substitution much less likely than para substitution‚ in which the bulk of the acetamido group has no influence. The ortho substitution product is formed in small quantities in this reaction. SPECIAL INSTRUCTIONS Concentrated sulfuric and nitric acids‚ in combination‚ form a very hazardous and corrosive mixture. These acids should be poured together carefully‚ and this procedure should be carried out in a hood‚ since noxious vapors are produced. You will begin with the sample of acetanilide
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of the total air pollution. It is produced by unburned fuel in the form of oxides of Nitrogen and hydrocarbons. One of the hydrocarbons produced is Carbon monoxide which is one of the most dangerous gases resulting in many health problems sometimes even death. Another cause of air pollution is Nitrogen oxides. Nitrogen oxide is one of the harmful gases‚ it is produced into the atmosphere by burning of fuel. Nitrogen oxide is very dangerous when combined with rain; it forms Nitrogen trioxide which
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Nitrocellulose Materials Christian Friedrich Schönbein’s procedure has been widely used. It calls for 1 part cotton to 15 parts acid. concentrated nitric acid concentrated sulfuric acid cotton balls (almost pure cellulose) Nitrocellulose Preparation Chill the acids below 0°C. In a fume hood‚ mix equal parts nitric and sulfuric acid in a beaker. Drop cotton balls into the acid. You can tamp them down using a glass stirring rod. Don’t use metal. Allow the nitration reaction to proceed for about 15
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In addition‚ nitric acid is not just yet another substance that you encounter and study in chemistry. It is actually utilized in many different industries. For instance‚ it is helpful in agriculture as it is utilized in the preparation of fertilizers such as ammonium nitrate. As you might have already identified‚ fertilizers aid improve meals production. One more chief use of the substance is in the production of explosives such as nitroglycerine and trinitrotoluene (T.N.T.). Likewise‚ did you know
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of Magnesium Oxide that was formed during the experiment: Average mass of Mg+ Average Mass of O2 = Mass of Magnesium Oxide 0.11g + 0.05g = 0.16g The mass of Magnesium Oxide formed in this experiment is 0.16 grams. Bar graph: The Magnesium’s increase in mass after the experiment. The bar graph shows an increase of mass of the Magnesium after the experiment was finished and the reaction occurred. Finding Magnesium Oxide’s Empirical Formula: Compound: Magnesium Oxide = MgO2 Mg:
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right when you need it. Hot-Can is non-toxic and non-flammable‚ and 100% recyclable. 1.How does Hot-Can work? Hot-Can has developed a special double-chambered aluminium can which contains the beverage in the outer chamber and holds water and calcium oxide (quick lime) separately in the inner chamber. When the seal at the bottom of the can is depressed and broken‚ the water mixes with the quicklime‚ starting an exothermic reaction that heats the contents of the outer chamber by 50-55°C in just 3 minutes
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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education *4308315385* CHEMISTRY Paper 2 Candidates answer on the Question Paper. No Additional Materials are required. READ THESE INSTRUCTIONS FIRST Write your Centre number‚ candidate number and name in the spaces at the top of this page. Write in dark blue or black pen. You may need to use a pencil for any diagrams‚ graphs or rough working. Do not use staples‚ paper clips‚ highlighters‚ glue or correction
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P-Nitroaniline is also used in gum inhibitors‚ poultry medicines and as a corrosion inhibitor. [2] Nitration is a type of chemical reaction which a nitro group is added to or substituted in a molecule. It can be carried out by a mixture of concentrated nitric acid and sulfuric acid. Mixture is useful to obtain the active nitronium ion. Electrophilic aromatic substitution is a method used when a functional group is needed to be substituted on to an aromatic compound. In the nitration‚ nitronium ion acts
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Magnesium Oxide: Lab Report The objective of the experiment is to determine the empirical formula of Magnesium Oxide through a procedure of heating magnesium ribbon to react with oxygen to form a magnesium oxide compound with the correct ratio of atoms within each element; 1:1. Equipment: REFER TO EXPERIMENT SHEET Method: REFER TO EXPERIMENT SHEET Results: Object | Mass (g) | Crucible + Lid | 38.23 | Crucible + Lid + Magnesium | 38.57 | Crucible + Lid+ Magnesium Oxide | 38.75 |
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| 0.16 | 0.08 | 0.24 | 0.19 | 0.11 | 0.30 | 0.21 | 0.11 | 0.32 | 0.23 | 0.09 | 0.32 | CONCLUSION: When a mass of magnesium is burnt in air‚ it combines with the oxygen molecules to form magnesium oxide. The graph doesn’t completely verify the empirical formula of magnesium oxide. There is a slight difference in the literature value of the empirical formula‚ MgO and the formula obtained from the graph. There are two points on the graph which do not fit into the trend line at all indicating
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