Essay about Rate of Reaction Between Marble Chips and Hydrochloric Acid

The atmospheric pressure of a room affects the reaction rate as it forces the particles closer together therefore inducing more collisions. The more energy released from the particles raises the temperature. The higher the concentration of the solutions the more particles there are therefore making it more likely to collide. The surface area can have an influence on the rate of reaction as the element had more exposed surfaces, allowing the reactant to collide with the element.

The results for the rate of reaction, as seen in Table 2, suggest that as the temperature increases, the rate of reaction increases at a progressively greater rate. When the temperature increases 21℃ from 4℃ to 25℃, the rate of reaction increases from 1.846 s-1 to 6.1100 s-1 while a similar increase in temperature from 25℃ to 65℃ has a much more significant difference in the rate of reaction: 47.85s-1 at 65℃.

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

According to the collision theory, the rate of a reaction depends on the frequency of collisions between reacting particles. The more frequent the collisions, the faster the rate of the reaction. However, in order for the collisions to be effective, the particles must collide with sufficient energy (activation energy). Furthermore, the particles must collide with the proper orientation.

The first factor is: Temperature of reactants: When the temperature increases the particles move around faster (because they have more energy). Because the particles are moving faster , they are more likely to collide. When the temperature is low, the particles are slower and they also collide less. The

An Investigation into the Factors Affecting the Rate of the Reaction between Calcium Carbonate and Hydrochloric Acid

As the amount of the reaction’s product of oxygen and water (figure 3) was observed by reacting with detergent and measuring the amount of froth produced, the volume of froth indicated the rate of reaction between catalase and hydrogen peroxide. However, the raw data of the first average bubble production, 40ml at 6°C, is constantly discordant with the introduction’s knowledge on the effects of temperature on particle collision, therefore is indicative to have been an outlier, affected by errors, and hence is excluded from the line of best fit. Discounting the outlier, the trend in figure 4 highlighted by the line of best fit supports the hypothesis and can be explained by the knowledge discussed in the introduction. Figure 4, supporting the

The hypothesis for this experiment stated that as concentration increased, the rate of reaction would increase as well. The experiment proved this hypothesis partially correct. The data supported the hypothesis since between 0.4 M and 1.6 M hydrochloric acid, the rate of reaction increased as

The measure of how fast reactants are converted into products is the rate of a chemical reaction. Some reactions occur more quickly than others, but the reaction rate can be made faster or slower depending on certain factors. Concentration, surface area, temperature, and the presence of a catalyst are all factors that can affect the rate of a reaction. A reaction is considered complete when the entirety of at least one of the reactants has been converted into products. If the end of a reaction is indicated by a color change or the formation of a precipitate, then the reaction rate can be found by measuring the time from when the reactants were mixed to when the color change occurred or the precipitate was formed.

My graphs (following on separate sheets of graph paper) and results table show me that the rate of reaction is greater when the

The study that focuses on chemical reaction rates is kinetics. Kinetics contributes to the understanding of the speed of chemical reactions and what determines if a reaction happens at all. A large factor in determining if a reaction occurs is if the activation energy can be achieved. Activation energy is the energy required to start a chemical reaction so that it will not need any additional energy to continue. The amount of energy absorbed or transmitted by a solution is proportional to the solution’s molar absorptivity and the concentration of the solute, this is known as Beer’s law.

If the temperature of a chemical reaction is increased then the rate at which product is being produced in the reaction will also increase. This is because as temperature increases kinetic energy increases which causes the molecules to speed up. As molecules speed up there are more collisions which also means there are more successful collisions. The more successful collisions that there are the more product that is produced.

Rate of reactions play a vital role in real life situations. Everyday situations, such as cooking, require reaction rates to be increased. To bake some cookies, you place them inside an oven. But why is that? Well, placing the cookies in the oven speeds up the rate of the reaction by heating it up. When the cookies have more heat energy, they cook faster. Additives may be added to foods to speed up the reaction. These are called catalysts. Likewise, we place milk in our fridges to slow down the reaction rate by removing heat and preventing the milk from going bad. This is because the milk would turn sour if we left it out near a window. (14)

The surface area of a solid reactant can speed up a reaction. This is because if a physical change is made to the substance than the particles originally on the inside are now exposed and will react with other particles from another reactant.

In everyday life, several reactions are encountered, but still knowledge on how fast these occur and the factors affecting it were still insufficient. This study