Electrochemistry Lab Report

An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

Name: Amra Aliyu Lab partner: Jamie Liang Lab: Empire of Electricity Course: Chem 106 Date: 7/11/2015 INTRODUCTION A galvanic cell is an electrochemical cell that goes through a redox reaction and produces electrical energy . It converts chemical energy to electrical energy and the energy goes from the anode to the cathode. In this lab we had manipulate an exothermic zinc reaction to produce electricity.

but then it turned into an aqueous solution back to a solid repeating in a cycle. The same happened with the zinc because when we added zinc and stirred it in the solution it “disappeared” but actually what happened was that the zinc dissolved into the solution and displaced the copper into a solid and also zinc sulfate, ZnSO4(aq). Therefore, in this experiment there was no compound or anything that was destroyed due to the law of conservation of mass which means that matter isn't destroyed neither is the elements and

1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give at least three different examples. (15 points)

After 1-2 minutes results were recorded in a observation table. The independent variable in this reaction is the amount of copper wire, magnesium ribbon, and zinc metal (powder form) and the 1/3 filled wells of copper (II) nitrate, magnesium nitrate, or zinc nitrate. The dependent variable in this reaction is the reaction that occured between the metals and the solution. Part B: Using the same experimental design as part A, three drops of sodium

The purpose of this experiment was to observe various reactions including copper at different stages of the cycle and to identify

Reacting a group I metal with Cl2 makes a binary ionic chloride with 1 metal to 1 chlorine (e.g. NaCl). Similarly, reacting group II metals give a stoichiometry of 1 metal to 2 chlorines and group I metals with Br2 give a 1:1 stoichiometry, for example MgCl2 and KBr, respectively. How can elements with such diffent masses such as Cl and Br react in the same stoichiometry with elements with such different masses as Na and K? It is because of they have the same number of valence electrons. Valence electrons are the higher energy, reactive electrons around an atom, which contrast with the lower energy, unreactive core electrons.

However, the results were not precise and accurate enough due to some experimental errors and human errors. First, the identicalness of test tubes. The interior of the test tubes were not the same and thus even though the measurement of the hydrogen peroxide and copper (II) sulphate were made precisely and accurately, the volume may differ. This contributed to countless of minor errors thorough the experiment, affecting the precision and accuracy of the result. The volume added should be weighed on the electronic balance every time after substance being added to obtain the most accurate results.

Method Prior to the experiment, the LabQuest must be set up and the conductivity probe must be calibrated. Calibrate the conductivity probe connected to a LabQuest using a solution of known conductivity. In this experiment, a solution with a conductivity of 1000 μS/cm was used. Choose “Calibrate” from the menu and choose “Calibrate Now”. Then submerge the conductivity probe into the standard solution and type in the known value of the solution; 1000 in this case.

Effect of ionic strength These reactions were also carried at different µ (0.050 to 0.30 i.e., at 0.050, 0.10, 0.150, 0.20, 0.250 and 0.30), keeping the concentrations of Fe(IIII), [PABAH] / [PCBAH], PPDTS and H+ constant. The data (Table 3.) show that ionic strength has little effect on these reactions. Determination of protonation constant of PABAH and

Swikriti Dasgupta HL IB Chemistry Determination of the Relationship Between Concentration and Rxn in Voltaic Cell: Research Question: How does the concentration of CuSO4 affect the voltaic cell as measured by voltmeter? Variables: Table 1: Independent Variable for Determining the Relationship Between Concentration and Rxn in Voltaic Cell: Independent Variable How it will be changed CuSO4 CuSO4 solution was diluted to 50% using distilled water. Then the diluted CuSO4 was further diluted to prepare 20%, 40%, 60%, 80%, and 100% dilution.

Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of

The rate constant (k) is a proportionality constant in the relationship between rate and concentrations, but changes when temperature changes. The effect of temperature on a reaction rate is given by the Arrhenius equation2 (Equation 2): k =Ae-Ea/RT (Eq.2) where A is the collision frequency factor, Ea the activation energy of the reaction, T the absolute temperature, and R the ideal gas constant. This experiment

Chemistry IA Background information: Introduction: Electrolysis it’s a chemical process that when you pass an electric current into a solution or a liquid that contains ions to separate substances back to their original form. The main components that are required for electrolysis to take a place are:  Electrolyte: it’s a substance that when dissolved in water it ionize and then it will contain free moving ions and without these moving ions the process of electrolysis won’t take place.  Direct current (DC): This current provides the energy needed to discharge the ions in the electrolyte  Electrodes: it’s an object that conducts electricity and it’s used in electrolysis as a bridge between the solution and power supply. A great example

Since equilibrium cannot be reached, an electrochemical driving force is generated which acts on the ions. It is derived by finding the difference between the membrane potential obtained and the equilibrium potential expected. The sign of the value of this force decides the direction of movement of ions. Since we have cations (positive ions), a positive value shows movement of ions outside the cell membrane and a negative value shows movement of ions inside the cell membrane. If the value is equal to that of the equilibrium potential, the driving force acting on the ion is 0.