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the
sum of the heats of reaction for the other two. This concept is sometimes referred to as the
additivity of heats of reaction. The primary objective of this experiment is to confirm this law.
The reactions we will use in this experiment are:
(1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions.
NaOH(s) Na+(aq) + OH–(aq) H1 = ?
(2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous
solution of sodium chloride.
NaOH(s) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H2 = ?
(3)
Solution
s of aqueous sodium hydroxide and hydrochloric acid react to form water and
aqueous sodium chloride.
Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H3 = ?
In the space below, combine two of the above equations algebraically to obtain the third
equation. Indicate the number of each reaction on the shorter lines.
______ __________________________________________________________________
______ __________________________________________________________________
______ __________________________________________________________________
You will use a Styrofoam cup in a beaker as a calorimeter, as shown in Figure 1. For purposes of
this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is
negligible. Even if heat is lost to either of these, it is a fairly constant factor in each part of the
experiment, and has little effect on the final results. You will make three grand assumptions in
this experiment:
1. The specific heat of solution is equivalent to the specific heat of water.
2. The density of solution is equivalent to the density of water.
3. All solutions are identical in temperature before mixing.
OBJECTIVES
In this experiment, you will
Combine equations for two reactions to obtain the equation for a third reaction.
Use a calorimeter to measure the temperature change in each of three reactions.
Calculate the heat of reaction, H, for the three reactions.
Use the results to confirm Hess’s law.
LabQuest 18
18 - 2 Chemistry with Vernier
MATERIALS
LabQuest 4.00 g of solid NaOH
LabQuest App ring stand
Temperature Probe utility clamp
50 mL of 1.0 M NaOH stirring rod
50 mL of 1.0 M HCl Styrofoam cup
100 mL of 0.50 M HCl 250 mL beaker
100 mL of water
PROCEDURE
Reaction 1
1. Obtain and wear goggles.
2. Connect the Temperature Probe to LabQuest and choose New from the File menu. If you
have an older sensor that does not auto-ID, manually ...
10 stoichiometry
This document provides an overview of stoichiometry concepts including mole ratios, mole-mole conversions, mole-mass conversions, mass-mole conversions, mass-mass conversions, and limiting reactants. Examples are provided to demonstrate how to use these concepts to solve stoichiometry problems involving amounts in moles or grams of reactants and products. The key aspects are determining the limiting reactant, calculating the theoretical yield based on this reactant, and identifying any excess reactants.
SPM F5 Chapter 1 Rate of Reaction
The document discusses rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. Rate of reaction is affected by several factors including surface area, concentration, temperature, catalysts and pressure (for gas reactions). The collision theory is also explained, stating that reactions only occur during effective collisions where particles attain sufficient kinetic energy to overcome the activation energy barrier. Examples of how scientific understanding of rate of reaction enhances quality of life through applications like food storage, cooking and petroleum processing are provided.
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The document discusses chemical reactions and stoichiometry. It defines stoichiometry as using ratios to determine quantities of reactants and products in a chemical reaction. It explains that coefficients in a balanced chemical equation represent molar ratios and can be used to determine moles, mass, and volume of substances in a reaction. It provides examples of solving stoichiometry problems, including determining limiting reactants.
Chemistry - Chp 12 - Stoichiometry - PowerPoint
The document discusses stoichiometry, which is the calculation of quantities in chemical reactions based on a balanced equation. It explains how to interpret balanced equations in terms of particles, moles, mass, and gas volume. It also covers how to perform stoichiometric calculations using mole-mole, mole-mass, and volume-volume conversions based on molar ratios from balanced equations.
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This document summarizes key concepts from a chapter on chemical quantities and aqueous reactions:
1) Stoichiometry allows one to predict amounts of products from a balanced chemical equation based on amounts of reactants. Molar ratios from balanced equations give relationships between amounts of substances in moles or grams.
2) The limiting reactant is the first reactant to be completely used up in a chemical reaction. It limits the amount of product that can be formed.
3) Solutions are homogeneous mixtures with a solvent and one or more dissolved solutes. Concentration is quantified as molarity - moles of solute per liter of solution.
Ch 9 Stoichiometry
The document discusses stoichiometry and limiting reactants in chemistry. It provides examples of calculating molar masses of compounds, moles of reactants and products in chemical reactions, and determining which reactant is limiting. It emphasizes that the limiting reactant determines the maximum amount of product that can be formed, and any excess reactant remains unused after the reaction completes.
Detecting Signs Of Chemical Change
The document describes an experiment to observe signs of chemical change. Various substances like cobalt chloride, zinc, and copper sulfate are combined with other liquids and metals. Observations are recorded about color changes, precipitates forming, gases bubbling, and changes to solids. The purpose is to determine if chemical or physical changes occurred based on these indicators. Data tables show the substances combined and observations made to identify chemical changes.
Grade 9 Chemistry ppt.pptx
This document provides an overview of stoichiometry including definitions, types of stoichiometry problems (mass-mass, volume-volume, mass-volume), and key concepts like limiting/excess reactants and theoretical, actual, and percentage yields. It defines stoichiometry as the quantitative relationship between reactants and products in a balanced chemical equation. There are three main types of stoichiometry problems - mass-mass problems calculate the mass of one substance given the mass of another using mass ratios or mole ratios, volume-volume problems use the molar volume and Avogadro's law, and mass-volume problems relate the mass of one substance to the volume of another. Limiting reactants are those that are completely consumed, while excess
Thermochemistry ok1294993378
The document discusses energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and standard enthalpy change. It provides examples of how to calculate enthalpy changes from experimental temperature change data using concepts like specific heat capacity. Hess's law, which states the enthalpy change of a reaction is equal to the sum of enthalpy changes of the steps in a reaction mechanism, is also introduced.
Module 3 in Methodology course
The document describes a scientific study that compares two different chemical oxygen demand (COD) test kits. Standard COD solutions and wastewater samples were tested using a COD kit containing mercury and a mercury-free kit. The results from both kits were analyzed statistically by examining the mean and standard deviation of the data. The study aimed to cross-validate the two kits by comparing the analyzed data. The results showed that the kits produce the same measurements for COD standard solutions, but do not overlap well when measuring wastewater samples.
Chemistry - Chp 12 - Stoichiometry - PowerPoint
The document summarizes key concepts from Chapter 12 of a chemistry textbook on stoichiometry. It discusses how to interpret and work with balanced chemical equations, including in terms of particles, moles, mass, and gas volume. It explains the concepts of limiting reagents, theoretical yield, actual yield and percent yield. Key steps for solving stoichiometry problems are outlined.
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LabQuest 18 Chemistry with Vernier 18 - 1 Additi.docx
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IB Chemistry HL IA Rate of reaction, Chemistry lab
- 1. HL Chemistry AssiaChelaghma Using Colorimeter to Determine the Effect of Concentration on the Rate of Reaction Introduction: When a light passes through a solution in a tube, electrons absorb light. The intensity of the light emitted through the tube will be less than the light absorbed. Copper II powder reacts with hydrochloric acid according to the equation: Cu(s) + 2HCl(aq) → CuCl2(s) + H2(g) When the reaction takes place, copper II chloride and hydrogen gas are produced. The concentration of hydrochloric acid decreases. Colorimeter is used to determine the rate of reaction by measuring the absorbance of a monochromatic light by the solution that contains excess copper II and hydrochloric acid. When the absorbance of light is obtained, the rate of reaction can be determined. Researchquestion: How do different concentrations of 5cm3 hydrochloric acid that react with 20g of copper II powder affect the rate of reaction? Variables: Independent variables: The concentration of hydrochloric acid. Dependant variables: The absorbance of light during three minutes. Controlled variables: Temperature of the solution must be kept constant so I will use a thermometer of check the temperature of the solution and keep it constant. Volume of the solution must be kept constant. So I will use the same volume of hydrochloric acid and the same mass of copper II. Time should be the same so that I can compare the absorbance of light between different concentrations. Intensity of the monochromatic light should be kept the same. Apparatus: Electronic balance to 0.01g. Five test tubes for different solutions of hydrochloric acid (of different concentrations).
- 2. HL Chemistry AssiaChelaghma Colorimeter to measure the absorbance of light. Two temperature sensors Five containers, each one contains 20g of Copper II powder Five different solutions of hydrochloric acid of these different concentrations: 0.25𝑚𝑜𝑙 𝑑𝑚−3 ; 0.50𝑚𝑜𝑙 𝑑𝑚−3 ; 0.75𝑚𝑜𝑙 𝑑𝑚−3 ; 1.25𝑚𝑜𝑙 𝑑𝑚−3 ; 1.50𝑚𝑜𝑙 𝑑𝑚3 Designof the experiment: The picture below shows how the colorimeter works: The picture below shows a real colorimeter: Method: Set up the experiment shown in the design above. Put 20g of copper II powder in the tube of the colorimeter. Set the colorimeter on with the monochromatic light. Put one temperature sensor inside the tube that contains copper II to control temperature of the solution later. Put the other temperature sensor in the room to keep room temperature under control. Add 5cm3 of hydrochloric acid to the copper II. Take the results of the absorbance of light. Propagate the graphs and calculate the order of reaction. Repeat the experiment using another concentration and then find the order of reaction.
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