Electrolysis of copper sulphate
Danny Aburas Introduction Electrolysis is referred to as the decomposition of a compound by applying a flow of electron current (electricity) into the solution. Electrolysis can only occur in solutions of electrolytes. Electrolytes are compounds that are able to conduct electricity when in a molten state or when dissolved in water. Electrolytes cannot conduct electricity when they are in a solid state as in this state the ions are held in a 3 dimensional lattice in which they cannot move, thus preventing the flow of electricity through the compound. If, however the compound is molten or dissolved in water, it’s component ions dissociate and are no longer held by this lattice thus, can move around and furthermore, meaning electrolysis can occur. Usually in electrolysis, something will be reduced (gain in e-) and something will be oxidized (loss of e-). Reduction takes place on the cathode (negative electrode) while oxidation occurs on the anode (positive electrode). This particular experiment involves the electrolysis of copper (II) sulphate using a pair of copper electrodes. The copper electrodes are “active” meaning they take a part in the electrolysis. First, the electric current passed through the electrolytic cell will cause the copper sulphate solution to dissociate into it’s two component ions, Cu2+ and SO42-. .The copper anode (+) will dissolve and fall into
The aim of this experiment is to examine the enthalpy of combustion of the first five alcohols and to see how does it change with the increasing chain length
united world college maastricht Internal Assessment Chemistry Enthalpy of combustion of Alcohols Merdanovic Imman [Pick the date] ________________ Introduction The aim of this experiment is to examine the enthalpy of combustion of the first five alcohols and to see how does it change with the increasing chain length, in other words , with the changes in the number of carbon atoms . An alcohol is an organic compound in which the hydroxyl functional group (-OH) is bound to a carbon atom.The enthalpy of combustion () is the energy released as heat , when a compound undergoes complete combustion with oxygen under standard conditions. Carbon atoms in alcohols are linked together by a covalent bond. Every covalent bond has a 'bond energy', which it is the amount of energy needed to break the bond or the amount of energy given out as a bond is formed. However, it is important that the covalent bond is very strong and that it does not break easily, on contrary, it requires a lot of energy to be break . Alcohol's react with oxygen in the air to form water and carbon dioxide. The reaction that is involved in burning alcohols is exothermic because heat is given out. From this reason the reactant energy is higher than that of the product. The energy is given out when forming the bonds between the new water and carbon dioxide molecules. The amount of energy produced by such
Change of Potential Difference in Voltaic Cells Lab Report
The Change of potential difference in Voltaic Cells I. Introduction Oxidation-Reduction (redox) reaction is a group of reactions that are linked to the transfer of electrons between species. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Each reaction by itself is called a half-reaction because there must be two halves of reactions to form a whole reaction. When a redox reaction takes place, electrons are transferred from one species to the other. If the reaction is spontaneous, energy is released. A Voltaic Cell (Galvanic Cell) is an electrochemical cell that uses spontaneous redox reactions to generate electricity. It consists of two separate half-cells. A half-cell is composed of an electrode within a solution containing Mn+ ions in which M is the metal and n is the number of charges of the metal. The two half cells are linked together by a wire running from one electrode to the other with a voltmeter to measure the potential difference between the two electrodes. A salt bridge also connects to the half cells to keep solutions neutral and allow free flow of electrons. In the absence of a salt bridge, electrons won't transfer and the voltmeter won't measure any voltage. When an electrode is oxidized in a solution, it is called an anode and when an electrode is reduced in a solution it is called a cathode. The electrons will
Group 4
An investigation on the development of car safety and the importance of airbags Chemistry experiment to simulate the inflation of an airbag in case of a car crash Aim Our aim is to create a chemical reaction to demonstrate the rapid inflation used in automobiles. The inflation of an airbag is a very fast reaction, and the typical reactants used are a mixture of Calcium carbonate (CaCO3), Potassium nitrate (KNO3) and Silicon dioxide. When a car crash occurs a sensor in the car's airbag triggers the reaction that will save the drivers life if the speed at which he is moving is greater than 16-24 km/h-1. The nitrogen has to be produces more quickly than the driver hitting the steering wheel. The entire reaction is completed in less than 1/25 of 1 sec, because of the danger of this reaction, to demonstrate in a similar way the reaction that takes place in an airbag we have chosen to inflate a balloon using the gas obtained by the reaction of a metal acid to produce sodium carbonate. Equation Ca(s) + 2HCl(aq) = Ca(aq) + (g) + O(l) Materials -Conical Flask -Cork with delivery tube -heat mats -spatula -chemicals (baking soda) - goggles (safety glasses) Procedure • Gather all apparatus needed for the entire experiment • Set up all apparatus • Pour CaCo3 into the conical flask • Add the HCl to the solution already in the conical flask • Cover the
A comparison of various proprieary antacids
Lab 14: A Comparison Of Various Proprietary Antacids Planning A: Research Question: How to determine and compare between a set of antacids( Eno powder, Tums Tablets and Zolicid gel), which antacid neutralizes the most moles of stomach acid( Hydrochloric acid, HCl), by conducting back-titration reactions using standardized hydrochloric acid(0.5M) and standardized sodium hydroxide(0.5M). Hypothesis: In this experiment I plan to compare between a set of antacids, which antacid neutralizes the most moles of Hydrochloric acid(0.5 M), as this will help me to establish their relative effectiveness in helping to reduce excess stomach acidity. I am going to use back titration reactions whereby I will place a fixed volume, 25 cm3 of standardized hydrochloric acid, 0,5M, in a conical flask. Then, I shall add the maximum daily dosages of each individual antacid to the hydrochloric acid in the flask. The antacid which is supposed to neutralize some of the excess hydrochloric acid of the stomach, will neutralize some of the excess hydrochloric acid in the conical flask. The number of moles of hydrochloric acid to be neutralized would be 0.0125 moles. I will then neutralize the unreacted hydrochloric acid, if any, using standardized aqueous sodium hydroxide(0.5 M) from a 50 cm3 burette. In order to clearly note the point of neutralization( the equivalence point), I will use
Hesss Law Lab, use Hesss law to find the enthalpy change of combustion of magnesium which is a highly exothermic reaction.
Hess's Law Lab Hess's Law Hess's Law states that that the value of ?H for a reaction is the same whether it occurs directly or as a series of steps. Purpose To use the Hess's law to find the enthalpy change of combustion of magnesium which is a highly exothermic reaction. Determining the enthalpy change for the reactions of Mg in HCl(aq) and MgO(s) HCl(aq) experimentally and alongside that use the enthalpy change for hydrogen gas (Table value) when it is combusted , to find the enthalpy change for the combustion of magnesium. HYPOTHESIS The heat of combustion for magnesium can be determined by determining the heat of reaction for the following reactions: ) Mg(s) + 2HCl (aq) › MgCl2(aq) + H2(g) 2) MgO(s) + 2HCl(aq) › MgCl2(aq) + H2O(l) 3) H2(g) + 1/2 O2(g) › H2O(l) Once these values have been obtained, I can add or subtract these values in order to achieve the heat of combustion for magnesium. Apparatus • Goggles • Lab apron • Electric balance • 100 mL graduated cylinder • 2 plastic foam cup • Thermometer • Beaker ( transportation of HCl) Procedure I began this experiment by gathering all the required lab equipment and the necessary chemicals. I found a lab station and started my investigation. I decided to start with hydrochloric acid and magnesium first. I measured 50 cm3 1.00 mol/dm3 amount of HCl solution using a
Chemistry Extended Essay - Viscosity of Xanthan Gum solutions
EXTENDED ESSAY - Chemistry - How does the introduction of xanthan gum into a solution and the resulting increased viscosity affect the rates of reactions occurring within that solution? Word Count: 3731 ANDREW PELLY IB NUMBER 000834 027 CONTENTS SECTION TITLE PAGE Abstract 2 Introduction 3 2 Research question 4 3 Background information 4 i. Xanthan gum in solution 4 ii. Electrolytic refinement 5 iii. Na-H2O ionisation reactions 6 4 Method 6 i. Viscosity measurements 6 ii. Rate of reaction measurement: electrolytic refinement 7 iii. Rate of reaction measurement: neutralisation reactions 7 5 Data 8 i. Relationship between xanthan gum concentrations and time taken for burette to empty, in order to model viscosity 8 ii. Comparison of mass change of the cathode in an electrolytic purification reaction involving a copper anode and a copper cathode in a copper sulphate solution 9 iii. Peak temperatures achieved during Na/H2O ionisation reaction 11 6 Analysis 12 i. The homogeneity assumption 12 ii. Sodium and water reaction 12 iii. Hydrogen bonding in water 13 7 Conclusion 15 i. Xanthan gum solution viscosity testing 15 ii. Electrolytic refinement testing 15 iii. Na/H2O ionisation reaction 15 Appendix 16 i. Bibliography 16 Abstract In this essay, I researched the question "How does the introduction of
Research question: how to convert NaOH to NaCl by two different routes , and measure the enthalpy changes for each one in order to test Hesss law ?
Name: Rand Ishaq School: katedralskolan chemistry IA 2011-12-17 converting NaOH to NaCl by two different routes , and measuring the enthalpy changes for each one in order to test Hess’s law . aim: the aim is to measure and compare the quantity of heat involved in three reactions and to provide experimental verification of Hess's Law research question: how to convert NaOH to NaCl by two different routes , and measure the enthalpy changes for each one in order to test Hess’s law ? general background: The foundation of the study of thermochemistry was laid by the chemist Germain Hess, who investigated heat in chemical reactions during the last century. One statement of the law that bears Hess's name says: The enthalpy change for any reaction depends on the products and reactants and is independent of the pathway or the number of steps between the reactant and product In this experiment, the enthalpy of several reactions will be determined using the method of calorimetry. The reactions that will be considered are the following: : NaOH (aq) + HCl (aq) NaCl (aq) + H2O (l) All of the reactions in this experiment are exothermic. As heat is given off for each reaction, the temperature of the mixture will increase. The amount of heat given off by the reaction can be calculated according to the following equation: q= mcΔT Where: m = mass
Esterification Equilibrium
IB Group 4 Internal Assessment Chemistry Biology Physics Name: Date(s): Candidate Number: Session: Level: Investigation Title: Internal Assessment Marking Form Criterion Required Aspects Level Complete (2) Partial (1) Not at All (0) Data Collection and Processing Records appropriate quantitative and associated qualitative raw data, including units and uncertainties where relevant. Records appropriate quantitative and associated qualitative raw data, but with some mistakes or omissions. Does not record any appropriate quantitative raw data or raw data is incomprehensible. 2 0 Aspect 1 - Recording Raw Data Aspect 2 - Processing Raw Data Processes the quantitative raw data correctly. Processes quantitative raw data, but with some mistakes and / or omissions. No processing of quantitative raw data is carried out or major mistakes are made in processing. 2 0 Aspect 3 - Presenting Raw Data Presents processed data appropriately and, where relevant, includes errors and uncertainties. Presents processed data appropriately, but with some mistakes and / or omissions. Presents processed data inappropriately or incomprehensibly. 2 0 Conclusion and Evaluation States a conclusion, with justification, based on a reasonable interpretation of the data. States a conclusion based on a
Chemistry Titration Acid Base Lab
Acid-Base Titration Lab By: Shawn Vickar Question: What effect does an indicators pH range have on the end point of the titration of vinegar and 1.00 mol dm-3 of sodium hydroxide solution? Equation: CH3COOH (aq) + NaOH (aq) NaCH3COO (aq) + HOH (l) Data Collection Table A: Table Representing the Initial Volume of NaOH in the Burette, the Final Volume of NaOH in the Burette and the Difference between Those Values for Specific Trials When Using Different Indicators. There were a minimum of three trials performed for this lab as there needed to be three of the same difference between the final and initial burette readings of the sodium hydroxide. This is due to the fact that a titration lab requires one to acquire three of the same values for this section to understand the exact amount of base required to reach the endpoint of the reaction. Indicator Initial Volume of NaOH solution (ml) ±0.05 Final Volume of NaOH solution (ml) ±0.05 Difference Between the Final and Initial Burette Readings (Volume of NaOH used) (ml) ±0.1 Qualitative Observations Phenolphthalein 0.0 0 0.90 0.9 The indicator is clear and transparent at first. However, when the base is added and the endpoint has been reached, the color changes to a light pink. If over titration occurs, the solution will be a fluorescent pink color. 0.90 2.30 1.4 2.30 3.20 0.9 3.20 4.10 0.9