Copy into this packet. Place flask in designated spot in classroom. Gas Volume Data Table Day data is recorded Circumference of balloon (cm) Day 1 4 cm Day 2 30 cm Day 3 33 cm Day 4 36cm Day 5 40 cm Analysis Questions Was your initial hypothesis correct? Restate your hypothesis and identify whether you were correct or incorrect, using data to support your answer. Yes, my hypothesis was correct (I predict the amount of gas produced over time by yeast is exponential, because it will keep growing overtime, and not by the same amount every single day.)
Introduction: Cellular Respiration is a process in which glucose is broken down to produce energy in the form of ATP. One of the products of cellular respiration is carbon dioxide. As cells produce carbon dioxide during cellular respiration, it is carried by the blood cells to the lungs where it is exhaled. To be able to test the rate of carbon dioxide, we use Bromothymol Blue, a chemical indicator that changes color as the pH of a solution changes. In a neutral solution, such as water, Bromothymol Blue is blue in color.
Aim: To investigate how different concentrations of hydrochloric acid affect the rate of carbon dioxide produced in the reaction with marble chips. Introduction: The reaction that takes place is shown below CaCO3 + HCl CO2 + H2O + CaCl2 As the concentration of hydrochloric acid is increased, this means that there is a higher probability of collisions due to the greater number of particular and so the rate of reaction will increas1e and more products will be produced. In this reaction the measurable product is the carbon dioxide produced which will be measured using a eudiometer. So we can find out by changing the concentrations of hydrochloric acid and finding the volume of carbon dioxide that is produced in a fixed time period as a comparison and hence determine the relationship. The eudiometer will show the displacement of the water in volume of CO2.
C3 Electrolysis and the Concentration Concentration of the solution (in g/dm3) | Current (in amps) | Average Results | | 1st try | 2nd try | 3rd try | | 8 | 0.54 | 0.48 | 0.57 | 0.555 | 12 | 0.63 | 0.66 | 0.64 | 0.635 | 16 | 0.84 | 0.81 | 0.85 | 0.845 | 20 | 0.92 | 1.1 | 1.04 | 1.07 | 24 | 1.34 | 1.15 | 1.62 | 1.245 | Conclusion My graph has a positive correlation. I can see from my table that the higher the concentration, the higher the current. Before I plotted my average results, I made sure that I identified the anomalies, by seeing which one stands out from the rest. I see the pattern because when it was 8 on average of 0.555 and then at 16 it was 0.845, this shows the test went well because it increased each time. The variables in this experiment are the concentration of solution.
Material * Three participants of similar weight and build. * Automatic Blood Pressure Monitor * Medium Measuring cylinder * Notebook to record results * 4 different caffeinated drinks – Kick Energy Drink, Coca-Cola, Hot Chocolate and Caffeine Free Coca Cola. * Clock and Stopwatch | KICK | COCA COLA | HOT CHOC | CAFFEINE FREE COCA COLA | MG IN 250ml of drink | 80mg | 23mg | 8.4mg | 0mg | Worked over 4 separate days (Monday, Tuesday, Wednesday and Friday) – 250 millilitres of each drink was measured out using a measuring cylinder. Using the automatic blood pressure monitor, the blood pressure of each participant was
Date : 18/02/2013 Micro-scale Determination of the Activation Energy of the Hydrogen Peroxide-Iodide Reaction Abstract: The purpose of this experiment was to determine the rate at which hydrogen peroxide decomposes to water and oxygen with the use of an iodide catalyst. Using the logarithmic form of the Arrhenius equation: ln k’ = -Ea/RT + ln A . the activation energy was determined to be 52.3 kJ/mol. It was also found that increasing the temperature also increased the rate, as there was more energy available to increase the speed of the reaction. Introduction: The purpose of this experiment was to determine the Activation Energy of the Hydrogen Peroxide-Iodide reaction.
From there, in order to balance oxygen, water molecules are enumerated to the opposite of the equation/reaction. Then from there, the Hydrogen ions need to be balanced, so the same numbers of Hydrogen ions are added to the opposite of the equation. Then it comes to the electrons, the same number of electrons added to a substance in the reduction half of reaction is taken away from the substance in the oxidation of half reaction. The last step is to add
Pocholo Panhon Rachel Smith -5 9/29/1999 Enzyme lab conclusion The problem that had was solved by the experiment was whether the pressure of a body was affected by a large amount of H2O2 being absorbed into it. I thought that if the amount of H2O2 (mL) increases then the pressure created by the reaction also increases, because in real life when somebody has a lot of H2O2 absorbed into their bloodstream the blood will start to froth and bubble up and pressure is created from it. To test this hypothesis I used H2O2 solution, blended cow liver, a flask with a pressure sensor hooked up to a laptop, 2 test tube (one for H2O2, and one for the cow liver). For the experiment I put a certain amount of H2O2 in one test tube and 10 mL of cow liver in another, then quickly emptied both contents of the test tubes into the single flask and put on the pressure sensor to figure out how much pressure was created. I did this five times with an amount of H2O2 then changed it by 2 mL higher while keeping the amount of the cow liver the same and continued to do everything else the same.
After 10 seconds, the colorless mixture suddenly turns blue. Concept: Demonstrates a typical clock reaction; shows the effect of the interaction between chemical reactions that have different rates. Materials: • Solution A o 0.6 grams Starch o 30 mLs of Acetic Acid o 4.1 grams of Sodium Acetate o 50 grams of Potassium Iodide o 4.7 grams of Sodium Thiosulfate ▪ Allow mixture to cool and dilute to 1 liter with distilled water o 1 liter flask • Solution B o 500 mLs of 3% Hydrogen Peroxide o 500 mLs of distilled water o 1 liter flask o Safety: Hydrogen Peroxide can be irritating to skin and eyes. Wear safety goggles and gloves. Procedure: Mix the two solutions together.
(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.