Burning Alcohols Lab Report

* Which of the following is true? Energy is created when a fuel is burned

C6H12O6 + 6O2 → 6CO2 + 6H2O + 686 kilocalories of energy/mole of glucose oxidized

overall, the investigation showed a positive correlation between the increase of carbon number in the linear alcohol homologous series, and the increase in enthalpy of combustion, which supports my hypothesis. Thus with the investigation of this experiment, it is to be concluded that, ignoring the cost of production, the more carbon in a alcohol, the more energy is released from the combustion of the molecule with oxygen.

have five C-H bonds, one C-C bond, one C-O bond and one O-H bond. To

And last but not least, the maximum temperature of alcohol was 26.5oC in 163 seconds. The data is shown in the Table 3 and the graph is shown in Figure

The purpose of this lab is to find most efficient way to capture energy from a combusted chip using a calorimeter. We made a basic calorimeter by using a steel can. Throughout our lab we made modifications to the calorimeter to increase the percent of energy captured by the water.

Alcohols are among the most common organic compounds on earth. They are used in toiletries, pharmaceuticals and fuels and are valuable intermediates in the synthesis of other compounds (Chemguide.co.uk, 2015). All alcohols vary in their degree of When fuels are burnt a combustion reaction takes place (bbc.co.uk, 2014). A combustion reaction is a type of oxidation reaction which is generally exothermic. Exothermic reactions result in the release of thermal and radiant energy. A combustion reaction occurs when a hydrocarbon reacts with oxygen to produce carbon dioxide and water (www.thoughtco.com, 2017). The energy released as heat during a reaction is the difference between that which is stored in the bonds of the molecules of the alcohol and

The energy that comes from the combustion from either ethanol or petrol comes from burning these hydrocarbons in order for the oxygen from the air to combine and combust (See Ethanol and the Environment for more). Energy is produced when the hydrocarbon bonds between the carbon and the hydrogen and

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

Calorimeters are devices used to indirectly calculate the energy output of burning fuels by measuring the changes of heat in a system which can then be converted to energy by known mathematical relationships. This investigation seeks to calculate the energy output of Ethanol and determine the optimal calorimeter apparatus for its combustion considering different types of insulation and the best substance in the Calorimeter to absorb the heat of the reaction.

The aim of this experiment was to test the heat of combustion over a period of time, and the energy required to combust alcohols with different carbon chain levels. It was hypothesised that the higher the carbon chain of the alcohol present, the faster the heat of combustion will occur. Meaning more energy will be released for a higher carbon chain. After calculating the results from the experiment it was found that the hypothesis was partially supported. The reasoning for this is as the alcohol that posses a higher carbon chain, generally increased there reaction rates. However there were a few exceptions to this rule.

The combustion of the hydrocarbons and organic molecules found in fuels is a chemical reaction that primarily involves the oxidation of carbon and hydrogen in various compounds to release heat and produce water and carbon dioxide. When the environment lacks sufficient oxygen, rendering oxygen as the limiting reagent in the reaction, incomplete combustion would occur. This involves the production of other chemicals such as carbon monoxide and solid carbon in addition to water and carbon dioxide. The general chemical equations for the incomplete and complete combustion of hydrocarbons are as follows:

This report will explore the energy release (or enthalpy change) when four different alcohols (methanol, ethanol, propan-1-ol, butan-1-ol) were burned. When these alcohols are burned, the chemical energy in their bonds is transferred into kinetic and thermal energy by heating water in a beaker. The rise in temperature of the water allows us to calculate the enthalpy change when each alcohol is burned in KJ mol-1.

Using this value it can be determined how my energy is required to raise the temperature of one litre of water from 20°C, to 100°C, as done by a kettle(Hyper Physics 2014). The amount of energy needed to boil the litre of water is; 4.2 × 1000 grams × 80 degrees = 336,000 joules, therefore it takes 336 kJ to raise the temperature by 80°C.

The purpose of this investigation is to explore how much energy is stored in different types of fuels and see which one would be better to purchase for a camping trip. The process that was used to find this was called calorimetery and the results from this were compared to the price per milliliter for each fuel. The fuel that was the best to purchase over all was deemed to be Ethanol. Ethanol was the alcohol fuel that held the highest amount of energy compared to the price and had the highest rating compared with the other fuels. The other fuels tested which were; Pentanol, 4 – methyl – 2 – Pentanol and Octanol.