The equation for this reaction tells that for every mole of magnesium reacted, the amount of hydrogen gas produced will also be one mole. Looking at just the first trial, after the 0.0388 g of magnesium was finished reacting in an excess of hydrochloric acid, the amount of gas produced was 42.7 mL. The number of moles of magnesium reacted, which is the same as moles of hydrogen produced, was 0.00160 moles, found by dividing the mass of magnesium by its molar mass. This, along with the temperature and pressure of the room, could them be used to find the volume of gas at STP; however, this only after taking into account the water vapor pressure in the eudiometer, which is by 23.8 was subtracted from the barometric pressure of the room. Using the combined gas law, the calculated volume of the gas at STP would be 0.0377 liters.
The goal of the experiment is to synthesize a bromohexane compound from 1-hexene and HBr(aq) under reflux conditions and use the silver nitrate and sodium iodide tests to determine if the product is a primary or secondary hydrocarbon. The heterogeneous reaction mixture contains 1-hexene, 48% HBr(aq), and tetrabutylammonium bromide and was heated to under reflux conditions. Heating under reflux means that the reaction mixture is heated at its boiling point so that the reaction can proceed at a faster rate. The attached reflux condenser allows volatile substances to return to the reaction flask so that no material is lost. Since alkenes are immiscible with concentrated HBr, tetrabutylammonium bromide is used as a phase-transfer catalyst.
The active ingredients in the alka seltzer tablet are “As the tablets dissolve, the sodium bicarbonate splits apart to form sodium and bicarbonate ions. The bicarbonate ions react with hydrogen ions from the citric acid to form carbon dioxide gas (and water). This is how the bubbles are made.”(Scientific American) These bubbles are representative of a chemical change and the resulting carbon dioxide should increase the water 's density. This may actually increase the volume of the water taking longer to boil, this difference may be minuscule, even negligible, but there 's a possibility for distinct change in results. This scientific American puts it best “For the reaction to occur,
Explain what is meant by relative atomic mass?- Relative atomic mass is the measure of the mass of an element which consists of the protons and neutrons; it is always the bigger number and has the symbol Ar. An obvious example of this is oxygen has the Ar of 16 yet sodium has the Ar of 23. Explain how relative formula mass is calculated using the periodic table- You need to find the relative atomic mass (M) for each atom but this can only be done when the relative atomic mass have been found, then you add all of the masses in the compound together to find the RFM. Sodium Hydroxide is the example we used within our experiment. Na= 23 O= 16 H= 1 NaOH 23 + 16 + 1 = 40 NaOH Mr= 40 Explain how it is possible to work out amounts of substance
Procedure The aim of this experiment was to determine how variations in the amounts of calcium carbonate would affect the amount of carbon dioxide produced within the time frame of one minute. By measuring the amount of carbon dioxide produced, the changes in the rate of reaction could also be determined. By the end of the minute, the more carbon dioxide was produced, the faster the rate of reaction. Throughout the minute, the flask containing hydrochloric acid and calcium carbonate was swirled around in continuous, circular motions. At the end of the sixty seconds, measurements were read off the indicator lines on the measuring cylinder where the waterline sat.
Specifically, this investigation analyses how the initial temperature effects the rate of Hydrogen Peroxide oxidising Potential Acid Sulfate Soil. Only when a rapid reaction took place, PASS has been oxidised using Redox theory with the presence of pyrite or other sulphides to react. The hypothesis that the rate of oxidation is correlates with the initial temperature of the solution is true, with the theory being supported that the higher temperatures result in increased reaction speed. This lab test was conducted over two different depths of PASS, with three trials of five temperatures for each of the two depths. The first and most obvious form of evidence lays within the averaged pH levels over time.
Then 35 ml of 1.00 M of Sodium hydroxide was measured and set aside. Using the calorimeter, the hydrochloric acid was stirred heartily and its temperature was recorded as the initial temperature. The temperature of the Sodium hydroxide was assumed to be similar because they were both in the same conditions (lab) for the exact amount of time. Next the Sodium Hydroxide solution was added to the hydrochloric acid solution in the cups and stirred until the temperature stabilized. This was recorded as the final
Substrate concentration basically means the amount used for the substrate. The substrate in our experiment was 0.1% hydrogen peroxide. The 0.1% is the concentration amount. Just like temperature and pH, substrate concentration can speed the reaction only up to a certain limit. When we mixed pH 3 enzyme tube with substrate tube, we used 0.3 mL of hydrogen peroxide, but if we were to increase the amount, then the experiment would have been faster.
Experiment 9: The Molar Volume of a Gas Introduction Description: The purpose of this experiment was to determine the molar volume of a gas by conducting the hydrogen gas producing chemical reaction: Mg(s)+2HCl (aq)→〖MgCl〗_2 (aq)+H_2 (g) A known mass of solid magnesium was reacted with an excess of hydrochloric acid in a sealed vessel, three times, for a total of three trials. A gas pressure sensor and temperature probe were connected to the vessel and a computer which allowed Logger Pro to collect the pressure and temperature change data through the course of the reaction. This data was then used to calculate the molar volume of the hydrogen gas at STP, and the Universal Gas Constant, R, for each trial. Background: STP stands for
Catalase, or enzymes, drastically increases the rate of hydrogen peroxide decomposition. This lab shows how catalase added to hydrogen peroxide leads to the release of oxygen, if hydrogen peroxide was required to decompose naturally, life could not survive. The addition of catalase increases this decomposition rate allowing life to continue. For enzymes to operate they must be able to make contact with the substrate; the enzyme or substrate or both must