Hydrochloric acid
White Cameron Mr. Bolton Physical Science 5 December 2009 Hydrochloric Acid Hydrochloric acid is one of the most acidic natural substances on Earth. Its name, Hydrogen chloride, comes from its chemical formula HCl. It is named this because it is an ionic bond. There is only one of each atom, because Hydrogen has a charge of 1 positive, and Chlorine has a charge of 1 negative. So using the "Criss-Cross Method" we can tell that there is only one of each atom. It is commonly referred to as Hydrochloric acid, or Muriatic acid. Their valence electrons are shared to form this compound. Hydrochloric acid is widely used in the modern world for the pickling of steel, or removing rust from iron and steel, it is even used to digest food in our bodies. It is a very useful compound in our everyday lives. Hydrochloric acid is essential for living nowadays, its wide range of uses makes life easier for everyone. The compound Hydrochloric acid has a unique set of physical properties. It is commonly found in its liquid state. It is sold at roughly distributed at 30% concentration, at a mixture of Hydrochloric acid and water. It is colorless to a light yellow. HCl's melting point is at -27.32°C. Its boiling point is at 110°C. Its density is 1.18 g/cm‹. It is an extremely corrosive substance with a ph level of -8 pKa. Hydrochloric acid has physical properties like no other
Compare and Contrast the properties and reactions of Butane and But-1-ene
Chemistry Essay Butane, Butene and all isomers that come with them are considered to be alkanes and alkenes respectively. They differ from each other in the fact that Butane contains only single bonds, whereas Butene has both single and one double bond. Regardless of this difference in many situations the two molecules can display similar behaviours. For the purposes of this comparison But-1-ene will be used as ‘Butene’ unless otherwise indicated. But-1-ene is almost identical to the other 3 isomers of Butene and hence makes a good molecules for comparison of the Butene group. Butene and Butane are both found to be extremely flammable gasses at Standard temperature and pressure, they will readily react with oxygen according to the following equations: C4H10+13O2 8CO2 + 10H2O C4H8+6O2 4CO2 + 4H2O Both of these reactions are very exothermic in nature. Inducing Fluorine in excess into a container of Butene will precipitate a addition reaction when the double bond between Carbons 1 and 2 is broken and attached to Carbons 1 and Two is Fluorine, creating CH2FCHFCH2CH3 or 1,2-diflurobutane Whereas the induction of a halogen in excess into a container of Butane will result in a substitution reaction where the electronegativity of the Fluorine causes one of the hydrogens to detach from the parent molecule and attach to the sister Fluorine resulting in Hydrogen
Alcohol Energy Release
GCSE Chemistry Coursework Planning a. I intend to investigate the factors, which affect the energy released by measuring the temperature change of water by the burning of different alcohols. For example, does the type of alcohol make a difference? b. The input variables I have identified are type of alcohol, size of wick, distance of wick to bas of calorimeter, amount of soot on calorimeter, amount of water in calorimeter. c. I will use temperature as my outcome variable by measuring the temperature at set time intervals d. I predict that the different types of alcohol will affect the temperature change (energy released) because each molecule of the different alcohols gives different bonds, when the bonds are broken, different amounts of energy are given of when the new bonds are formed. e. f. For each experiment in the series I will put 100cm3 of water into the calorimeter and make sure the underside is scraped of soot. I will keep the distance between the spirit burner and calorimeter a constant, although the size of the flame may vary. I will try to choose spirit burners with similar sized wicks so as to avoid a second variable altering the reactions. I will place a thermometer into the calorimeter and after the flame has been lit, I will check the temperature every 30 seconds to get a reading I will do this to a maximum of 4 minutes. g. I will ensure a fair test
Comparing the enthalpy changes of combustion of different alcohol’s
Comparing the enthalpy changes of combustion of different alcohol's PLANNING Apparatus The apparatus I will use during this experiment will be: - Heat Proof mat - Clamp - Retort Stand - Copper can - Measuring cylinder - Thermometer - Alcohol's (Methanol, Ethanol and Propanol) - Water - Bunsen Burner - Safety glasses - Access to balance - Draught Shield Quantities of materials required The only Quantity that I know I will use will be the 50ml of water. Method The Diagram below shows the apparatus set up for burning a liquid fuel. - Put 100cm3 of cold water in a copper can and record its temperature - Support the copper can approximately 2cm over a spirit burner containing the fuel you are going to test. - Arrange a draught system to reduce energy loss. - Weigh the spirit burner - Replace the spirit burner under the copper can and light the wick - Use the thermometer to stir the water al the time it is being heated. Continue heating until the temperature has risen by 15oC - 20oC. Do not let the thermometer touch the bottom of the copper can as this is the hottest part of the can and so the experiment would be unfair. - Extinguish the burner and immediately weigh the fuel burner to note the mass of fuel burned - Keep stirring the water and note the highest temperature reached. - Subtract the starting spirit burner weight from the second to
Formation of Ethanol
Formation of Ethanol. Ethanol is a straight chain alcohol (C2H5OH); it is a volatile, colourless liquid that has a strong characteristic odour. Ethanol is commonly used as a psychoactive drug in alcoholic beverages. It has a numeral uses such as an antiseptic, feedstock and fuel. Ethanol is notable as a renewable energy, derived by several means from the fermentation of sugar or hydration of ethylene; ethanol is being developed as an alternative to petrol to fuel cars. In present time, in several countries, ethanol is blended with motor fuels as an additive, to increase the octane rating of the fuel. This reduces ground-level ozone formation by lowering volatile organic compound and hydrocarbon emissions, decreasing carcinogenic benzene, particular matter emissions from the combustion of petrol, resulting in fuel burning more cleaning. As aforementioned, ethanol is made by two ways; hydration of ethylene and by the fermentation of sugars or cellulous. Fermentation Ethanol is the most common biologically produced alcohol. It is formed from the action of microorganisms and enzymes through the fermentation of sugars or starches, or cellulous, which is a more difficult process than the usage of sugars. The most widely know process of the formation of ethanol by the means of fermentation begins with carbohydrates; mainly monosaccharides and disaccharides such as glucose,
Methanol Basics
Methanol Methanol is the simplest alcohol, containing one carbon atom. It is a colorless, tasteless liquid with a very faint odor and is commonly known as "wood alcohol." Methanol is one of a number of fuels that could substitute for gasoline or diesel fuel in passenger cars, light trucks, and heavy-duty trucks and buses. It is also known as Methyl Alcohol. Why Consider Methanol? Methanol's physical and chemical characteristics result in several inherent advantages as an automotive fuel: ADVANTAGES * LOW POLLUTION Emissions from methanol cars are low in reactive hydrocarbons (which form smog) and in toxic compounds. Methanol-fueled trucks and buses emit almost no particulate matter (which cause smoke and odor, and can also be carcinogenic), and much less nitrogen oxides than their diesel-fueled counterparts. * FUEL SUPPLY Methanol can be manufactured from a variety of carbon-based feedstocks such as natural gas, coal, and biomass (e.g., wood). Use of methanol would diversify the country's fuel supply and reduce its dependence on imported petroleum. * FIRE SAFETY Methanol is much less flammable than gasoline and results in less severe fires when it does ignite. * HIGH PERFORMANCE Methanol is a high-octane fuel that offers excellent acceleration and vehicle power. * ECONOMICALLY ATTRACTIVE With economies of scale, methanol could be produced,
Science Coursework:Methanol & Ethanol
Aim: To observe temperature change in ethanol and methanol and predict which of the two fuels has the highest temperature while burning for 10mins. Introduction: I'm going to burn methanol and ethanol to find out which one of the fuels will have the highest temperature. Methanol and Ethanol are both types of alcohols. Methanol is a clear colourless liquid which is made from fossil fuels and natural gases. Ethanol is made from grains and is renewable. Prediction: I think methanol will have a higher temperature than ethanol because Fair test: The test was fair because the amount of water and temperature for both experiments were the same. The height of the flame was also the same and we timed each experiment for 10 minutes. We used the same equipment for both experiment. Safety: To make the experiment safe we tied back long hair, put on our goggles and cleared the space in front of us. Equipment: The equipment we used were: beehive stands, tripod, gauze mat, timer, thermometer, beaker, goggles and heat proof mat Method: 50ml of water at room temperature was poured into the beaker. The beaker was placed on a tripod which was on a gauze mat. The fuel was then lit and we used a thermometer to measure the temperature every minute. The experiment was repeated three times. Both fuels were used. We recorded the data in two tables; one for ethanol and another for methanol. We
Comparing the enthalpy changes of combustion of different alcohol's and fuels.
Comparing the Enthalpy Changes of Combustion of Different Alcohol's and fuels Plan Introduction In this experiment I will attempt to find out the energy needed to raise the temperature of 1g of water by 1oC using different fuels and alcohol's. This will enable us to determine the change in enthalpy for the different substances. Method * Firstly I will measure 200cm3 of water out into a copper coulometer * Then I will half fill a spirit burner with the required fuel, the burner must have a lid to stop evaporation * This will be weighed and the weight recorded * I will then set up the apparatus as shown above trying to keep the draft excluder ad need to the experiment as possible to reduce heat loss but not so close as to starve the reaction of oxygen, thus causing incomplete combustion * The water temperature will be recorded and the wick of the burner ignited * After securing the draft excluder with heat proof gloves and leaving a small gap at the bottom for air to get in I will stir the water to insure that the temperature rise is equal throughout the 200cm3 of water. * Just before a suitable temperature rise e.g. 20oc the flame will be extinguished with the burner cap to immediately stop the consumption of fuel. * The new temperature will recorded the new weight of burner weighed. * all information will be placed in a results table Safety To insure a safe
To find how much energy is released when different alcohols are burnt.
Aim To find how much energy is released when different alcohols are burnt. Prediction I predict that there will be more energy released when ethanol is burnt because it is a very flammable substance. Equipment Spirit burners, thermometer, tin can, clamp stand, goggles, Ethanol, Propanol, Butanol, Pentanol, Hexanol. Method We will get an alcohol burner and weigh it with the alcohol we're using and then set up the tin can above the burner. We will put 100ml of water into the tin can and take the temperature then we will light the alcohol burner and wait until the temperature has risen by 50°C. After the temperature has risen by 50°C we will re weigh the burner and record how much alcohol was used. We will repeat this for all 5 alcohols. Fair test I will keep this a fair test by keeping the amount of water the same for each alcohol and keeping the tin can the same distance from the burner for each one. Results Alcohols Used First Temp of water (°C) Final Temp of water (°C) Rise in temp (°C) Mass of water being heated (g) Mass of burner and alcohol at start (g) Mass of burner and alcohol at end (g) Mass of alcohol used (g) Ethonal 9 69 50 00 18.30 14.43 3.87 Propanol 22 72 50 00 60.46 58.21 2.25 Butanol 9 69 50 00 37.30 35.23 2.07 Pentanol 9 69 50 00 22.59 20.38 2.21 Hexanol 20 60 50 00 38.91 37.47
Describe, in terms of production of photochemical smog, what is meant by primary pollutants and secondary pollutants in the atmosphere, and list the main primary and secondary pollutants produced as a result of motor vehicles.
Chemistry Open Book 2003 Describe, in terms of production of photochemical smog, what is meant by primary pollutants and secondary pollutants in the atmosphere, and list the main primary and secondary pollutants produced as a result of motor vehicles The combustion of fossil fuels in vehicles releases incompletely burnt chemicals and oxidised species known as primary pollutants into the atmosphere. The dangers they pose range from eye irritation to global warming. Many of the primary pollutants undergo further reaction under the influence of sunlight. The produces of these photochemical reactions are called secondary pollutants. Primary pollutants consist of oxides of nitrogen. In the atmosphere nitric acid, which is produced by high temperature combustion cylinders in engines, is oxidised to the brown gas nitrogen dioxide NO2, a major constituent to smog. N2(g) + O2 2NO(g) 2NO(g) + O2 2NO2(g) Describe how primary pollutants are formed in the combustion of the fuel in a coal-fired power station Describe and explain the most favourable conditions for forming photochemical smog, and how the high concentrations of tropospheric ozone are produced Describe the chemistry of the processes chosen as BPEOs at Longannet for minimising sulphur dioxide and NOx, emissions, and suggest why the Longannet management made
