Chemistry - Rates of Reaction Investigation

As the substrate in increased the initial reaction rate will increase until it is fully submerged and then will not increase any more. The relationship is linear. As the substrate concentration increases, the initial reaction rate increases.

In this experiment we tested the effects that enzymes and substrate have on chemical reaction rates, which is the rate at which chemical reactions occur.. This experiment tested how different concentrations of enzyme and substrate affected the light absorption measurements on a spectrophotometer. The experiment also tested how temperature affected the light absorption, and in a separate test, the effect of the enzyme inhibitor hydroxylamine was also tested. In the first test conducted, 3 different concentrations of enzyme, and three different concentrations of substrate were measured in a spectrophotometer. For the enzyme and the substrate, the measurements got higher as the concentrations were higher, but the over measurements of the substrate were smaller than those of the enzyme. In the second test conducted, the medium concentration enzyme was tested under the temperatures; 4°C, 23°C, 37°C, and 60°C. The measurements in this test got higher as the temperature got higher, but did the measurements under 4°C were overall significantly higher than the other temperature measurements. Lastly, the last test conducted showed that the measurements of the substance with 0 and 1 drop of hydroxylamine inhibitor went up, but the measurements of the enzyme with 5 drops of hydroxylamine inhibitor stayed rather low and did not change much. In conclusion, these experiments showed that chemical reaction rates are sped up with higher concentrations of enzyme, substrate,

4. If HNO3 was used in place of HCl, I’d expect the rate of change to be about the same as both are strong acids. However, if acetic acid (CH3COOH) were to be used instead of HCl, I’d except the reaction rate to be slower as acetic acid is a weak acid and it will dissociate in the water unlike the stronger

Marble, or calcium carbonate, is a fairly insoluble compound with the chemical formula CaCO3. This compound has a carbonate ion, which has a charge of -2 and a calcium ion, which has a charge of +2. Calcium carbonate has a few forms including chalk and limestone. The main use of these two materials is in the making of concrete, which is used for many things including buildings. The rate of the reaction is the speed that the reaction takes place; therefore, by measuring the rate, the amount of time the reaction takes will be measured. Hydrochloric acid is a stronger acid that is found in digestive juices in the human stomach and is also used for cleaning metals before they are coated. When you mix a strong acid like HCl with any carbonate you will have a chemical reaction in which CO2 gas is released. This means that it will fizz indicating a chemical reaction. These two elements can react with hydrochloric acid to yield carbon dioxide, calcium chloride and water. The chemical reaction equation for hydrochloric acid and calcium carbonate is:

Kalah Bailey October10th 2015 Chem 109 Pre-Lab 6 Title: Observations of Chemical Reactions. In this lab, students will recognize and record the chemical reaction results of seven different anions and one cation. This experiment also focuses on the reaction of salt solutions and what happens when two different solutions mix.

The results obtained clearly prove the hypothesis stated as the average rate of reaction of the chalk and acid increased as the temperature changed from iced water, to room temperature, to boiling water. The average rate of reaction in seconds in room temperature water was 57.34, this decreased to 68.93 seconds when the chalk was placed in iced water and then when placed in boiling water there was a dramatic increase in the rate of reaction to 23.77 seconds.

Objective: This lab was performed to help students understand what enzymes do, what they are, and how they are effected by temperature, pH, and concentration. This lab write up only contains information based on the temperature portion of the lab. Introduction: In lab 5; enzyme activity, yeast solution was used as an enzyme to test the rate that oxygen was produced.

A few drops of hydrochloric acid, HCL were added to both of the solutions and the observations were recorded. It is observed that bubbles were formed in the sodium carbonate solution. It can be said that effervescence occurred during the reaction. Effervescence can be defined as the escape of gas from a solution and the foaming and fizzing that results from the release of a gas. As there is a gas that is released from the solution, the composition of the solution and its molecular formula must have undergone a change during the reaction and this change can be classified as a chemical change.

I aim to discover how different concentrations of Hydrochloric acid influence the rates of reaction. In order to carry out this investigation I have decided to use marble chips, which I will vary the sizes as powder, small chips and large chips. I will also be changing the concentration, the different concentrations are as follows 0.2m, 0.5m, 1m, 1.5, 2m. I have chosen these concentrations as they have a good range, we have to take this in to account, in view of the fact that if I was to use a concentration lower than 0.2m, the rate of reaction will be to slow or if I was to use over 2 molars, it is too dangerous to handle and violates

Just from looking at the aim of the investigation I already know that a salt would be formed because a carbonate with an acid forms a salt. In this investigation the substance that is formed is Calcium Chloride, Water and Carbon Dioxide. The symbol equation for this is:

By conducting this investigation we were able to discover the effects both reaction distance and breaking distance have when a person is faced with a pedestrian walking onto the road. The distance from when the driver recognised the pedestrian entering onto the road was 80 metres. The speeds of 40, 50, 60 and 80km/h were all able to stop in time. Even at 80km/h it was able to stop in 58 metres giving it plenty of distance to the pedestrian. Except for the legal speeds of 100km/h and 110/km/h were the only ones to fail and resulted in them having a collision resulting in serious injury or death. At the speed of 100/km/h it would take 81 metres to come to a complete stop and colliding with the pedestrian. It would have a collision speed of 16.2km/h

Chemical kinetics is based on the use of an experimental rate law to determine the mechanism of a reaction. The experimental rate law for the given experiment can be found through the experimental instantaneous initial rate and the concentrations of each of the reactants present. First, using the equation rate = k[A]n[B]m, a ratio can be created of the rate equation of trial 1 to that of trial 2. These two trials are chosen because the concentration of reactant A is the same for both trials, so it can be simplified to one in the ratio. Since k is a constant and thus the same in both trials, it can be simplified to one in the ratio as well. After exchanging variables for the experimental data and simplifying, the resulting equation is 0.5 = 0.5m,

We conclude that the concentration of hydrochloric acid does not have an effect on the rate of the reaction. The concentration of sodium thiosulfate, however, is directly proportional to the rate of the reaction.

Rate of Reaction Between Marble Chips and Hydrochloric Acid To investigate the factors which affect the rate of reaction between marble chips and hydrochloric acid, with one in specific detail. Scientific knowledge: Marble chips erode when they are exposed to acid rain or pollution. Erosion is evident when you look at older marble buildings as in certain cases the erosion take a long time. It is more likely to occur in areas, where there is more pollution.

Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid