How Much Co2 Lab

The next step in this lab is to rinse the Erlenmeyer flask with distilled water down the drain and then repeat the experiment, this time adding 10 ml of 0.10M KI and 10 ml of distilled water to the flask instead. The flask should again be swirling to allow the solution to succumb to the same temperature as the water bath and once it has reached the same temperature, 10 ml of 3% H2O2 must then be added and a stopper must be immediately placed on the flask and recording should then begin for experiment two. After recording the times, the Erlenmeyer flask must then be rinsed again with distilled water down the drain. After rinsing the flask, the last part of the lab can now be performed. Experiment three is performed the same way, but instead, 20 ml of 0.10 ml M KI and 5 ml of distilled water will be added and after the swirling of the flask, 5 ml of 3% H2O2 will be added. After the times have been recorded, data collection should now be complete.

As with many experiments that are performed in a setting where we cannot be exact on every measurement, error could arise from it. For instance, from this particular experiment, we needed to measure 5mL of water and 5mL of the borax mixture after it had cooled. Measuring 5mL with the bulb pipet that we were provided was not an exact measurement tool. The pipets provided were not calibrated and/or could have contained pockets of air with the assumed 5mL of water or solution.

When compared to the theoretical value, we had a 2.6% error in our experiment. Any errors that occurred maybe due to a too low intensity

We will be using the ratios 1:1, 1:2, 1:3, 4:1, and 5:1. We will tell how much carbon dioxide was produced from the reactants of the sodium bicarbonate and acetic acid. In our data shown below the data shows the ratios we used and the averages of the the carbon dioxide produced. We collected data so we can tell the amount of CO2 was

Soda is not only unhealthy because it is a sugary drink, but it is also the most acidic thing that people drink on a daily basis. Knowing this the question, which sodas will release the most carbon dioxide when mixed with hydrochloric acid arose. In addition, knowing background information about what it is that is being tested is very important. When it is said that soda is acidic that may catch people off guard, but how acidic soda is goes across as an even bigger surprise. The acidity of something is measured using pH. The pH scale is a way to measure the amount of hydrogen available to form a chemical bond. Containing a pH of 7 means that it is neutral in the acidity it contains. Soda has a pH of about 2.5 which is about the same pH as vinegar. To put this into perspective, battery acid has a pH of 1 and water has a pH of 7. Soda is closer in pH to battery acid rather than water in the amount of acid it contains. An interesting fact found was, “A pH below 4 or above 10 will kill most fish and very few animals can tolerate waters with a pH below 3 or above 11” (“8 Reasons Why People Drink Soda & 16 Reasons To Give Up Soda Drinking”). Hydrochloric acid can have range of the pH. This is determined on the concentration it is at. Muriatic acid is another name for hydrochloric acid. It can be found in the home in different cleaners. This acid is very poisonous (“Hydrochloric Acid”). Since the hydrochloric acid is secreted in the stomach, it is able

By subtracting the today’s barometric pressure by the pressure of water at 23oC given in the manual, we determined the pressure of O2 was 717.42 mmHg. We then used that information to find the volume of oxygen produced at STP using this equation:

In this experiment, the effect of temperature and agitation on soda will be observed. The pressure of a sample of soda will be observed at three different temperatures, and the pressure of the sample will be observed at those temperatures initially without agitation, and then with agitation for different amounts of time.

The third error encountered during testing also occurred during the first experiment. After the first three days of the trial, since the beakers were not covered, the water level began to decrease. Since more and more water was evaporating, the salt concentration became higher and higher causing the results to be completely inaccurate. In order to avoid this, the beakers could have been covered whilst not being used to ensure that minimal evaporation

In order to complete this lab students must have a well rounded understanding of the science concepts of the phase of gas and the properties of a gas, the experiment apparatus and how it works, the environment of the procedure including standard temperature and pressure and kinetic molecular theory. To complete the calculations students must understand stoichometry and conversion factors. A gas is a phase of matter that has no shape, no set volume, is easily compressed, and is less dense then both solids and liquids. When matter changes its state, gases can be formed. When liquids vaporize and when solids sublimate gases are formed. In the Molar Volume of a Gas Lab the gas is formed when a measured amount of Zinc metal is combined with five milliliters of Hydrochloric Acid the single replacement reaction occurs causing zinc metal to displace the hydrogen and form hydrogen, a gas and zinc chloride, a salt. In this reaction a gas is formed and bubbles of hydrogen are seen. The apparatus needed for this experiment consists of a small tub of water, graduated cylinder

Pressure caused by gases and gases being placed under pressure is used in our everyday life. Without the use of gases we would be unable to fly in airplanes, play basketball or even have carbonated drinks. “Gases exert pressure on any surface with which they come in contact, because gas molecules are constantly in motion. We humans have adapted so well psychologically to the pressure of the air around us that we are usually unaware of it” (Chang 155). The equation often used to measure the pressure of gases is the ideal gas equation P=nRT/V. Where P is the pressure of the gas in atm, n is the number of moles of gas, R is the proportionality constant (0.0821 L*atm) T is the temperature in Kelvin of the gas, and V is the volume the gas occupies (Chang 160).

Using the data from Table 1, calculations were performed to determine how much CO2 was expelled. This data is listed in Table 2. According to the data in Table 2, it is confirmed that more CO2 was expelled after exercising. While exercising, more oxygen is needed in the body for energy. Since more oxygen is inhaled, it makes sense that more CO2 is exhaled.

Abstract. In this review methods of photocatalytic reduction of CO2 are analysed and compared to determine the most suitable method to lower the CO2 concentration within the atmosphere. The use of transition metal, metalloporphyrin and supramolecular catalysts are investigated in depth, as well as Z-scheme photocatalysis. Comparisons of the methods are based upon efficiencies of the catalyst, selectivity and yield of the product and general commercial viability. It was found that the transition metal and supramolecular catalysts were generally more efficient than metalloporphyrin catalysts. Also, the Z-scheme despite being less efficient was notably cheaper and easier to produce.

The three gas laws that were covered during this experiment were: Boyle's law, Charles' law, and Gay-Lussac's law. These laws support this experiment's findings by showing the increased and decreased values. Boyle is an indirect (1/α), and Charles and Gay-Lussac are both a direct (α) relationship.

As previously stated, knowledge on this particular subject has been limited. Ever since Gause’s experiment, not many other scientists have attempted it until recently. As a class, the experiment was a way to observe competition and better interpret the results gathered

The results of the experiment showed that as the time the soda water was left out for increased, the moles of carbon dioxide present in the soda water decreased. Similar results can be seen in the following study conducted by R Wiebe and V. L Gladdy which investigated carbon dioxide solubility in water at different pressures and temperatures. This investigation found that at all temperatures, when the pressures were increased the solubility of the carbon dioxide also increased. At 40°, the cc of carbon dioxide per mL of water increased from 11.62 cc per mL at a pressure of 25 atmospheres to 36.73cc per mL at a pressure of 500 atmospheres (Wiebe & Gladdy, Solubility of Carbon Dioxide in Water, 1940). The results from the Wiebe and Gladdy corroborate the results of this investigation by showing that at lower pressures less carbon dioxide is dissolved in water. The results of this experiment occurred because the opening of the bottle causes the loss of carbon dioxide into the atmosphere due to the release of pressure. Prior to opening, the carbonic acid had reached equilibrium with the oxygen and carbon dioxide inside the bottle, which was a closed system. However when the bottle, and thus the system, was opened, the carbon dioxide was able to escape into the atmosphere. This lead to fewer moles of carbon dioxide, thus causing a decline in the quantity of carbonic acid. The change in pressure caused the equilibrium constant to change, as shown by le Chatelier’s principle. The