Enthalpy Mind Map
Isla ALLEN
Created on March 23, 2022
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Transcript
Deconstruction
Types of Fuels Considered
How to investigate these factors
Safety Concern
Expectations
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Hydrocarbons - Potentially produce harmful fumes Wood - Heavy, require time to heat up Paper - Burns too quickly Coal- Takes a long time to heat up, heavy
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The efficiency of the different types of fuel can be investigated by doing experiments to test how fast they burn, how much fuel is required, and the fuel's weight. The cost can also be researched to find the most efficient and cost-effective fuel.
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Safety ConcernCausePrecautionsDrowsiness, respiratory irritationPotentially toxic fumes producedWell ventilated roomBurnsFlammable fuels, uncontrollable flameConduct in a safe space on work benchesEye DamageFuel in eyesWear safety glassesSkin IrritationSkin contact with fuelWash hands if in contact with chemicals.
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The expectations are that the chosen fuel will burn the least amount of fuel but produce the most amount of heat. This would be ideal for camping as less fuel would be needed, making the weight of the bag lighter and food able to be cooked quickly.
How to measure and record results
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Results will be recorded in a table much alike the one below:
Background Scientific Information
Limitations
Ways to test guiding question
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A fuel is a substance that can be made to react with another substance to produce exothermic energy. Exothermic reactions release heat energy to the surroundings. Endothermic reactions absorb heat energy from the surroundings. The heat energy of a reaction is measure in joules (J) and is found by following the equation: Q= m x C x Δ T where Q= heat energy released or absorbed (J) C= specific heat capacity of water Δ T= change in temperature of water(° C) m= mass of water (g) The molar enthalpy of a reaction is measure in kJ/mol and is found by following the equation: Δ H= (m x C x Δ T) / (1000 x n) where Δ H= molar enthalpy (kJ/mol) C= specific heat capacity of water Δ T= change in temperature of water (° C) m= mass of water (g) n= number of moles of substance (mol)
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Limitations include:
- Fuels available
- Time frame
- Equipment
- Loss of heat due to improper insulation/ equipment
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The guiding question can be tested by doing a range of different experiments and research to find the most cost-effective, lightest fuel that releases the most heat. The enthalpy of each fuel can be will be calculated following the method.
Experiment Set up
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Is the method explainable in steps
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- Set up apparatus as per diagram.
- Weigh the first fuel and burner. Record in results table. Place burner below beaker.
- Measure 100ml of water using a measuring cylinder, then add to 250ml beaker, held by the clamp.
- Adjust the height of the beaker until the base is 1cm above the top of the wick of the burner.
- Measure the current temperature of the water with a thermometer and record in results table.
- Light the burner and stir water in the beaker with the thermometer.
- When the temperature has increased by 20°C, blow out the fuel burner and immediately record the temperature of the water.
- Reweigh the burner to determine the mass of the fuel burnt. Return the fuel to the stock container.
- Repeat steps 2-8 with the remaining fuels.
- Calculate the enthalpy for each fuel using the equation Q= m x C x Δ T