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…
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
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
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
= 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: -. =
The Enthalpy Values for the Reaction Between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride
An endothermic reaction is a chemical reaction that absorbs heat into its environment. The energy is usually transferred as heat energy, causing its surroundings to get colder. The opposite to an endothermic reaction is an exothermic reaction. An exothermic reaction releases cold energy which absorbs heat energy. As a result of this, the surroundings distinctively become hotter. In this experiment an exothermic reaction takes place.
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.
• Investigate the effect of temperature on the rate and use the results to find the activation enthalpy for this particular reaction.
Have you ever been sitting there and just wondered about various things dealing with some things in chemistry known as calorimetry or thermochemistry? No, yes, maybe, well whatever your answer you were really thinking yes so I’m going to explain these topics to you in this paper, and teach you how they work so you can figure these things out if you ever run into them I a real life situation.
When the reaction is giving off heat, it is exothermic. In this case, the enthalpy change is negative, since the reaction is going from high energy to low energy due to the loss of heat energy to its surroundings. If energy flows from the surrounding environment and heat is being taken in, it is endothermic. The change is positive as the system is gaining energy in the form of heat.
To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
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.
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).
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.