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,
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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
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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
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:
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-
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.
The results of this experiment are shown in the compiled student data in Table 1 below.
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
Possible sources of error in this experiment include the inaccuracy of measurements, as correct measurements are vital for the experiment.
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
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.
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.
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.
The aim of this experiment was to investigate the affect of the use of a catalyst and temperature on the rate of reaction while keeping all the other factors that affect the reaction rate constant.
There are five factors which affect the rate of a reaction, according to the collision theory of reacting particles: temperature, concentration (of solution), pressure (in gases), surface area (of solid reactants), and catalysts. I have chosen to investigate the effect of concentration on the rate of reaction. This is because it is the most practical way to investigate. Dealing with temperatures is a difficult task, especially when we have to keep constant high temperatures. Secondly, the rate equation and the constant k changes when the temperature of the reaction changes.
There was no temperature change; else, it would not have remained constant failing to validate Boyle’s law.
t = time, a = volume of reactant, k is a constant of proportionality; x is the order of reaction. Because k is a constant of proportionality 1/t is directly proportional to the rate of reactant. Then to find out the order of reaction in a catalysed system the volume of ammonia molbydate is varied and the concentration of the other reactants kept the same. Thirdly to investigate the activation energies, the concentrations are kept the same and the temperature is varied.