Raw Data Page 10 Essay Example
Raw Data Page 10 Essay Example

Raw Data Page 10 Essay Example

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  • Pages: 5 (1254 words)
  • Published: September 19, 2017
  • Type: Essay
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There are several factors that affect the corrosion rate of marble buildings due to acid rain. These factors include temperature, concentration, pressure, surface area, and occasionally light. To better comprehend how acid rain corrodes marble, we conducted a study on the corrosion rate of marble chips using Hydrochloric acid. It is crucial to understand that sulphur dioxide (SO2) and nitrogen oxides (NO2), which consist of nitric oxide and nitrogen dioxide, are the primary chemicals accountable for causing acid rain. The emission of these pollutants into the atmosphere is attributed to both natural phenomena and human activities.

Throughout the history of the Earth, various natural processes have affected its atmospheric chemistry and climate. These processes include bacterial activity in soils, volcanic eruptions, and degassing from oceanic plankton. Volcanic eruptions are especially important because they release large quantities of S

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O2 into the atmosphere. Over time, there have been significant periods of volcanic activity that have resulted in the expulsion of substantial amounts of this gas.

While pollution caused by human activities has been known for centuries, it wasn't until the 19th century that the connection between pollution and acid rain was acknowledged. In fact, during Edward I's reign in England, using coal washed ashore from exposed sea floor beds was made illegal and punishable by death due to its harmful effects.

Industrial processes are primarily responsible for most atmospheric pollutants such as smoke from factories or emissions like SO2 and NOx from power stations. However, other activities including agriculture (pollen), construction sites (dust), and insulation materials (asbestos) also contribute to these pollutants. When it comes specifically to acid rain though, emissions from factories and power stations play a significant role.

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120 million tonnes of SO2 are released each year globally by industries that rely on oil and coal as fossil fuels. This has a significant impact on the environment, particularly in areas with concentrated industry and power production. In the Trent valley region of Britain, for instance, power stations located close to each other emit approximately 600,000 tonnes of SO2 annually. The formation of acid rain involves chemical reactions between ozone molecules (O2), reactive oxygen atoms (affected by sunlight photons), and water molecules (H2O). These reactions produce negatively charged hydroxyl radicals (HO) which play a crucial role in oxidizing sulphur dioxide and nitrogen oxide to create sulphuric acid and nitric acid.

Additionally, the creation of nitric acid can lead to additional reactions that produce more hydroxyl radicals. These radicals then contribute to the formation of additional sulphuric acid. Typically, these acids are carried to the Earth's surface as rainwater droplets originating from clouds. However, sulphuric acid is capable of condensing into small droplets, which contributes to various types of acid hazes, mists, and fogs observed in urban areas. Certain particles may fall onto the ground while vegetation can directly take in certain amounts of SO2 gas from the atmosphere.

Dry deposition, also known as the latter process, is separate from wet deposition or true acid rain. In urban areas, pollutants can be concentrated near the ground through temperature inversions, resulting in persistent smog. The December 1952 London smog covered an area with a radius of 30km from the center and had a pH range between 1.4 and 1.9, making it more acidic than lemon juice. This smog caused approximately 4,000 deaths due to bronchial infections.

Another instance of

acid deposition occurred on September 9th, 1989 along the Lincolnshire and Norfolk coastline in Britain. This incident was caused by heavy industry and vehicle emissions from Germany and Poland, leading to an acid mist with a pH of 2.

Thousands of trees have had their leaves scorched overnight and aluminium tools have corroded. These incidents are not uncommon. Athens, Mexico City, Tokyo, and Los Angeles regularly experience unusually high levels of sulphur and nitric acid.

We will be investigating the factor of concentration and my prediction is that if the concentration is doubled, the rate will also double, indicating proportionality. Our secondary factor is temperature and my prediction is that if the temperature is doubled, the rate will double as well.

The concept behind my predictions is explained by the collision theory. According to this theory, particles of different substances, like marble and hydrochloric acid, move around and react upon collision. Factors such as heat, pressure, concentration, and catalysts can speed up reactions. The collision theory can help us understand how these factors work. By heating a reaction, for example, particles are provided with more energy, causing them to move faster. Consequently, this increased motion increases the likelihood of collisions.

By increasing the concentration, the number of particles and the likelihood of collisions also increase, thus accelerating the reaction. This implies that changes in temperature or concentration will directly affect the rate of reaction. In order to ensure safety during the lab experiment, we cleared the working surface of any objects and removed our blazers while tucking our ties inside our shirts to prevent any interference with the experiment. Additionally, we consistently wore safety goggles and placed safety

mats on the desks. This investigation will focus on examining how the rate of reaction between hydrochloric acid and marble chips is influenced by varying the concentration.

In our experiments, we will manipulate the concentrations while keeping temperature, pressure, light, and surface area constant. To ensure sufficient observations, we will record each result three times and determine the average. We will cover a wide range of concentrations including 0.25M, 0.5M, 0.75M, 1.0M, 1.5M, and 2.0M to collect comprehensive data. Readings will be taken every 10 seconds for a total duration of 180 seconds. To enhance accuracy, we will measure three times and calculate the average value; this compensates for outliers by considering the other two readings and improves overall precision.

The gas syringe will provide results with an accuracy of two decimal places, while the stop clock will measure time with an accuracy of one second. During the preliminary work, we explored the impact of factors such as marble chip size, timing, and acid concentration. Three sizes of marble chips were used: small, medium, and large. The small chips resulted in readings that were too fast for the higher acid concentrations. The medium chips were suitable for most reactions, but proved too fast with the highest concentrations and too slow with the lowest concentrations. The large chips were optimal for higher concentrations but ineffective for lower ones. Therefore, we concluded that the medium chips would be the most appropriate choice. In the preliminary work, we agreed to record readings every 10 seconds and select concentrations and chip size accordingly.

When selecting the medium chips, we identified that the higher concentrations were most likely to contain errors, so we

opted for a smaller number of high concentrations and more lower concentrations. The experimental procedure involved the following equipment: Gas Syringe, 500ml Conical Flask, Measuring Cylinder, Hydrochloric acid, Distilled Water, Marble Chips, Electric Scales, and Stop Clock. Firstly, we cleared the workspace and followed the safety precautions outlined. Afterwards, we gathered our equipment and set it up according to the diagram provided. Then, we measured out 10g of medium marble chips and 10ml of acid.

We conducted an experiment where we added acid into a conical flask. Then, my partner placed marble chips into the flask and sealed it with a bung. Meanwhile, I started the clock. Every 10 seconds, my partner would communicate the results, and I would record them in a table. We measured the results by observing the quantity of gas released. Alternatively, we could have weighed the conical flask and recorded the loss of mass.

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