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Rate Of Reaction

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Name: Brendan Date : 24th Nov How temperature affects the rate of reaction Research Question: Does increasing or decreasing the temperature of hydrochloric acid affect the rate of reaction with magnesium? Introduction: The four factors that affect the rate of reaction; surface area, catalysts, temperature and concentration. In this case, it would be the temperature (Rate of Reaction of Magnesium with Hydrochloric Acid). According to the chemistry textbook, Chemistry higher tier, by increasing the temperature the rate of reaction increases. This happens because of the collision theory. The collision theory states that when particles are heated they gain more energy and move with a higher rate and force. Therefore …show more content…

Rate of Reaction Mg / HCl R2 = 0.96 The R2 value is close to 1 which means the data is reliable and accurate. The data for 28.0°C is the furthest away from the line of best fit probably because either the temperature or time was not measured properly. This graph evidently proves my hypothesis right. Although the room temperature experiment was not as close to the line of best fit as others, we can roughly estimate the time taken for the magnesium to dissolve in the hydrochloric acid. …show more content…

The hypothesis can be accepted because when the temperature of the hydrochloric acid was 55.0°C, the time taken for the magnesium to dissolve completely was 182.23 seconds. As I decreased the temperature of the hydrochloric acid, the 3 cm magnesiums trip took longer to dissolve. When the temperature was 42.7°C, the time taken to dissolve the magnesium strip was 406.26 seconds. The time taken increased dramatically by 224.03. This proves that my hypothesis was correct. Furthermore, my data compared to other resources are fairly similar. The rate of reaction approximately doubles every time the temperature increases by the 10°C (Ingram, Paul). Whereas my rate of reactions double every 20°C instead of 10°C. This tells me that I was not accurate enough with my timing and measuring. The results of the experiment was as predicted and more successful than I thought it was going to

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The reaction was repeated 3 times and average rate noted. From these rates a graph was plotted which describes the relationship of the pressure produced and number of drops added. The reaction rates were measured by Kpa/min and were written to 4 figures for precise results. Time was measured by stop watch. Table 4 shows a summary of all the groups which participated in the lab session.

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Our objective was to pick the best chemical to be used in a hand warm. This chemical had to be cheap, relatively safe, and must raise the temperature by 20oC and no more. We add 6 different chemicals to water we record the inshell temperature and then add one a the 6 chemicals to the water and record the temperature change of the water. We also add cold water hot water together to find how much heat would escape the calorimeter. We found that the calorimeter absorbed 71.1J/oC. Then this information to calculate the energy that was released by all of the chemical reaction.

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How is temperature related to this reaction? The higher the temperature the slower they move.

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This was done by taking the absolute value of the difference between the experimental value and the actual value, dividing by the actual value and multiplying by a 100. ((87.5005-92.09382)/92.09382)

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One way we could improve the experiment is by doing more trials, the more trials the more accurate the resolutes are. Another way we could improve the experiment is to have more time so we could make sure all the temperatures

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The reaction rate changes based on temperature, so if the cold temperature or hot temperature isn’t the same for all of the trials, the reaction time won’t be either. If the temperatures are too similar, like the cold and room temperature in all three trials, there isn’t a constant temperature gap to accurately see the reaction time difference. The temperature difference between the cold, room temperature, and hot water for each beaker should be constant for all trials. The timer could also be a potential error. The time needs to be started and stopped at the same point for all of the tablets, so human error could have occurred.

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One of the issues was pouring the water in the different test tubes at the same time, as only one member of the group poured in the water into the test tube at separate times. This is an issue as it makes the initial temperature for each of the test tubes lower than the recorded initial temperature (43 degrees Celsius) because the room temperature can cool down the water when the timer isn’t activated. It also affects the data as the temperature change for the first 3 minutes can’t be observed, so I can not know if the temperature for each of the test tubes decreased fast or slow from 0 to 3 minutes. This effect has great significance to making the data inaccurate, because the calculated temperature drop most likely is incorrect, meaning the evaluation of the hypothesis - that is based on the temperature drop - could be also wrong. Additionally, I can not observe an accurate reliable pattern between the different tests, because of the altered data.

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This occurs due to the fact that as temperature increases the kinetic energy, and thus the speed of the particles, increases. Subsequently, as the kinetic energy in the particles increase, the number of times the particles make contact, and have sufficient speed, grow allowing the rate of the reaction to increase. As a result, three different temperatures have been tested, one at room temperature, one at approximately 71oC, and another at roughly -4oC.

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What were some problems with the experiment? In the experiment I came along some slight issues with the experiment. On the first test we did. The weather was different compared to the second test, due to the difference in the weather and temperature.

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Exploration Title: Effect of Temperature on rate of Osmosis Submitted By: Abdulkarim Kamal Date Submitted: October 19th 2015 Subject: Biology HL Teacher: Mr. Nick   Aim: This is an investigation to determine the relation between temperature of a solution (sucrose) and the rate of osmosis Scientific Context: Osmosis is defined a passive transport process in which a fluid diffuses across a semi-permeable membrane, from an area of high solute concentration to an area of low solute concentration and vice-versa. There are various factors that could potentially influence the rate of osmosis; these factors include volume, concentration, and temperature. If all external factors that may interfere with rate of osmosis are controlled, the results will show equal amounts of fluid on both sides of the barrier (membrane); this is known as an “isotonic” state.

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Based off the values obtained in the experiment compared to the theoretical values, there is a very little experimental error, meaning the method was precise. Therefore, the calorimeter was efficient method of measuring the change in temperature because it allowed chemical and physical process to occur, while being isolated. Some of the errors that may have occurred causing the result not to be as precise, is that our eyes are not a precise measuring

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Experiment 5: Study of Solubility Equilibrium Aim To determine the solubility product constant Ksp of a sparingly soluble salt potassium hydrogen tartrate (KHC4H4O6) in water To calculate the change in enthalpy (ΔH° reaction) and entropy (ΔS° reaction) of the reaction Results and Discussion The dissociation reaction of potassium hydrogen tartrate (KHC4H4O6) in water can be written as: KHC4H4O6 (aq) ⇆ K+ (aq)  HC4H4O6- (aq) Determination of Ksp at 284 K The expression of its solubility product constant Ksp is Ksp =

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Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.

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