How Does Surface Area Affect The Rate Of Reaction

In reference to the collision theory, molecules act as small spheres that collide and bounce off each other, transferring energy among themselves when the collide. In order for a reaction to occur, there must be collisions between molecules. Through experimentation, factors are discovered that influence the reaction rates of chemical reactions include the concentration of reactants, temperature, surface area, the physical state of reactants, and a catalyst. This experiment regarding the factors that affect reaction rate tests the effects of increased concentration and

As surface area increases, the reaction rate increases. This is represented by the positive slope and trend line.

From the results that were collect throughout the experimental investigation has proved the hypothesis to only be partially right. Multiple tests were made when conducting the experiment, two clear solutions were combined at various temperatures and concentrations. The hypothesis states that by adjusting the concentration of the reactants will cause the reaction to either speed up at a higher concentration or slow down at a lower concentration. In the reaction temperature should have a similar effect on the experiment, in that increasing the temperature will cause an increase of particle movement and cause more collision, thus increasing the reaction rate. Therefore decreasing the temperature will decrease the rate of the reaction. From the results given in Tables 2 and 3 it shown that every time the concentration is halved the time is increased. When the concentrations of both KIO3 and NaHSO3 are decreased the time has increased, some concentrations having a higher increase than others. In each concentration decrease the time is at least doubled from the previous concentration time, which is therefore increasing the rate of the reaction.

Limiting Reactant Lab Abstract The purpose of this lab was to use stoichiometry (fixed molar ratios) to determine quantitatively how Copper (II) Chloride and metallic aluminum react, known as an oxidation-reduction reaction. By varying the quantities of CuCl2H2O and Al and observing the reaction we were able to determine the limiting and excess reactants, and were also able to use stoichiometric calculations to determine the theoretical yield of Cu and then compare it to the actual yield of Cu to determine the percent yield of the reaction, which was found to be 22.5%. The percent yield of this experiment was less than desirable due to the fact that not enough Al was added to fully react all of the Cu. Using stoichiometry it was determined

This experiment is called Elephant’s toothpaste. Which is a decomposition reaction where hydrogen peroxide (H2O2) is decomposed with the aid of a catalyst (either Sodium iodide or Potassium iodide). By placing a small amount of detergent in the mixture the amount of oxygen produced can be determined by the volume of foam produced in 2 minutes. By performing the experiment at different temperatures its tests the effect varying the reaction temperature will have on the reaction rate. My hypothesis was If the temperature of the reaction rate is increased than the oxygen production will

Many factors effect reaction rates, two shown above include temperature and concentration. Concentration affects the rate of reactions because the more concentrated a solution the more likely collisions between particles will be. This is simply because there are more particles present to collide with each other. When the temperature is higher, particles will

Enzymes are proteins which can catalyse chemical reactions without changing themselves. The enzyme lipase breaks down the fat in dairy products such as full-cream milk for people who are lactose intolerant. Lipase acts on its specific substrate, lipids produces fatty acids. If enzyme concentration increases, random collisions between the substrates and active sites of enzyme increase due to the increasing amount of active sites which allow more collisions to happen, so the rate of breakdown of lipids to simpler substances will increase. During the experiment, sodium carbonate solution and pH indicator phenolphthalein will be added ahead of

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.

The null hypothesis for the first experiment was that substrate concentration would have no effect on the reaction rate. It was hypothesized that the reaction rate would increase with rising substrate concentrations, until all active sites were bound. The null hypothesis for the second experiment was that temperature would not have an effect on reaction rates. It was hypothesized that until the enzyme is denatured, as temperature increased, so would the reaction rate.

This means that substances that absorb more hydrogen ions will produce faster reactions times due to higher temperatures. The data obtained from this experiment did not support the claim hypothesized. In the hypothesis it was stated that the acidic solution would produce the fastest reaction time. At the end of the completed experiment it was discovered that the basic solution produced the fastest reaction time of 60.771 seconds, while the acidic solutions reaction time was 65.971 seconds, and the neutral solution produced a 63.425 reaction time. Some potential problems that could have arouse during this experiment were that not all beakers contained the same amount of substance. Since the liquids were measured with the naked eye there is a chance that amount of solutions in each beaker were different. Another potential issue could have been not allowing all of the antacid tablet to dissolve before stopping the timer. This issue much like the one stated before would be hard to tell by just looking at the experiment with a naked eye. Perhaps in another experiment looking to test pH and reaction times an experimenter should take solutions ranging across the pH scale and change the temperature of each substance to see how temperature can affect the reaction

The cup with the second greatest change in mass of the rock was number 2. Cup 2 had the solution of 10% vinegar and resulted in the change of -0.3g. Lastly, Cup 3 with distilled water had the lowest change in the mass of the rock, of 0g. It was hypothesized at the beginning that Cup 3 with distilled water would have the least amount of change, if any. This hypothesis was correct. Water is not acidic, so there would be no reason for the rock to change. When the hypothesis was conducted, it was based on the pH level. Instead, the actual solution should have been taken into consideration. The fact that the soda water would eventually lose its carbonation and become flat within a few days. Therefore, taking the acidity away. The experiment was done correctly, and there did not need to be any changes. Just the hypothesis could have been more thoroughly

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,

2. Slope can be used to determine the effect of the magnesium on the reaction rate by how close it is to the number one, when it is showing an increase in reaction rate. As hypothesized, the magnesium with the greatest surface area would have the fastest reaction rate. Hence, it would have the greater slope value as well.

In my hypothesis, I stated that there would be a faster reaction rate when the marble chips are small and is mixed with a higher level of concentration ( crushed marble chips, 2.0M hydrochloric acid). According to my results, there was a faster reaction in Part B, which was the small chips mixed with 2.0M HCI.

The results of the experiment prove the hypothesis of the group. It was hypothesised that the less diluted the acid is, the faster the ant-acid will dissolve. The results show this, as the ant-acid in the 0.5M acid took 9:02 minutes to dissolve; the ant-acid in the 1.0M acid took 2:50 minutes to dissolve and the ant-acid in the 2.0M acid took 2:09 minutes to dissolve. The trend of this experiment is the downward slope of the time when the acid becomes stronger, however, it is not as mathematically correct as the group had expected. The group had hypothesised that the 1.0M acid would take half the amount of time that the 0.5M acid would take, and the 2.0M would take half the amount of time the 1.0M acid would take. This was not the case, as