Carbon Looping Lab Report

The mixture of sodium bicarbonate and sodium carbonate can be separated due to the different temperatures at which the carbonate and bicarbonate decompose. This separation is the focus of the experiment. The bicarbonate decomposes when heated by the Bunsen burner. The carbonate also will decompose but at a much higher temperature. So, when the bicarbonate is heated it decomposes into carbonate, and during the decomposition it releases water and carbon dioxide. Furthermore, the amount of water and carbon dioxide released can be found by finding the difference in mass of the original mixture (before heating) and the final mixture (after heating). The mass of the water and carbon dioxide can be used to find the percent composition of bicarbonate in the mixture.

Write a balanced chemical equation for the reaction of carbon dioxide with limewater. The formula for the active substance in limewater is on the pipet, and the products of the reaction are calcium carbonate and water.

To use the ideal gas law, the atmospheric pressure was adjusted for due to the lower pressure in the buret when compared to the outer atmospheric pressure. This unequalization of pressures, although corrected, may still be slightly off, thus potentially causing later calculation error when using the ideal gas law to solve for the moles of CO2.

Here, the bicarbonate reacts with a proton(from excess acid in the stomach)to release carbon dioxide(H20 + co2).

Name: Date: Graded Assignment Unit Test, Part 2 Answer the questions below. Unless otherwise instructed, you may use a scientific calculator for this test. When you have finished, submit this assignment to your teacher by the due date for full credit. (5 points) Score 1. Nitroglycerine (C3H5(NO3)) is a powerful explosive.

Alka-Seltzer contains both baking soda (NaHCO3) and citric acid (H3C6H5O7). The reaction between the bicarbonate ion and citric acid produces water, carbon dioxide, and the citrate ion. Equation 1 shows the balanced equation for the reaction, which can be expressed by, C_6 H_8 O_7 (aq)+ 3NaHCO_3 (aq)→ 3H_2 O(l) + 3CO_2 (g) + Na_3 C_6 H_5 O_7 (aq) (1)

The procedure to obtain the mass lost for these two reactions was to first calculate the mass of HCl. For the first reaction, which was sodium bicarbonate, the mass of the beaker was weighted, then the grams of NaHCO_3 were added to the beaker and the mass was weighted. After recording the mass of the beaker with the NaHCO_3, 25 mL of HCl were added to the beaker and the mass after the reaction was weighted. To determine the mass lost in the reaction, the initial mass of the reagents was subtracted with the final mass of the reagents. The same procedure was performed with the sodium carbonate reaction, however 50 mL of HCl were used instead of 25 mL. Each chemical reaction was

Two tea bags, 1.1 g of sodium carbonate, and 40 mL of water were added to a 250 mL beaker. It was made sure that the tea bags were completely submerged. The contents of the beaker were swirled so that the sodium carbonate dissolved. The beaker was covered with a watch glass and the solution was heated and allowed to gently boil for 30 minutes. The beaker was then removed from the hot plate and allowed to cool.

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

If the amount of reactants (acidic acid and sodium bicarbonate) are increased then the amount of CO2 produced will be increased because of the law of conservation of mass.

Zainulabidin Adhami BB3 Experiment 3: The Gravimetric Determination of Calcium Abstract: The Gravimetric Determination of Calcium Lab utilized homogenous precipitation to determine the percent Calcium (Ca) in an impure sample of Calcium Carbonate (CaCO3). Three samples of 0.3574g, 0.3500g and 0.3736g of an impure sample of Calcium Carbonate (CaCO3) were added to three beakers, two of which were 250 ml and one which was 400 ml. These three samples were reacted with many different substances. After the reaction, presented above, was completed, the solution was promptly put into a vacuum filtration and then subsequently massed.

Sodium carbonate solution is used to provide the alkaline environment as it is a relatively strong base. When sodium carbonate is added to water to form the solution, sodium hydroxide, a base, is formed as shown in the equation below. Na2CO3 + H2O → 2NaOH + CO2

Do it the same way with other 3 examples of solution, which includes Sodium Carbonate solution and Calcium Chloride solution, Potassium Iodide solution and Silver Nitrate solution, Silver Nitrate solution and Calcium Chloride solution. 5. Record or collect all observations. Observation will be collect: by seeing when two chosen aqueous (Eg. Carbonate solution and Calcium Chloride solution) solution are mixed together it will become solid or a

Next, spatula tips of sodium bicarbonate were added to the solution until CO2 was no longer being produced. This was observed by when the solution stopped bubbling after the addition of the sodium bicarbonate. Once the sodium bicarbonate was no longer reacting with the

CO2 is the most significant greenhouse gas, which mainly comes from the use of fossil fuels. Many people feel that content of CO2 in the atmosphere is the main reason for manmade global warming. The main sources of CO2 emissions involve electricity generation, industrial processes, fumes from transportation and commercial buildings and use. Emissions of greenhouse gases, such as CO2, to the atmosphere are expected to cause even more of a significant change in global climate (Davison, 2007). The main focus to try to reduce the amount of carbon dioxide in the atmosphere is to reduce the amount that is released from coal-fired power plants. Greenhouse gas emissions that involve the productions of electricity come from natural gas production and coal-fired power plant operations. Natural gas production accounts for twenty-four percent and coal-fired power plant operations accounts for seventy-five percent, while the other one percent is caused by other electricity generation operations. The main reason why coal-fired power plants have a higher percentage of emissions is because the sulfur content of coal is much higher than that of other fossil fuels (Jarmaillo et al., 2007). This proves that there is a great need to find an alternative fossil fuel to use instead of coal. Although coal is easy to mine, transport and process for the electricity generation process, it is also the