Chemical reactions p pt
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This experiment investigated how the concentration of hydrochloric acid affects the reaction time of magnesium ribbon. Five concentrations of HCl from 100% to 20% were tested, and the time taken for the magnesium ribbon to completely disappear was recorded. The results showed that higher concentrations of HCl led to faster reaction times, supporting the particle collision theory that higher concentrations provide more opportunities for effective particle collisions between HCl and magnesium.
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Rate of reaction temperature
This document outlines an experiment to determine how temperature affects the rate of reaction between sodium thiosulfate and hydrochloric acid. It describes the independent variable as the temperature of the hydrochloric acid ranging from 0°C to 80°C. The dependent variable is the time for a cross drawn on paper to become invisible when placed behind a test tube containing the reaction. The method involves timing how long it takes for the cross to disappear at each temperature, with results recorded in a table. The conclusion states that higher temperatures led to faster reaction times, supporting the particle collision theory that increasing temperature causes particles to move faster and collide more frequently.
Elly lee effect of temperature on reaction rate
Elly Lee conducted an experiment to observe the effect of temperature on reaction rates. Zinc was reacted with HCl at different temperatures and the reaction times were recorded. The results showed that reaction times decreased as temperature increased, with the fastest reaction occurring at 49.9°C and the slowest at 6.1°C. The type of gas produced also changed with temperature. This supports the hypothesis that increasing temperature increases reaction rates.
Effect Temperature Reaction rate
This document describes an experiment to observe the effect of temperature changes on reaction rate. The experiment involves a reaction between potassium permanganate, sulfuric acid, and oxalic acid. The reaction rate is determined by measuring the time it takes for the purple permanganate solution to become colorless. Results show that as temperature increases from 40°C to 70°C, the reaction time decreases and the reaction rate increases. The conclusion is that higher temperatures lead to faster reaction rates.
Temperature reaction rate
This document summarizes an experiment that investigates the effect of temperature on reaction rate. The experiment uses the reaction between potassium permanganate and oxalic acid, where the disappearance of the purple permanganate color indicates the extent of reaction. The experiment is conducted at different temperatures (40, 50, 60, 70°C), with all other variables kept constant. The results show that increasing the temperature leads to faster reaction rates, as indicated by shorter reaction times.
Lab report writing
This document provides guidance on writing an eighth grade science lab report on how temperature affects the rate of a chemical reaction. It recommends writing a focused research question that specifies the independent variable (temperature from 40 to 80 degrees Celsius) and dependent variable (mass of reaction mixture in grams). The hypothesis should state that as temperature increases, the mass will decrease due to one of the products escaping as a gas. The method section describes the controlled variables and step-by-step process for conducting trials at different temperatures, recording data, and presenting it in a table.
Rates of reaction
Here are the effects on the rate of reaction of changing each condition:
- If the concentration of acid is increased, the rate of reaction will increase. This is because there will be more reactant particles per unit volume, resulting in more frequent collisions between reactants.
- If calcium carbonate powder is used instead of small pieces, the rate of reaction will increase. This is because powder has a larger surface area, allowing for more reactant particles at the interface where the reaction occurs.
- If the volume of acid is increased, the rate of reaction will initially increase but then level off. This is because there will be more reactant particles initially, but the reaction will use them up over time.
- If the
Rate of Reaction
The document outlines the procedures for 5 experiments that investigate factors that affect the rate of chemical reactions. The experiments will study how:
1) The size of calcium carbonate affects the rate of its reaction with hydrochloric acid.
2) The concentration of sodium thiosulphate solution affects the rate of its reaction with sulfuric acid.
3) The temperature of sodium thiosulphate solution affects its reaction rate with sulfuric acid.
4) The presence of manganese(IV) oxide affects the decomposition rate of hydrogen peroxide.
5) The presence of copper(II) sulfate affects the reaction rate between zinc and sulfuric acid.
TOPIC 5. RATE OF REACTION-LAB
The document discusses several experiments on factors that affect the rate of chemical reactions:
1. Particle size - Comparing the reaction of dilute HCl with large vs. small marble chips to see how particle size impacts the reaction rate. Smaller particles react faster due to a greater surface area.
2. Catalyst - Adding manganese dioxide speeds up the decomposition of hydrogen peroxide into oxygen and water, showing how a catalyst increases the reaction rate without being used up in the reaction.
3. Temperature - Measuring the time it takes for tablets to dissolve in hot, room temperature, and cold water, demonstrating that higher temperatures increase molecular motion and collision frequency, speeding up reactions.
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Rate of reaction temperature
This document outlines an experiment to determine how temperature affects the rate of reaction between sodium thiosulfate and hydrochloric acid. It describes the independent variable as the temperature of the hydrochloric acid ranging from 0°C to 80°C. The dependent variable is the time for a cross drawn on paper to become invisible when placed behind a test tube containing the reaction. The method involves timing how long it takes for the cross to disappear at each temperature, with results recorded in a table. The conclusion states that higher temperatures led to faster reaction times, supporting the particle collision theory that increasing temperature causes particles to move faster and collide more frequently.
Elly lee effect of temperature on reaction rate
Elly Lee conducted an experiment to observe the effect of temperature on reaction rates. Zinc was reacted with HCl at different temperatures and the reaction times were recorded. The results showed that reaction times decreased as temperature increased, with the fastest reaction occurring at 49.9°C and the slowest at 6.1°C. The type of gas produced also changed with temperature. This supports the hypothesis that increasing temperature increases reaction rates.
Effect Temperature Reaction rate
This document describes an experiment to observe the effect of temperature changes on reaction rate. The experiment involves a reaction between potassium permanganate, sulfuric acid, and oxalic acid. The reaction rate is determined by measuring the time it takes for the purple permanganate solution to become colorless. Results show that as temperature increases from 40°C to 70°C, the reaction time decreases and the reaction rate increases. The conclusion is that higher temperatures lead to faster reaction rates.
Temperature reaction rate
This document summarizes an experiment that investigates the effect of temperature on reaction rate. The experiment uses the reaction between potassium permanganate and oxalic acid, where the disappearance of the purple permanganate color indicates the extent of reaction. The experiment is conducted at different temperatures (40, 50, 60, 70°C), with all other variables kept constant. The results show that increasing the temperature leads to faster reaction rates, as indicated by shorter reaction times.
Lab report writing
This document provides guidance on writing an eighth grade science lab report on how temperature affects the rate of a chemical reaction. It recommends writing a focused research question that specifies the independent variable (temperature from 40 to 80 degrees Celsius) and dependent variable (mass of reaction mixture in grams). The hypothesis should state that as temperature increases, the mass will decrease due to one of the products escaping as a gas. The method section describes the controlled variables and step-by-step process for conducting trials at different temperatures, recording data, and presenting it in a table.
Rates of reaction
Here are the effects on the rate of reaction of changing each condition:
- If the concentration of acid is increased, the rate of reaction will increase. This is because there will be more reactant particles per unit volume, resulting in more frequent collisions between reactants.
- If calcium carbonate powder is used instead of small pieces, the rate of reaction will increase. This is because powder has a larger surface area, allowing for more reactant particles at the interface where the reaction occurs.
- If the volume of acid is increased, the rate of reaction will initially increase but then level off. This is because there will be more reactant particles initially, but the reaction will use them up over time.
- If the
Rate of Reaction
The document outlines the procedures for 5 experiments that investigate factors that affect the rate of chemical reactions. The experiments will study how:
1) The size of calcium carbonate affects the rate of its reaction with hydrochloric acid.
2) The concentration of sodium thiosulphate solution affects the rate of its reaction with sulfuric acid.
3) The temperature of sodium thiosulphate solution affects its reaction rate with sulfuric acid.
4) The presence of manganese(IV) oxide affects the decomposition rate of hydrogen peroxide.
5) The presence of copper(II) sulfate affects the reaction rate between zinc and sulfuric acid.
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The document discusses several experiments on factors that affect the rate of chemical reactions:
1. Particle size - Comparing the reaction of dilute HCl with large vs. small marble chips to see how particle size impacts the reaction rate. Smaller particles react faster due to a greater surface area.
2. Catalyst - Adding manganese dioxide speeds up the decomposition of hydrogen peroxide into oxygen and water, showing how a catalyst increases the reaction rate without being used up in the reaction.
3. Temperature - Measuring the time it takes for tablets to dissolve in hot, room temperature, and cold water, demonstrating that higher temperatures increase molecular motion and collision frequency, speeding up reactions.
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The document discusses how several factors affect the rate of chemical reactions according to collision theory:
1. Increasing the surface area of reactants by decreasing their size increases the rate of reaction by increasing collision frequency.
2. Higher concentrations increase collision frequency by providing more particles in a given volume, likewise increasing the reaction rate.
3. Higher temperatures cause reactants to move faster and collide more frequently, also increasing the reaction rate.
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Factors affecting rate of chemical reactions
The document summarizes experiments that demonstrate factors affecting the rate of chemical reactions. The experiments show that increasing the concentration of reactants, surface area of reactants, temperature, or adding a catalyst can increase the reaction rate. The nature of reactants also influences the reaction rate, as some combinations react faster than others.
Rate Of Reaction
Here are some potential solutions to optimize industrial processes to produce higher yields at lower cost:
1. Use a catalyst. Adding a catalyst can lower the activation energy of the reaction, allowing it to proceed at a faster rate even at lower temperatures and pressures. This reduces energy costs while maintaining or increasing product yields.
2. Improve reactor design. Advanced reactor designs that improve heat and mass transfer can allow reactions to reach optimum conditions more efficiently. Examples include continuous flow reactors, microreactors, and reactive distillation columns.
3. Employ process intensification techniques. Methods like ultrasound, microwave irradiation, and supercritical fluid processing can accelerate reaction kinetics, reducing processing time. Some also allow operation at lower temperatures and pressures.
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This document outlines the procedures for four experiments to determine heat of reaction: heat of precipitation by mixing silver nitrate and sodium chloride solutions; heat of displacement by adding zinc to copper nitrate; heat of neutralization by mixing hydrochloric acid and sodium hydroxide; and heat of combustion by burning butanol to heat water. It records the initial and highest temperatures of the reactions and solutions, as well as the mass of butanol used.
C14 rates of reactions
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This document describes an experiment to measure the rate of reaction between magnesium and sulfuric acid. The rate is measured by collecting hydrogen gas produced over time. The results show the volume of hydrogen increases rapidly at first as the reaction proceeds, then slows down as the magnesium is used up. The document also discusses factors that generally affect chemical reaction rates, such as concentration, surface area, temperature, and catalysts.
IB IA Chemistry HL Lab
1. The document describes an experiment to determine the equilibrium constant Kc for the esterification reaction of ethanoic acid and ethanol.
2. Initial concentrations of reactants and products were measured and the mixture was allowed to reach equilibrium. Samples were then titrated with sodium hydroxide and the volume added was used to calculate Kc.
3. The experimental value of Kc was found to be 4.80, which has a 20% error from the theoretical value of 4.07 given by the teacher. Sources of error are discussed.
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1) The document describes an experiment to determine the specific gravity and API gravity of kerosene and gasoline using two methods: the hydrometer method and pycnometer method.
2) The pycnometer method was found to be more accurate than the hydrometer method for measuring API and specific gravity, as the hydrometer can be affected by temperature, carbon dioxide, and alcohol content.
3) The API gravity value provides information about the quality and composition of petroleum products, with higher API gravity indicating a product contains more desirable and valuable components like gasoline.
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This a laboratory report of an experiment conducted at the American University of Nigeria as a requirement of completing the Petroleum Science course.
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2. The results found the API gravity of kerosin to be 48.53 using the hydrometer method but 35.56 using the pycnometer method, showing a difference between the methods.
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(Admiral) exp. no.3 find api of crude oil by wusing hydrometer
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Effect Temperature reaction rate
This document describes a lab experiment investigating the effect of temperature on reaction rate. The experiment involves mixing sulphuric acid, potassium permanganate, and water in an Erlenmeyer flask, heating the solution to different temperatures, and measuring the time it takes for the solution to change color with the addition of oxalic acid. The results show that as the temperature increases from 40°C to 70°C, the time it takes for the color change decreases significantly, from 135 seconds to 8 seconds, demonstrating that higher temperatures increase reaction rates.
Presentación (corregida)
This document summarizes an experiment that investigates the effect of temperature on reaction rate. The experiment uses the reaction between potassium permanganate and oxalic acid, where the disappearance of the purple permanganate color indicates the extent of reaction. The time it takes for the color to disappear at different temperatures (40, 50, 60, 70°C) is measured and the reaction rate is calculated as the inverse of time. The results show that increasing the temperature leads to faster reaction rates, demonstrating that temperature has an activating effect on reaction kinetics.
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There are several common methods for measuring properties of substances including salinity, pH, temperature, turbidity, and particle size. Salinity can be measured using an electrical conductivity meter or by measuring the amount of salt in a solution. pH is a measure of acidity and can be tested using pH paper or a digital pH meter. Temperature is measured with thermometers calibrated to different scales. Turbidity is assessed using a measurement of cloudiness, and particle size can be determined by measuring the displacement of water in a calibrated laboratory method.
Science example
The document summarizes a chemistry experiment that investigated how the concentration of hydrochloric acid (HCl) affects the rate of reaction when magnesium (Mg) is added. It was hypothesized that higher HCl concentrations would increase the reaction rate. Experiments were conducted using different HCl concentrations from 0.1M to 0.5M. The results showed that higher concentrations produced hydrogen gas faster, supporting the hypothesis. A graph of the reaction rates demonstrated they increased quadratically with increasing HCl concentration. However, the conclusion noted some weaknesses in temperature control and material reuse that could be improved.
acidity.pdf
This document describes a procedure for determining the acidity of water samples. It involves titrating an aliquot of the water sample with a sodium hydroxide solution of a known normality until the color change endpoint is reached using either phenolphthalein or methyl orange indicators. The volume of sodium hydroxide used is then used to calculate the total or mineral acidity levels present in the water sample expressed as mg/L of calcium carbonate equivalent. Precise sample handling, chemical preparation steps, a data sheet format, and calculation equations are provided to standardize the acidity determination.
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The document describes an experiment to determine how different concentrations of hydrochloric acid affect the rate of reaction with copper (II) powder. A colorimeter will be used to measure the absorbance of light by solutions containing copper (II) and hydrochloric acid over three minutes. Five concentrations of hydrochloric acid will react with 20g of copper (II) powder in separate trials. Variables like temperature, volume, and light intensity will be controlled. Absorbance readings will be taken and used to calculate the order of reaction and compare how concentration impacts the rate. The experiment will be repeated three times for each concentration to collect sufficient data.
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The document describes an experiment to investigate the effect of temperature on amylase activity. The aim is to determine the reaction rate of amylase and starch solutions at different temperatures (0°C, room temperature, 40°C, 60°C, 80°C). It is hypothesized that the reaction rate will initially increase with temperature until an optimal temperature is reached, above which the enzyme will denature and the rate will decrease. The method involves mixing amylase and starch solutions at the various temperatures and recording the time taken for the blue-black color from iodine solution to disappear. However, the results showed no color change, suggesting a failure of the experimental method.
Factors affecting rate of reaction (recovered)
The document discusses how several factors affect the rate of chemical reactions according to collision theory:
1. Increasing the surface area of reactants by decreasing their size increases the rate of reaction by increasing collision frequency.
2. Higher concentrations increase collision frequency by providing more particles in a given volume, likewise increasing the reaction rate.
3. Higher temperatures cause reactants to move faster and collide more frequently, also increasing the reaction rate.
4. Catalysts can lower the activation energy for a reaction, increasing the frequency of effective collisions and thereby accelerating the reaction.
5. For gas reactions, higher pressures compress the gas, providing more particles per volume and thus more collisions and a faster reaction.
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This document discusses measuring the pH of drilling mud using a pH meter. It begins with an introduction of the aim, which is to measure the pH of drilling mud to understand its acidity and alkalinity. It then discusses the theory behind pH and how hydrogen ion concentration relates to acidity and alkalinity. The apparatus used is a pH meter, which is calibrated using standard water. Samples are then tested and the pH is measured and recorded. The discussion covers how pH is important for drilling operations and can impact equipment, as well as methods for measuring pH.
Factors affecting rate of chemical reactions
The document summarizes experiments that demonstrate factors affecting the rate of chemical reactions. The experiments show that increasing the concentration of reactants, surface area of reactants, temperature, or adding a catalyst can increase the reaction rate. The nature of reactants also influences the reaction rate, as some combinations react faster than others.
Rate Of Reaction
Here are some potential solutions to optimize industrial processes to produce higher yields at lower cost:
1. Use a catalyst. Adding a catalyst can lower the activation energy of the reaction, allowing it to proceed at a faster rate even at lower temperatures and pressures. This reduces energy costs while maintaining or increasing product yields.
2. Improve reactor design. Advanced reactor designs that improve heat and mass transfer can allow reactions to reach optimum conditions more efficiently. Examples include continuous flow reactors, microreactors, and reactive distillation columns.
3. Employ process intensification techniques. Methods like ultrasound, microwave irradiation, and supercritical fluid processing can accelerate reaction kinetics, reducing processing time. Some also allow operation at lower temperatures and pressures.
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This document outlines the procedures for four experiments to determine heat of reaction: heat of precipitation by mixing silver nitrate and sodium chloride solutions; heat of displacement by adding zinc to copper nitrate; heat of neutralization by mixing hydrochloric acid and sodium hydroxide; and heat of combustion by burning butanol to heat water. It records the initial and highest temperatures of the reactions and solutions, as well as the mass of butanol used.
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This chapter discusses rates of reactions. It defines rate of reaction as how fast or slow a reaction is taking place. There are three main ways to measure rate of reaction: measuring time taken for reaction to complete, measuring amount of product formed per unit time, and measuring amount of reactant used up or remaining per unit time. The rate of reaction is affected by several factors like temperature, concentration, particle size, catalyst, and pressure. Temperature has the greatest effect as increasing temperature increases the kinetic energy of particles, leading to more successful collisions. Catalysts are substances that increase reaction rate without being used up in the reaction. They provide alternative reaction pathways or increase surface area for contact between reactants.
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This document describes an experiment to measure the rate of reaction between magnesium and sulfuric acid. The rate is measured by collecting hydrogen gas produced over time. The results show the volume of hydrogen increases rapidly at first as the reaction proceeds, then slows down as the magnesium is used up. The document also discusses factors that generally affect chemical reaction rates, such as concentration, surface area, temperature, and catalysts.
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1. The document describes an experiment to determine the equilibrium constant Kc for the esterification reaction of ethanoic acid and ethanol.
2. Initial concentrations of reactants and products were measured and the mixture was allowed to reach equilibrium. Samples were then titrated with sodium hydroxide and the volume added was used to calculate Kc.
3. The experimental value of Kc was found to be 4.80, which has a 20% error from the theoretical value of 4.07 given by the teacher. Sources of error are discussed.
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1) The document describes an experiment to determine the specific gravity and API gravity of kerosene and gasoline using two methods: the hydrometer method and pycnometer method.
2) The pycnometer method was found to be more accurate than the hydrometer method for measuring API and specific gravity, as the hydrometer can be affected by temperature, carbon dioxide, and alcohol content.
3) The API gravity value provides information about the quality and composition of petroleum products, with higher API gravity indicating a product contains more desirable and valuable components like gasoline.
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This document describes a lab experiment investigating the effect of temperature on reaction rate. The experiment involves mixing sulphuric acid, potassium permanganate, and water in an Erlenmeyer flask, heating the solution to different temperatures, and measuring the time it takes for the solution to change color with the addition of oxalic acid. The results show that as the temperature increases from 40°C to 70°C, the time it takes for the color change decreases significantly, from 135 seconds to 8 seconds, demonstrating that higher temperatures increase reaction rates.
Presentación (corregida)
This document summarizes an experiment that investigates the effect of temperature on reaction rate. The experiment uses the reaction between potassium permanganate and oxalic acid, where the disappearance of the purple permanganate color indicates the extent of reaction. The time it takes for the color to disappear at different temperatures (40, 50, 60, 70°C) is measured and the reaction rate is calculated as the inverse of time. The results show that increasing the temperature leads to faster reaction rates, demonstrating that temperature has an activating effect on reaction kinetics.
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1) The document describes an experiment to test how different types of sugar (white, brown, black) affect the growth of yeast when mixed together over 15 minutes.
2) The hypothesis is that black sugar mixed with yeast will produce more carbon dioxide than the other sugars.
3) The variables, materials, method, data table, and conclusion are described. The conclusion is that black sugar produced more yeast growth than the other sugars tested.
Measuring Abiotic Components
There are several common methods for measuring properties of substances including salinity, pH, temperature, turbidity, and particle size. Salinity can be measured using an electrical conductivity meter or by measuring the amount of salt in a solution. pH is a measure of acidity and can be tested using pH paper or a digital pH meter. Temperature is measured with thermometers calibrated to different scales. Turbidity is assessed using a measurement of cloudiness, and particle size can be determined by measuring the displacement of water in a calibrated laboratory method.
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Similar to Chemical reactions p pt
Science example
The document summarizes a chemistry experiment that investigated how the concentration of hydrochloric acid (HCl) affects the rate of reaction when magnesium (Mg) is added. It was hypothesized that higher HCl concentrations would increase the reaction rate. Experiments were conducted using different HCl concentrations from 0.1M to 0.5M. The results showed that higher concentrations produced hydrogen gas faster, supporting the hypothesis. A graph of the reaction rates demonstrated they increased quadratically with increasing HCl concentration. However, the conclusion noted some weaknesses in temperature control and material reuse that could be improved.
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This document describes a procedure for determining the acidity of water samples. It involves titrating an aliquot of the water sample with a sodium hydroxide solution of a known normality until the color change endpoint is reached using either phenolphthalein or methyl orange indicators. The volume of sodium hydroxide used is then used to calculate the total or mineral acidity levels present in the water sample expressed as mg/L of calcium carbonate equivalent. Precise sample handling, chemical preparation steps, a data sheet format, and calculation equations are provided to standardize the acidity determination.
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1) This experiment aimed to determine the statistical errors associated with diluting a 10M NaOH solution to 0.05M using seven different dilution pathways, including both direct and serial dilutions.
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The document summarizes a study measuring levels of iron (Fe2+), phosphate (PO43-), and nitrate (NO3-) ions in wastewater from four sources at a school over three months. Standard levels of each ion are provided for comparison. The principles and procedures of measuring each ion using UV-Vis or infrared spectrophotometry are described. Calibration curves were plotted and used to calculate ion concentrations from absorbance measurements. Results showed the canteen wastewater had the highest levels of Fe2+ and NO3- ions, while the wastewater behind the school had the highest PO43- level.
Report 1 prepare and standardize a 0.1 M NaOH solutions
This document describes an experiment to prepare and standardize a 0.1 M sodium hydroxide (NaOH) solution through titration. The student measured and diluted a 3 M NaOH solution to make an approximate 0.1 M NaOH solution. This solution was then standardized through titration against a 0.104 M sulfamic acid standard solution. The student determined the concentration of the NaOH solution to be 0.092 M on average, with a percent error of -9% due to imprecise measurement of the initial 3 M NaOH solution. The student concluded the procedure was successful in standardizing the NaOH solution and learning the titration technique.
Similar to Chemical reactions p pt (10)
Department of biochemistry cell ad molecular biology (1)
Department of biochemistry cell ad molecular biology (1)
Report 1 prepare and standardize a 0.1 M NaOH solutions
Report 1 prepare and standardize a 0.1 M NaOH solutions
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Chemical reactions p pt
- 2. Aim: To determine how the concentration of Hydrochloric acid affects the time taken for magnesium ribbon to disappear
- 3. Independent variable (What we are changing): Concentration of Hydrochloric Acid (HCl) Range: 100%, 80%, 60%, 40%, 20% of 2.0 M Dependent variable (What we measure to record for results): Time take in seconds for magnesium ribbon to disappear.
- 4. Controlled variables (What will remain the same) • Temperature of acid • Volume of concentration • Size of magnesium strip • Same person timing
- 5. Equipment: • 5 Test tubes • 10 mL Test tube stand • 10 mL Measuring cylinder • Magnesium Ribbon • 50 mL beaker • Hydrochloric Acid 2.0 M • Water • Stop watch • Thermometer
- 6. Method: 1. Collect 5 Test tubes, Test tube stand, 50 mL Beaker, Thermometer, Measuring cylinder, Stop watch and Bottle of hydrochloric acid (2.0 M) 2. Collect 10 pieces of magnesium ribbon, making sure they are exactly the same size. 3. Fill your beaker with tap water 4. Measure 5 mL of 2.0 M HCl using a measuring cylinder. Place in water bath to keep temperature constant. 5. Add Magnesium and record the time it takes to disappear. Start recording from the time you add the Mg to test tube and stop when it disappears (This is when the chemical reaction has finished) 6. Record Results in table. 7. Do steps 4,5 and 6 again to test for reliability 8. Test 80% concentration. Place 4 mL of 2.0 M HCl in a test tube and 1 mL of water. Place test tube in water bath. 9. Place Mg in Test tube and record from when you place it in the test tube until it has disappeared. - Record results 10. Repeat steps 8,9,10 again to test for reliability 11. Repeat steps 8,9,10 and 11 for 60% concentration, 40% Concentration and 20% concentration.
- 7. Milliliters of 2.0 Mol Hydrochloric Acid Milliliters of Water Concentration of 2.0 M Hydrochloric acid in Percentage (%) 5 mL 0 mL 100% 4 mL 1 mL 80% 3 mL 2 mL 60% 2 mL 3 mL 40% 1 mL 4 mL 20% Concentration Table:
- 8. Results Table: Time taken for Magnesium strip to disappear (seconds) Concentration of 2.0 M HCl Test 1 Test 2 Test 3 Average 100% 80% 60% 40% 20%
- 9. Graph Results: Time taken for Magnesiumto dissapear in different concentrations of 2.0 M HCl 0 20 40 60 80 100 120 100% 80% 60% 40% 20% Percentage Concentration of 2.0 M Hydrochloric Acid Time(Seconds) Time
- 10. Conclusion: Needs to state what happened in the results and how we know that it happened Example: These results show the higher the concentration of 2.0 Mol Hydrochloric Acid the faster the magnesium ribbon disappeared and therefore the faster the rate of reaction. The results show this clearly with the magnesium ribbon disappearing in _____seconds at the 100% concentration of 2.0 M Hydrochloric acid compared to the magnesium ribbon disappearing in ____ seconds at the 20% concentration of 2.0 M Hydrochloric acid.
- 11. Justification: Explanation of why you did what you did during the method • I used 5 different concentrations of Hydrochloric acid so that I can have accuracy in my data as the more tests I complete the more data I have to review • 1 only had one reaction going at a time to ensure that I correctly timed the reaction • I used the same equipment to ensure their were no differences in the measuring • I was the only one doing the experiment to keep the measuring and timing of the experiment the same. • I measured the magnesium so that they were all the same size so that the size of Mg was not a factor in the investigation. • We used a water bath to keep the temperature of the reaction the same
- 12. Collision THEORY
- 13. Discussion – Relate the finding from your investigation to the particle collision theory of reaction: The higher the concentration of Hydrochloric acid the more particles there are in the 5 milliliters of concentrate to collide with the magnesium, this means the chance of collision is greater which mean higher change o f effective collision. The higher the chance of collision between the Hydrochloric acid and the magnesium, the faster the reaction will be completed