Experiment 1: Introducing Equilibrium I (Appendix 1) The purpose of this experiment was to observe what happens when the reactants and productions of a reversible reaction are placed separately into a sealed container. This experiment investigated the chemistry of equilibrium using N_2 O_4 ⇋ 〖2NO〗_2. This experiment will determine if dynamic chemical equilibrium can be achieved by starting with either reactants or products. In part one of the experiment, the following conditions were: Volume lock on 1 mole of N_2 O_4 and 0 mole of 〖2NO〗_2 0.0409M of N_2 O_4 and 0M of 〖2NO〗_2 IN 24.47 L at 106.4 kPa No catalyst No unreactive gas Temperature 40°C In part two of the experiment, the following conditions were the same as part one, …show more content…
Therefore, it can be concluded that a catalyst has a major effect upon the time taken in a reversible reaction to reach equilibrium in a closed system, but does not have any effect the macroscopic properties of the system. Experiment 9: Equilibrium III – Temperature The purpose of this experiment was to see if changing the temperature has an effect upon the value of the equilibrium constant. This experiment investigated the chemistry of equilibrium using N_2 O_4 ⇋ 〖2NO〗_2. In part one of the experiment, the following conditions were: Volume lock on 1 mole of N_2 O_4 and 0 mole of 〖2NO〗_2 0.0409M of N_2 O_4 and 0M of 〖2NO〗_2 IN 24.47 L at 101.3 kPa No catalyst No unreactive gas Temperature 25°C In part two and three of the experiment, the following conditions were the same as part one, but with: 50°C (part …show more content…
It was found that at 25°C the equilibrium constant equalled to 0046750725M, at 50°C the equilibrium constant was 0.0276014706M, and at 75°C the equilibrium constant was 0.126954023M (refer to appendix 3). So, it can be concluded that with increased temperature, the equilibrium constant also increases. In addition, the increase in temperature also increased the concentration of 〖2NO〗_2, but decreased the concentration of N_2 O_4, which can also be seen in appendix 3. Experiment 12: Le Chatelier’s Principle II Pressure Effects I The purpose of this experiment was to observe the effect on an equilibrium system when the pressure acting upon it is increased. This experiment investigated the chemistry of equilibrium using N_2 O_4 ⇋ 〖2NO〗_2. In part one of the experiment, the conditions were set to: Volume lock on 1 mole of N_2 O_4 and 0 mole of 〖2NO〗_2 0.0409M of N_2 O_4 and 0M of 〖2NO〗_2 IN 24.47 L at 101.3 kPa No catalyst No unreactive gas Temperature 25°C The temperature was changed to 50°C accordingly, which caused the pressure to change to 109.8
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
... got very different results, however they had carried out the experiment in slightly different ways, making it difficult to compare results.
When it comes to the observation part of forming the experiment as well as after the experiment was done, a lot of groups observed the same things. The most significant observations were we observed the
At equilibrium, the rate of decomposition of N2O4 is equal to the rate of combination of NO2. As the NO2 increases, then it starts declining as NO2 starts combining to form N2O4. This is called reverse reaction. The physical characteristic for this reaction is that the colour changes from colourless, d...
The Effect of Temperature on the Activity of the Enzyme Catalase Introduction: The catalase is added to hydrogen peroxide (H²0²), a vigorous reaction occurs and oxygen gas is evolved. This experiment investigates the effect of temperature on the rate at which the enzyme works by measuring the amount of oxygen evolved over a period of time. The experiment was carried out varying the temperature and recording the results. It was then repeated but we removed the catalase (potato) and added Lead Nitrate in its place, we again tested this experiment at two different temperatures and recorded the results. Once all the experiments were calculated, comparisons against two other groups were recorded.
Objective: The objective of the experiment is to determine what factors cause a change in speed of a reaction. It is also to decide if the change is correlated with the balanced equation of the reaction and, therefore, predictable. To obtain a reaction, permanganate, MnO_4^(1-), must be reduced by oxalic acid, C_2 O_4 H_2. The balanced equation for the reaction is:
2) the experiment with the milk jug and the hot water is that the milk jug will remain the same.
Specific heat capacity of aqueous solution (taken as water = 4.18 J.g-1.K-1). T = Temperature change (oK). We can thus determine the enthalpy changes of reaction 1 and reaction 2 using the mean (14) of the data obtained. Reaction 1: H = 50 x 4.18 x -2.12.
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
In a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
Another example of a systematic error that might have taken place during this experiment could have been that the room temperature water could have been in flux due to the fact that the temperature of the room may not have been constant and therefore the temperature of the room temperature water could have changed. This error could have been prevented by making sure that there were no occasional blasts of cold or warm air coming into the room that the experiment would be taking place
There is also the potential of human error within this experiment for example finding the meniscus is important to get an accurate amount using the graduated pipettes and burettes. There is a possibility that at one point in the experiment a chemical was measured inaccurately affecting the results. To resolve this, the experiment should have been repeated three times.
There was no temperature change; else, it would not have remained constant failing to validate Boyle’s law.
Possible sources of error in this experiment include the inaccuracy of measurements, as correct measurements are vital for the experiment.
Firstly, we need to keep the chemical at a constant concentration. So, in this experiment we have chosen to keep hydrochloric acid at a constant concentration (5cm3). We could have, however, used Sodium Thiosulphate as a constant, but we had chosen to use Hydrochloric acid. Next, we must make sure that the solution is kept at a constant volume throughout the experiment. If the volume is different, then it could give different results if it was at a constant volume.