Chemical Reaction and Test Tube
2.MATERIALS and METHODS
2.1. Nature of Reactants 2.1.1 We placed 3mL of 3 M HCl into each of 3 seperate test tubes. Next we added mossy zinc to the first test tubes, Sn granules to the second and Cu filings to the third and compared the rates of evolution of hydrogen gas in each test tube. 2.1.2. We mixed 3mL of 0.02 M KMnO4 and 2mL of 3 M H2SO4 in a test tube and stirred using a glass rod. Next, we divided the solution into two. We added 2mL of 0.03 M Na2C2O4 solution to the first half and 2 ml of H2O2 to the second and compared the rates at which the violet color of KMnO4 in the two test tubes disappeared.
2.2. Concentration 2.2.1. We placed into three separate test tubes 3mL of 12 M, 6 M, and 3 M of HCl each. Then, we placed Mg ribbons 1cm in length into each test tube and measured the time it took for each solution to dissolve the Mg ribbon.
2.3. Temperature 2.3.1. We placed 3mL of 0.2 M sodium thiosulfate solution into three separate test tubes. Next, we placed the first test tube in a 250mL beaker half-filled with water and applied heat. When the temperature reached 40º C, we added 3mL of 3 M HCl solution and measured the time it took for the solution to become cloudy. 2.3.2. We repeated procedure 1 using a temperature of 60ºC for the second test tube. 2.3.3. We palced the third test tube in a 250mL beaker with crushed ice and let it cool to 20ºC and added 3mL of 2 M HCl solution and measured the time it took for the solution to become cloudy.
2.4 Catalyst 2.4.1. We placed 2mL of H2O2 solution into two seperate test tubes and added a pinch of MnO2 to the first test tube and compared the rate of evolution of O2 in each test tube.
2.5 Particle Size or Surface Area 2.5.1. We secured two pieces of Mg ribbon 1cm in length and cut the first one into pieces and folded the the other. We then placed 3mL of 3 M HCl solution into two seperate test tubes. Next, we added the small pieces of Mg riboon to the first test tube and the rolled Mg
2.1. Nature of Reactants 2.1.1 We placed 3mL of 3 M HCl into each of 3 seperate test tubes. Next we added mossy zinc to the first test tubes, Sn granules to the second and Cu filings to the third and compared the rates of evolution of hydrogen gas in each test tube. 2.1.2. We mixed 3mL of 0.02 M KMnO4 and 2mL of 3 M H2SO4 in a test tube and stirred using a glass rod. Next, we divided the solution into two. We added 2mL of 0.03 M Na2C2O4 solution to the first half and 2 ml of H2O2 to the second and compared the rates at which the violet color of KMnO4 in the two test tubes disappeared.
2.2. Concentration 2.2.1. We placed into three separate test tubes 3mL of 12 M, 6 M, and 3 M of HCl each. Then, we placed Mg ribbons 1cm in length into each test tube and measured the time it took for each solution to dissolve the Mg ribbon.
2.3. Temperature 2.3.1. We placed 3mL of 0.2 M sodium thiosulfate solution into three separate test tubes. Next, we placed the first test tube in a 250mL beaker half-filled with water and applied heat. When the temperature reached 40º C, we added 3mL of 3 M HCl solution and measured the time it took for the solution to become cloudy. 2.3.2. We repeated procedure 1 using a temperature of 60ºC for the second test tube. 2.3.3. We palced the third test tube in a 250mL beaker with crushed ice and let it cool to 20ºC and added 3mL of 2 M HCl solution and measured the time it took for the solution to become cloudy.
2.4 Catalyst 2.4.1. We placed 2mL of H2O2 solution into two seperate test tubes and added a pinch of MnO2 to the first test tube and compared the rate of evolution of O2 in each test tube.
2.5 Particle Size or Surface Area 2.5.1. We secured two pieces of Mg ribbon 1cm in length and cut the first one into pieces and folded the the other. We then placed 3mL of 3 M HCl solution into two seperate test tubes. Next, we added the small pieces of Mg riboon to the first test tube and the rolled Mg