Aim / Research Question:
The aim of this investigation was to determine how five different metals of differing reactivity reacting with Copper Sulfate solution would affect the enthalpy change of the reaction.
Introduction:
The original idea for this investigation was developed from an in-class experiment done earlier in the year during our energetics unit where we learnt about enthalpy changes within a reaction by conducting an experiment between Copper Sulfate solution and Zinc. This experiment stimulated follow up questions, which were how would the enthalpy change differ for different metals of differing reactivity? Why would the changes in enthalpy differ for every metal?
I decided that the experiment would focus on conducting reactions between Copper Sulfate and five different metals. The enthalpy change of each
…show more content…
reaction would be calculated and then placed against the reactivity chart of all five metals. This would then determine if the reactivity of metals had an affect on the absolute enthalpy change. Background: Understanding the reactivity of metals can help predict how the metals will react and which metals they may displace in a single displacement reaction. A single displacement reaction is defined as a chemical reaction in which a reactant is exchanged for an ion of the second reactant. In a single displacement exothermic reaction, energy is released or given off during the reaction. The energy change, or enthalpy change, within a system is represented by the amount of heat released. The enthalpy change is calculated by finding the temperature change within the single displacement reaction. The enthalpy change can be calculated through the following reaction: ΔH = mcΔT in Joules In which ΔH represents the enthalpy change, m represents the mass of the solution, c represents the specific heat capacity of the solution, (it is accepted as water = 4.18Jg-1K-1) and ΔT is the temperature change of the reaction.
The higher the temperature change is, the higher the enthalpy change will be and vice versa.
In this experiment a variety of single displacement reactions with copper sulfate and various metals of differing reactivity were conducted to investigate how the reactivity of different metals affect the enthalpy change. The single displacement reactions that were conducted with copper sulfate and various metals are listed below by decreasing reactivity:
Hypothesis:
When the reactivity of a metal increases, they react more vigorously and thus more heat is released during a reaction. Therefore, the enthalpy change value will be greatest during the reaction between copper sulfate and magnesium since it is the one with the greatest reactivity between the other four metals. Thus it is hypothesized that as the reactivity of different metals begins to increase the absolute value of enthalpy change is expected to increase as
well.
The purpose of this lab is to determine the empirical formula of copper oxide (CuxOy) through a single-displacement reaction that extracts the copper (Cu) from the original compound. In order to do this, hydrochloric acid (HCl) was mixed in with solid CuxOy; the mixture was stirred until the CuxOy was totally dissolved in the solvent. Zinc (Zn) was then added to the solution as a way to enact a single displacement reaction in which Cu begin to form on the Zn; the Cu gets knocked off the Zn through gentle stirring. To isolate the Cu, the supernatant liquid was decanted and the Cu was then washed with first water then second, isopropyl alcohol. Once done, the hydrated Cu is transferred onto an evaporating dish where it was heated multiple times
= I plan to investigate the effect of temperature, to see if it. increases or decreases the rate of reaction between magnesium and hydrochloric acid. Prediction: -. =
In this lab, I determined the amount of heat exchanged in four different chemical reactions only using two different compounds and water. The two compounds used were Magnesium Hydroxide and Citric Acid. Both compounds were in there solid states in powder form. Magnesium Hydroxide was mixed with water and the change in heat was measured using a thermometer. The next reaction combined citric acid and magnesium hydroxide in water. The change in heat was measured as well. For the third reaction citric acid was placed in water to measure the change in heat. In the last reaction, citric acid was combined with water. The heat exchanged was again measured. It is obvious we were studying the calorimetry of each reaction. We used a calorimeter
If heat is applied to Copper (Ⅱ) sulfate pentahydrate, then the experimental form will be equivalent to the theoretical formula. Important key data that will be needed to achieve the goal of the lab experiments includes the initial mass of hydrated crystal, the final mass of anhydrous crystal, the
The Enthalpy Values for the Reaction Between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride
To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
" This means that therefore the enthalpy change of a reaction can be measured by the calculation of 2 other reactions which relate directly to the reactants used in the first reaction and provided the same reaction conditions are used, the results will not be affected. We have the problem set by the experiment to determine the enthalpy change of the thermal decomposition of calcium carbonate. This is difficult because we cannot accurately measure how much thermal energy is taken from the surroundings and provided via thermal energy from a Bunsen flame into the reactants, due to its endothermic nature. Therefore, using the enthalpy changes obtained in reaction 1 and reaction 2 we can set up a Hess cycle.
Simple procedure steps were followed for each lab section, using flames and different types of chemicals. The water jug explosion, the cutting torch and the magnesium strip all resulted in a chemical change because the physical properties changed from one to another. It was concluded the copper wire experiment was a physical change because the only difference that occurred was an alteration in color. After observing each change, it was determined if the change was physical or chemical and specific data was used to support each
Enthalpy of solution is heat change when one mole of salt is dissolved in excess of solvent so that all heat change takes place in one time.
In this experiment, the water of crystallization is removed from hydrated copper(II) sulfate. The mass of water is found by weighing before and after heating. This information is used to find x in the formula: CuSO4.xH2O. Note that x must be an integer (a whole number).
• Investigate the effect of temperature on the rate and use the results to find the activation enthalpy for this particular reaction.
Investigating the Effects of Temperature on the Rate of Reaction between Magnesium and Hydrochloric Acid Introduction Chemical kinetics is the study and examination of chemical reactions regarding re-arrangement of atoms, reaction rates, effect of various variables, and more. Chemical reaction rates, are the rates of change in amounts or concentrations of either products or reactants. Concentration of solutions, surface area, catalysts, temperature and the nature of reactants are all factors that can influence the rate of reaction. Increasing the concentration of a solution allows the rate of reaction to increase because highly concentrated solutions have more molecules and as a result the molecules collide faster. Surface area also affects reaction rate because when the surface area of a reactant is increased, more particles are exposed to the other reactant.
Instructional Purpose - “I Wonder.” Statements - Guided Reading Instructional Purpose: Students need to understand the importance of thermochemistry. Thermochemistry revolves around the energy (heat) associated with reactions and other materials. This field of chemistry has a variety of terms and applications that need to be understood before heading into college-level chemistry courses. Terms such as temperature, specific heat, calorimeter, and enthalpy are commonly used within lab experiments.
Enthalpy is defined as the change in heat, or ΔH. The change in heat of a specific reaction is symbolized by ΔH°rxn. The heat of a reaction is measured by the enthalpy of the product minus the enthalpy of the reactants. This heat of reaction, ΔH°rxn, is important for many reasons, including its use in metabolism, fuel combustion, food, everyday items like refrigerators and hand warmers, and other chemical processes.