Copper Sulfate Reaction Lab Report
comparative Essay
450 words
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…
In this essay, the author
- Explains the aim of this investigation was to determine how five different metals of different reactivity reacting with copper sulfate solution would affect the enthalpy change of the reaction.
- Hypothesizes that as the reactivity of different metals increases, the absolute value of enthalpy change is expected to increase as well.
- Explains that the idea for this investigation was developed from an in-class experiment done during our energetics unit where we learned about enthalpy changes within a reaction by conducting an experiment between copper sulfate solution and zinc.
- Describes the enthalpy change in a single displacement exothermic reaction, which is calculated by finding the temperature change within 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
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- To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powdercomparative essayTo investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
In this essay, the author
- Explains that they will mix magnesium ribbon and copper sulphate solution into polystyrene cups until they find a reaction.
- Predicts that magnesium will displace the copper and the temperature will rise because it is more reactive and it's an exothermic reaction.
- Explains that the preliminary experiment was useful because it was clear that there was a very small rise in temperature, which can be solved by using the powdered form of metal.
- Predicts that the reaction of the zinc and copper sulphate will be exothermic, therefore it will produce its own heat.
- Predicts that the temperature will increase when adding more zinc until a certain mass of zinc is reached.
- Explains that copper sulphate solution will only partially be heated because there is not enough zinc to react with all of the copper depending on the mass of zinc. the zinc powder will release more heat than zinc ribbon due to thepowder having a larger surface area.
- Explains that the peak temperature is when there is enough zinc to react with the copper sulphate. any less zinc and it would not react as much producing less heat.
- Explains that a set amount of zinc powder will be added to the solution then mixed. the ‘peak’ temperature of the mixed solution will then be taken.
- Explains that their prediction and hypothesis were correct. the experiment was a success and had no anomalies.
- Explains that the reaction was exothermic because heat was produced without a main source (bunsen burner).
- Concludes that they did not do many tests, although more tests would make their conclusion more accurate.
- Opines that the experiment was a fair test. all the apparatus was cleanedefficiently before use, but it could have been fairer.
- Explains that the starting temperature of the copper sulphate solution was slightly different because the experiment took place over several days.
- Explains that they did not do this test with each mass when the coppersulphate solution was at the same starting temperature. the experiment could have been held in an area that had a lower or higher roomtemperature so evidence could be gathered.
- Explains that the experiment was straightforward from beginning to end, requiring a high voltage lamp, torch, or bunsenburner.
1074 wordsRead More - Hydrated Copper II Sulfate Labexplanatory essayTo find the formula of hydrated copper(II) sulfate Introduction 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). Diagram Method Safety: Wear eye protection Find the mass of your crucible.
In this essay, the author
- Explains how the water of crystallization is removed from hydrated copper(ii) sulfate. the mass of water is found by weighing before and after heating.
- Explains how to heat crystals until they have gone completely white, but not so strongly that they start to blacken.
- Explains that the reaction is reversible. what do you expect if you add a few drops of water to the white copper(ii) sulfate?
- Opines that a processed data section should include explanations of your calculations towards calculating the value of x.
- Describes the observations of compound (hydrated cuso4) before, during and after the substance has been heated.
- Explains the process of finding the mr, moles and empirical formula from the compounds anhydrous cuso4 and h2o.
- Explains that 160 is the molecular mass of cuso4, this is done by adding up each ar of each element in the compound.
- Explains that 18 is the molecular mass of h2o, done by adding up each ar of each element in the compound.
- Explains that the number of moles of anhydrated cuso4 is found by dividing the mass in grams by the mr.
- Explains that the number of moles of h2o is found by dividing the mass in grams by the mr.
- Explains that to find the mole ratio of anhydrated cuso4, divide the number of moles (0.008625) by the smallest number.
- Explains how to find the mole ratio of h2o by multiplying the number of moles by the smallest number.
- Explains how to write an equation and a balanced chemical equation for the reaction that has occurred.
- Explains that hydrous cuso4 after heating turns into a white opaque solid crystal, which is also odorless.
- Explains how the formula of hydrous copper(ii) sulfate requires one molecule of cuso4 and four molecules of h2o.
1159 wordsRead More - Use of Enthalpy Changes of Metal Reactionsexplanatory essaybe yes as I will then be able to use enthalpy change of reaction to
In this essay, the author
- Explains the use of enthalpy changes of metal reactions to experimentally test the reactivity series of common metals.
- Argues that enthalpy changes of reaction can predict the place of a metal in the metals reactivity series.
- Explains that if the hypothesis is proved correct through experimentation then they can apply it to predict the place of metals they have investigated in the reactivity series.
- Explains that arranging the metals investigated in order of decreasing enthalpy change of reaction and comparing this list with published and accepted data will prove the hypothesis is correct.
- Explains that the enthalpy change of a reaction is the heat evolved when the reaction takes place. all chemical bonds hold heat energy within them.
- Explains that an exothermic reaction would be considered to have a negative enthalpy change because heat energy has been given up into the surroundings.
- Explains their hypothesis based on the understanding that more reactive metals will create more stable compounds on reaction, meaning less energy will be held in their strong and stable bonds.
- Explains that the reaction between lithium metal and copper sulphate is simple and safe, and should be spontaneous with a good number of common metals.
- Explains how they calculate the enthalpy change of the reaction using î” h = m c ( tinitial – tfinal).
- Explains that the independent variable is the choice of metal in the experiment, which changes from experiment to experiment. the dependant variable changes because of the changing metal.
- Explains that uncontrolled variables are aspects over which they have no effective control, such as the ambient temperature in the cup which may change with external temperatures. the surface area of the metal affects the rate of reaction.
- Explains that the faster the reaction, the harder it will be to measure the enthalpy change. metal filings can mitigate this by using the thermometer.
- Explains that the reaction will be conducted in the insulated styrofoam cup to minimise the heat loss to the surroundings.
- Explains how the temperature of the reaction is measured in situ by measuring 25cm3 of copper sulphate into a cup and adding 0.5 g (an excess) of metal to the stopwatch.
- Explains that leaving the cup is responsible for the fall in temperature after this point. it is important to take further readings after the peak temperature has passed.
- Explains that heat loss error will mean that the temperature measured will not take account of all the heat generated by the reaction.
- Explains that they have chosen five metals with which to conduct the reaction. they expect them to react with copper ions on the basis of their standard electrode potentials and cover a reasonable range of the reactivity series.
982 wordsRead More - ulhiiexplanatory essayThe purpose of this experiment was to use measurements of change in heat and Hess’s law to compare reactions. In this lab we used the formula q=(cp)(m)(∆T). Where cp or Specific heat is the heat capacity of 1 gram of a substance in units J / (g x K). The reactions were all exothermic meaning energy was released from the system. This is the opposite of endothermic which means energy is absorbed by a system. After we had recorded the initial and final temperatures from the experiment we subtracted the final temperature from the initial temperature to find the change in temperature or (∆T). After we had obtained the change in temperature we took this number and plugged it into the formula q=(cp)(m)(∆T). This gave us the heat of the reaction, which we took and divided by the amount of mole concentration. That is how we calculated the change of heat for reaction #1. We used the same process for reactions #2 and #3, except we used the numbers we had recorded for those reactions. We then took the the change in heat from reaction #1-3 and placed them in order to find our actual heat. We then modified the setup to find the theoretical yield and compared our answers. This also proved our hypothesis because the values of the change in heat from reaction #1 and #2 should have been equal to the value of the change in heat form reaction #3. Reaction #1 and #2 were sub reactions, to reaction #3. Meaning that reaction #3 was a reaction that consisted of all the parts reaction #1 and #2 had combined. This agrees with the rules of Hess’s law which states: if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the individual steps. For reaction #1 the data we recorded is as follow...
In this essay, the author
- Explains how the experiment used heat measurements and hess's law to compare reactions.
- Explains that reaction #3 was a reaction that consisted of all the parts reaction #1 and #2 had combined.
- Opines that the equipment they used was not top-of-the-line, but their measurements could have been more accurate with a little more care.
- Explains that adding parts of heat to come up with the total is more important than it may seem. small errors can lead to disasters. hess's law is important and a big contribution to society.
674 wordsRead More - The Importance Of Enthalpy In Chemistryexplanatory essayEnthalpy 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.
In this essay, the author
- Explains that enthalpy is defined as the change in heat, or h°rxn. the heat of a reaction is measured by the product minus the reactants.
- Explains h°rxn's role in metabolism. metabolism is a set of reactions that create important energy sources for every living thing.
- Explains the importance of the h°rxn in the use of fuels. it allows people to measure just how much energy a reaction is going to produce.
- Explains that h°rxn is the main reason that some foods give people more energy than others.
- Explains how refrigerators work by vaporizing a refrigerant to cool food. the h°rxn of this process is equivalent to how cold the fridge gets.
- Explains how h°rxn is used in hand warmers. it is a chemical reaction in which iron, water, salt, and carbon react to produce heat.
- Explains how the h°rxn can be used to find other chemical variables, such as the equilibrium constant of a reaction.
- Explains that h°rxn is important for metabolism and the creation of energy. it provides useful information about various common fuels and what to use them for.
1232 wordsRead More - Enthalpy Essayexplanatory essayWhen 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.
In this essay, the author
- Defines enthalpy as the amount of heat content used or released in a system at persistent pressure.
- Explains that when the reaction is giving off heat, it is exothermic, and the enthalpy change is negative. if energy flows from the surrounding environment and heat is being taken in, the change in energy is positive.
- Explains that bond enthalpy is the energy required to break a chemical bond. it is expressed in units of kj mol-1, measured at 298 k.
- Explains that bond making is an exothermic process. however, if a certain bond is broken and then reformed, then the same amount of energy must be involved.
- Explains that 2 o-h bonds are formed per water molecule, and there are 2 water molecules formed, therefore 4
- Explains that combustion is the process in which fuel is burnt in exchange for energy. there are two forms of combustion, "complete" and "incomplete".
- Explains that stand and boss are connected to the clamp. boss is used to secure the can in place and for safety.
- Recommends clamping the metal can (or flask) at a suitable height to allow room for the spirit burner to be placed below.
- Opines that there were factors in this practical that could have led to better results. loads of errors had occurred with the practical and means of improvement made the experiment better.
- Explains that thin layer chromotography is carried out by packing the same materials into a verticle glass column.
- Explains separations in tlc involve distributing a mixture of two or more substances between the stationary phase and the mobile phase.
- Explains that gas chromatography is a dominant tool in analysis. it contains different variations in the way it is done.
- Explains that gas chromatography has limited uses due to the decomposition temperature of the mixture and the composition of a column. most columns cannot withstand temperatures greater than 250-350 °c.
- Explains how the pen reacts with the solvent and separates the substances in the ink.
- Explains how it helps draw out straight lines (1cm from the top) and makes it more accurate.
- Explains how the thin layer chromatography strip is used to extract the green liquid and place small drops.
- Explains the use of thin layer chromatography to dry the liquid faster.
- Explains that the second solvent is used as the mobile phase to travel up the thin layer chromatography strip and separate out the substances.
- Explains that the glass beaker is used to contain the second solvent, and it is where the thin layer chromatography is held.
- Explains how to cut strips of thin layer of the chromatography plate to fit into tubes provided.
- Explains how they crush the contents together using the mortar until plenty of green fluid is made.
- Explains how to draw a line using sharp pencils, not pen, approximately 1cm above the bottom of the chromatography paper.
- Explains how to collect the green fluid and dab it on the thin layer chromatography strip in the middle of the pencil line drawn.
- Recommends using a hair dryer to dry the thin layer chromatography strip so the green fluid is not wet anymore.
- Explains how to add a few drops of solvent to the glass beaker once it is dry.
- Explains how to put the thin layer chromatography strip into the beaker filled with solvent and make sure that it is held up right.
- Explains that if the sample is solid, it is weighed using an accurate balance, and then dissolved to make up a known volume of solution.
- Explains how a safety pipette filler is used to draw the solution into it, which is then emptied into the conical flask.
- Explains that a few drops of an indicator may be added to the conical flask, which will show titration results.
- Explains that the second chemical is placed in a burette, which reacts with the synthesised chemical sample in the conical flask.
- Explains how the solution from the burette is run into the conical flask. the solution is added one drop at a time, with swirling to mix the solutions as the end-point is approached.
- Explains that a standard solution is an accurately known concentration prepared from the primary standard, which is stable, of high purity, highly soluble in water, and of molar mass to allow accurate weighing.
- Explains that the solution is in a virtually pure form and so there is no requirement to find out the concentration.
- Explains that a primary standard solution can be valued to high level of accuracy and reliability.
- Explains the difference between a primary standard solution, and one that is stable enough for titrimetric work.
- Explains that as the atomic mass is known, the volume of the solution can be calculated using this formula.
- Explains that if a solution was to be made of (nacl) with 6mol dm-3 and the volume is 50cm3, then:
- Recommends weighing sodium carbonate and placing it in a small beaker.
- Explains that colorimetry is the scientific method used to classify the colours of the spectrum.
- Explains that colorimetry is used in chemistry for things such as colour painting, food manufacturing, and textiles. the amount of light absorbed is measured as the absorbance.
- Explains how to weigh the spirit burner, remove the cap, light the wick, and allow the alcohol to heat the water.
- Explains how to record the final temperature of the water using the thermometer and work out the temperature change.
- Recommends that the experiment be carried out in a temperature-controlled area, as the atmosphere affects the practical. elimination of the flame as soon as possible is important. alcohol and water spillage should be avoided.
- Recommends repeating the experiment as many times as possible. 90% of the heat released from the spirit burner didn't grasp the metal can.
- Explains that thin layer chromatography provides a speedy answer to how many components are in the mixture.
- Explains that chromatography is used to separate mixtures of substances into their components.
- Explains that paper is replaced by a thin layer of powder, such as silica, on glass or plastic backing. it is used to determine amino acids in blood samples and in analysis of food dyes.
- Explains how a thin layer chromatography plate (cut into strips) is used to make markings on the strip. the pen reacts with the solvent and separates the substances in the ink.
- Explains how to draw around each colour spot, that has appeared, and label/ not down the colour of each spot.
- Explains the importance of a high level of purity in synthesised chemical compounds, such as pharmaceuticals. a titration measures the volume of one solution that reacts with another solution.
- Explains how titration results can be used to calculate the amount of the synthesised chemical in the sample, and therefore find its purity.
- Explains that they are using the standard solution for titration, because the term ‘standard solution’ is a scientific phrase.
- Explains that nacl must be used to make a solution of 50cm3 standard solution.
3212 wordsRead More - The Enthalpy Values for the Reaction Between Calcium Carbonate and Calcium Oxide with Hydrogen Chlorideexplanatory essayThe Enthalpy Values for the Reaction Between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride
In this essay, the author
- Describes the enthalpy values for the reaction between calcium carbonate and calcium oxide with hydrogen chloride.
- Describes the variables of temperature mass of cao + weighing bottle.
- Explains the calculations for the reaction between caco3 + hcl — heat capacity, temperature change, volume, mass of reactant moles, ar, and ca.
- Explains that they are using hess' law to calculate a value for the enthalpy change of the reaction.
- Explains the indirect method, wherein the h2 must be reversed so the result is changed to a positive number.
- Opines that when measuring exothermic reactions, it is important to ensure that the calcium oxide and calcium carbonate are in lumps.
- Explains that when the reaction takes place, as little heat is lost to the environment as possible. the glass beakers provided for the first attempt were not very efficient at retaining the heat.
- Explains that the polystyrene beaker did not have a lid. the use of the thermometers gave inaccurate results as the highest temperature recorded was 27 c.
- Opines that a digital thermometer would show much more accurate temperature changes.
587 wordsRead More - Investigation into the kinetics of the reaction between peroxodisulphate(VI) ions and iodide ionsanalytical essay• Investigate the effect of temperature on the rate and use the results to find the activation enthalpy for this particular reaction.
In this essay, the author
- Explains that they were interested in using this reaction to support and quantify some of the theories they have studied along with perhaps extending on them.
- Explains that the initial rate of the reaction can be measured by measuring the time it takes to produce a fixed small amount of iodine.
- Analyzes the effect of concentration and temperature on the rate and the activation enthalpy for this particular reaction.
- Describes the 'iodine clock reaction', where the time taken to form a definite, small amount is recorded to work out the rate.
- Explains how the rate of iodine produced in a reaction can be calculated by adding thiosulphate to the reaction mixture. the rate can also be controlled using the clock method.
- Explains that they will study a suitable percentage of reaction in their method to ensure that the rate is constant, while progressively lower percentages mean using smaller concentrations which lead to larger uncertainties.
955 wordsRead More - Chemical Reactions In Sports Essayexplanatory essayDuring an intense game, athletes need a way to soothe their acute injuries leading them to the instant cold packs in their team’s med kit as fans huddle under blankets clutching hot packs between frigid fingers. What these two groups don’t realize is that they are utilizing chemical reactions in order to either expel or absorb heat. Chemical reactions that were discovered and utilized by inventors to create the very packs they are using. The chemicals inside each respective pack have various properties and applications that make them useful in their thermochemistry reactions. The compounds used are salts including sodium acetate and calcium chloride for hot packs and ammonium nitrate for cold packs.
In this essay, the author
- Explains that athletes need a way to soothe their acute injuries leading them to instant cold packs in their team’s med kit as fans huddle under blankets clutching hot packs between frigid fingers.
- Explains that the compounds used for hot and cold packs have numerous properties, including sodium acetate, calcium chloride, and ammonium nitrate.
- Explains that both the hot and cold packs were invented in the 20th century. the first instant cold pack was patented in 1959 by albert a. robbins to keep foods and beverages refrigerated.
552 wordsRead More - Thermochemistry Essayexplanatory essayHave any of you wondered about the magic that occurs within a hot hand? The hot hand is a small pouch that contains mysterious elements that combines to start a reaction that produces heat. There is a specific field of chemistry that studies the heat associated with reactions, and today we begin our journey learning about this form of chemistry called thermochemistry! Thermochemistry is a fascinating field of chemistry that contains new terms and ideas that need to be understood in order to proceed into the mathematical applications of thermochemistry. We are going to create “I wonder…” statements to help with learning about these new terms while we read the
In this essay, the author
- Explains that students need to understand the importance of thermochemistry. thermochemistry revolves around the energy (heat) associated with reactions and other materials.
- Explains that the introduction of the term specific heat can be difficult to understand because the temperature scales of kelvin and celsius are interchangeable.
- Explains that enthalpy is difficult to understand for the beginning chemist because it cannot be measured within a reaction system, so they must focus on its change.
- Explains that they will model how to think when reading this section of the test. their metacognitive process will be witnessed as they come up with "i wonder..." statements that will benefit them the most.
- Explains that students will analyze the text and create statements that will be used for reading the upcoming sections of text in more detail.
- Explains that the students' thinking will be contained and retained by the statements they have created. the hot hand contains mysterious elements that combines to start a reaction that produces heat.
- Explains that the "i wonder..." activity revolves around reading an introduction to a section of text and determining statements that strike curiosity within the brain.
- Explains how they created an "i wonder..." statement based on a section of the text about heat and temperature.
- Asks students to create an "i wonder..." statement after reading the section titled "energy transferred varies from reaction to reaction."
- Explains that the purpose of the statements is to provide motivation for reading each upcoming section of text and to learn something new within each new section.
1328 wordsRead More