Compare The Rate Of Reaction Of Sodium Bicarbonate With Citric Acid

3. Turned off the laboratory burner and observed the properties of the product in the evaporating dish.

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the

always give out or take in energy most of the time this is heat energy

The aim of the experiment will be to investigate how varying water temperatures influence the time of a chemical reaction, in this case being, a combination of Sodium Thiosulfate and Hydrochloric Acid.

Experiment 2 focused on finding the enthalpy of solution of magnesium chloride. Testing the enthalpy of solution started with measuring out 10 mL of deionized water in a graduated cylinder for three separate trials, each trial having a different mass of magnesium chloride. The water was then poured into a well of a Styrofoam calorimeter then the initial temperature of water was taken using a temperature probe and the LoggerPro programming. A measured amount of magnesium chloride was placed in the same well as the water in the calorimeter,

In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The balanced formula for this is:

To see if the concentration of hydrochloric acid will increase the rate of the reaction between magnesium ribbon and hydrochloric acid.

In this experiment, we investigate the change in temperature caused by adding a chemical substance into the water and dissolving it. The results recorded in the table below show that our hypothesis is correct.

As the acid was being added, the mixture was being stirred over a stir plate. Once completed, the reaction mixture was poured from the round bottom flask into a 500 mL separatory funnel and its top (organic) layer was extracted into another beaker. The bottom (aqueous) layer was placed back into the funnel and extracted twice with 50.0 mL of ethyl ether each. The newly extracted layers were combined and dried over magnesium sulfate (MgSO4). The dried solution was the decanted into a beaker to remove the MgSO4 salts and the product solution was collected via Buchner vacuum filtration. The resulting product was transferred into an Erlenmeyer flask with an inverted beaker on top and stored in a drawer.

Equation of magnesium and hydrochloric acid: 2 HCl+ + Mg [IMAGE]Mg2+ + H2 Measuring rates of reaction In this investigation there are two experiments that can be used to test rates of reaction. Using a gas syringe As more gas is produced the plunger inside the syringe moves out of the syringe so the gas can be measured by marks on the syringes length.

The styrofoam cups were used to store the acid (cup was labeled A) and base (cup was labeled B) prepare for them to be mixed. A lid was put on cup A and then the temperature probe was inserted to begin to measure the temperature

Introduction: In this experiment we will be investigating how changing the temperature of the made up solution (copper chloride dihydrate and water) will impact the rate of a reaction when aluminium foil is dropped into it. We will determine this by selecting five different temperatures: 26 degrees, 36 degrees, 46 degrees, 56 degrees and 66 degrees and seeing at which temperature the reaction between the solution and aluminium foil produces the most heat. We will be recording the before and after temperatures after 2 minutes when the aluminium foil has been placed in the solution and also the average of the temperatures, this will help us determine if a hotter or colder

Part A of this experiment was essential because it set up the chemical solutions needed for Part B and C, as well as the equipment that was used throughout the entire experiment. To start, a 300mL solution of 2M HCl was prepared with the stock solution of 6M HCl. For this, 200mL of deionized water was collected and added it to a 400mL beaker. Then, 100mL of 6M HCl was added to the water. Next, 150mL of 2M NaOH was prepped by 50mL deionized water combined with 100mL 3M NaOH in another 400mL beaker. Before the experiment began, the LabQuest was plugged in and turned on. The temperature probe was then plugged into channel one of the LabQuest. In order to fully set up the LabQuest, the interval was changed to 15 s/sample.

The presence or absence of a catalyst also affects a chemical reaction because they speed up chemical

The procedure was performed as follows: For run 1, 20cm3 of acetone, 10cm3 of sulphuric acid and 145cm3 of water was added to a conical flask. 25cm3 of iodine was then added to this solution which started the reaction and immediately, 20cm3