The balanced equation shows that two moles of silver nitrate react with one mole of copper
Copper and Silver Reaction Chemistry Internal Assessment Raw data table: What I measured Value (unit) Uncertainty Weight of Beaker 103.335(g) ±0.001g Volume of Silver nitrate 100(cm3) ±1 cm3 Concentration of Silver Nitrate 0.1(mol dm-3) Initial weight of Copper wire 2.020(g) ±0.001g Final weight of copper wire 1.688 ±0.001g Final weight of silver crystals and beaker 105.139 ±0.001g Qualitative Observations: * The copper was a orange/red colour before being submerged. * While the silver nitrate AgNO3 was a clear colourless liquid. * Immediately after the copper was submerged it turned black. * The copper wire was resting on the bottom of the beaker. * After prolonged submersion the wire became thicker as more precipitate was formed on the wire. * After prolonged submersion the solution became a clear light blue solution. * After 24 hours a silver/grey crystalline structure formed around the wire and on the bottom of the beaker. Processed data table: What I measured Value (unit) 3sf Uncertainty Mass of reacted Cu 0.332(g) ±0.002g Number of reacted Cu 0.00522 mol % uncertainty = ±0.605 Mass of reacted Ag 1.804(g) ±0.002g Number of reacted Ag 0. 0167 mol % uncertainty = ±0.166 Constants table: Constant Value Mr(Cu) 63.55 gmol-1 Mr (Ag) 107.87 gmol-1 Calculations Balanced chemical equation between copper and
Enthalpy of Neutralisation Between HCl and NaOH
Year 12 Chemistry Enthalpy of Neutralisation Internal Assessment Raw Data Table: What I measured Value (unit) Uncertainty Volume of HCl 20cm3 ±1 cm3 Volume of NaOH 20cm3 ±1 cm3 Concentration of HCl 1.00 mol dm-3 Concentration of NaOH 1.00 mol dm-3 Initial Temperature of HCl 21.3 ˚C ±0.005 ˚C Initial Temperature of NaOH 21.3 ˚C ±0.005 ˚C Table displaying the relationship between temperature and time after 20cm3 of an HCl solution is combined with 20cm3 of a NaOH solution Time (seconds) Temperature (˚C) 1 21.3 2 21.3 3 22.1 4 24.1 5 25.5 6 26.3 7 26.7 8 26.9 9 27.1 10 27.1 11 27.2 12 27.3 13 27.4 14 27.5 15 27.5 16 27.5 17 27.4 18 27.4 19 27.3 20 27.3 Qualitative: * The temperature probe often touched the bottom of the cup. * Not all the liquid was poured out of the measuring cylinder * The measuring cylinder had to been rinsed before each measurement meaning it may have been contaminated. * The two reactants are both clear liquids and when mixed, the result is also a clear liquid. There is no colour change seen in the experiment * The container of the neutralizing NaOH and HCl rose slightly in temperature, and at the end of the experiment felt slightly warmer than before the experiment * When stirring, the stirring rod sometimes knocked against the temperature probe * Small bubbles could be seen
Chemistry Internal Assessment Hesss Law
Chemistry Internal Assessment DCP and CE “Hess’s Law” 2014 Raw data table: Observations: * The solution with MgSO4 a white precipitate formed * In the experiment using MgSO4 the thermos got warm * The solution with MgSO4.7H2O turned a cloudy white * In the experiment using MgSO4.7H2O the thermos got cooler Measurement Mass (g) ±0.001 Volume –measuring cylinder (mL) ±1 Mass of MgSO4 3.801 Mass of MgSO4.7H2O 7.958 Volume of H2O 50 Full Equations of Reactions ) MgSO4(s) → Mg2+(aq) + SO42-(aq) 2) MgSO4.7H2O(s) → Mg2+(aq) + SO42-(aq) + 7H2O(l) Literature Values Constant Value Source Specific Heat Capacity of Water 4.18 J g-1K-1 http://www.sphsgator.net/sphsteachers/domanskil1/databooknew.pdf A Raw Data Table Showing the Relationship between Time Elapsed and the Temperature of the Reaction of Hydrous and Anhydrous Magnesium Sulphate using a logger pro temperature sensor. Time (seconds) ± 0.1 seconds Anhydrous MgSO4 Temperature (°C) ±0.1°C Hydrated MgSO4 Temperature (°C) ±0.1°C 0 20.7 17.3 10 20.7 17.3 20 21.8 16.8 30 23.3 15.9 40 24.4 15.7 50 25.3 15.6 60 26.1 15.6 70 26.6 15.7 80 27.1 15.7 90 27.4 15.7 100 27.7 15.8 120 28.0 15.8 130 28.0 15.9 140 28.1 15.9 150
Reaction Rate
Science Reaction Rate Between an Acid and Metal Investigation PROBLEM/RESEARCH QUESTION In this investigation, a controlled experiment will be conducted to determine whether the varying concentration of an acid alters its reaction rate with a metal substance and if so, what is the resultant relationship between the rate of reaction and the concentration of the acid. In particular, we will be reacting Sulfuric acid (H2SO4) with Magnesium metal (Mg) and collect data based on the resultant hydrogen gas produced by the reaction. Word Equation: Magnesium + Sulfuric Acid → Hydrogen gas + Magnesium Sulfate Balanced Equation: Mg (S) + H2SO4 (aq) → MgSo4 (aq) + H2 (g) Research will be formulated by conducting a controlled experiment in which we will react 0.05g of Magnesium metal ribbons (Mg) with 10mL of four different H2SO4 (Sulfuric Acid) solutions varying in concentration and determine the time it takes for the reaction to produce 20mL of Hydrogen gas with each varying concentration. HYPOTHESIS I hypothesise that as the concentration of the H2SO4 solution increases/strengthens (measured in molarity mass), it will correspond to an increased/quicker rate of reaction with Mg metal. Hence, I also hypothesise that - based on the above premise- the 2M solution of H2SO4 would be the quickest to produce 20mL of H2 gas when reacted with magnesium, as it is the strongest of
To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.
Candidate Name: Candidate Number: Page | International Baccalaureate Diploma Program (IBDP) Session: May 2015 Chemistry HL Lab Report Lab Report Title: To determine the standard enthalpy of formation of Magnesium Oxide using Hess’ Law. Criteria Assessed: * Data Collection and Processing (DCP) * Conclusion and Evaluation (CE) Candidate Name: Candidate Number: International School, Singapore AIM: To determine the standard enthalpy of formation of Magnesium Oxide using Hess’s law. INTRODUCTION: The objective of this experiment was to determine the change in enthalpy when one mole of Magnesium (Mg) reacts with half a mole of Oxygen (O2) to give one mole of Magnesium Oxide (MgO). The balanced chemical equation is as follows: Mg (s) + O2 (g) → MgO (s) ---- ΔHMgO f The reaction between Magnesium and Oxygen to form Magnesium Oxide is essentially the combustion of Magnesium and since every combustion reaction is an exothermic reaction, this reaction too is an exothermic reaction, i.e. it too will produce heat to the surroundings. In fact, the combustion of Magnesium is highly exothermic as it produces flames whose temperatures reach almost 2500oC (http://physics.stackexchange.com). At such high temperatures, a very bright white light is produced and if directly looked upon for long
Biodiesel Investigation - How the concentration of Potassium Hydroxide solution would affect the yield of biodiesel when transesterified with a standard sample of vegetable oil .
1th May 2015 Biodiesel Experiment Introduction ‘Biodiesel is a clean burning renewable fuel made using natural vegetable oils and fats.1 Biodiesel is a revelation to chemists, engineers and environmentalists who are looking for more sustainable ways to make use of fuels. Since it is a natural and renewable fuel, it can be fitted in as a substitute for petroleum diesel, which is the substance conventionally used in automobile transport. Biodiesel is normally utilised as a replacement for petroleum diesel fuel or can be blended together with petroleum diesel fuel in any ratio. Biodiesel is a biodegradable substance with a lower toxicity in comparison to petroleum diesel fuel and is preferred as it is safer to handle since there is little human risk involved in its handling. The use of biodiesel as a petroleum substitute reduces the degree of exhaust emission. Biodiesel are notorious for their easy use in terms of how they can easily be pumped and stored in existing engines without having to make major industrial alterations to the engines themselves. They are usually blended together with petroleum fuels in order to create the optimal usage in engines. The output yield of biodiesel is I had never really heard of biodiesel until it was a topic covered in school. After finding out what biodiesel was, I looked into the IB chemistry syllabus to see what points it had on
synthesis of aspirin
Synthesis of Aspirin Anabel Castro Chemistry III IB Planning A Research question: Which is more pure, salicylic acid, commerical aspirin, or home-made aspirin when tested with Ferric Chloride solution? Hypothesis: If the three substances are tested for purification by the addition of Ferric Chloride solution, then the purest substance will be salicylic acid then the home-made aspirin because Ferric chloride solution produces characteristic color changes when it reacts with certain organic compounds. In addition, the test tube containing the purest substance will have the smallest color change. Variables(Independant): The substances mixed with Ferric Chloride solution. (Dependant): Pureness (Controlled): amount of ferric chloride solution, amount of distilled water, clean test tubes. Planning B Chemicals: * Acetic anhydride * Salicylic acid * 85% phosphoric acid Materials: * 125 mL Erlenmeyer flask * 5 mL or 10 mL graduated cylinder * 600 mL beaker * 400 mL beaker * thermometer * burner * suction flask * buchner funnel * vertical upright * extension clamp with clamp holder * top loading balance * test tube with cork * split cork to hold thermometer Method: * Warning: Be careful when using Acetic Anhydride and Phosphoric Acid. Both chemicals can cause serious burns. Use gloves when handling and use in hood. * Using a top loading balance to
Reaction Rate Investigation
Reaction Rate Investigation- Introduction- Background Information- • The reaction rate is the rate of which the reactant reacts with the reactor. • We will measure the rate of reaction by measuring the volume of gas let off by the reaction. • In order to find the average rate I will use the equation below. Aim- The aim of this investigation is to find how the surface area effects the reaction rate in the reaction between calcium chloride and hydrochloric acid. Hypothesis- I think that with a greater surface area(smaller particles) the acid will react quicker. I think this because of the collision theory. In the collision theory it states that in order for two substances to react together they must collide with each other and they must have enough energy. Procedure- Variables- Independent Dependent Control The concentration of the acid Rate of reaction (volume of gas) Volume of HCL (1 mol l-1) Temp. (room temp) Mass of Calcium Carbonate(2.5g) Volume of Dilute HCL (50 cm3) Time (40 seconds) Agitation (none) Diagram- Materials- • 25 ml graduated cylinder • 100 ml graduated cylinder • Stopwatch • Stopper • Plastic tube • Side- arm test tube • Calcium carbonate with large(powder), medium(small chips) and small(large chips) surface areas • 1 mol l-1 of hydrochloric acid Method- . Set up the apparatus as shown in the
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
enthalpy change
Investigation 19 MEASURING ENTHALPY CHANGES Method: Part A ) Put 100 cm3 of water at about 60 ºC into a polystyrene cup by mixing boiling water from the kettle with cold water from the tap. 2) Dry about 25 g of ice with a piece of paper towel and weight them both. 3) Rapidly record the temperature of the water and transfer the ice to it, then record the mass of the paper towel and the water it has absorbed. 4) Stir the water ice mixture and record the temperature of the water as soon as all the ice has just melted. Part B ) Take the polystyrene cup and use measuring cylinder to put 50 cm3 of 1 M aqueous copper sulphate in it. 2) Weigh out accurately about 5 g of powdered zinc into a weighing bottle. 3) Stir and record the temperature of the copper sulphate at half minute intervals for 2 minutes and then add the powdered zinc. 4) Record the temperature at half minute intervals until the temperature has been falling for ten consecutive recordings. Part A: the heat required for a change of state Firstly, I needed to boil the water in the kettle, so that it can be used in the experiment. Also I weighted the ice I was going to put in the water. m= mass of ice- mass of ice in the paper= 25g - 7.1 g = 17.9 g of ice mole - 18g X - 17.9g X= 0.99 moles Than, I started the experiment. Table1: The measurements of the temperature change for the first reaction.