Calcium Carbonate and Self-heating Food
There are many different types of self-heating food and drinks, but there are more self-heating drinks available to purchase than self-heating food. Companies like HOTCAN only produce self-heating food, they have a lot of variety in what they sell in there cans. The price of the food varies depending on the stores but self-heating food is ranged between ? 3. 99-? 5. 99. Companies like OnTech produce self-heating drinks, drinks such as Coffee, Hot chocolate and tea.
These are more popular in the market and more common, this is due to more demand in people wanting to heat drinks up with ease. Self-heating drinks are much cheaper as well. Ranging between ? 2-? 4. What type of reaction takes place with the chemicals used? Self-heating cans heat up thanks to chemicals which are held inside the can but separate from the food or beverage inside. The chemicals are combined when heating is required and the reaction between them produces heat through an exothermic reaction.
Calcium Carbonate and Self-heating Food Essay Example
The heat caused by the reaction is then absorbed by the can’s contents.  The reaction used in self-heating food & drinks is safe it’s a non-toxic reaction which produces chalk, water and heat. (5) What chemicals are used to heat up self-heating food & drink products? Heat is generated inside Self-Heating food & drinks from the mixing of Calcium Oxide (quicklime, CaO) with Hydrogen Dioxide (water, H2O) which produces Calcium Hydroxide (Ca(OH)2).  The formula for this exothermic reaction is: CaO + H2O > Ca(OH)2 + Heat
Once the heating reaction is complete, the Calcium Hydroxide (Ca(OH)2) reacts readily with Carbon Dioxide (CO2 ) in the air to form Calcium Carbonate (limestone, Ca CO3) and returns to its original state The formula for this reaction is: Ca(OH)2 + CO2 > Ca CO3 + H2O The reactions are essentially CO2 neutral: Carbon dioxide (CO2) is released in producing the Calcium Oxide (quicklime, CaO ) by heating Calcium Carbonate (limestone, Ca CO3) to extremely high temperatures, and is subsequently reabsorbed during the reaction.  Data about how hot food and drinks can get, including the energy released per gram in these chemical reactions.
Hot can says their cans will get to 60°-70°C in 8 minutes, another source says that each gram of calcium oxide and water will give about 60 calories of energy which using the equation E=MC(change in)T, substituting values I get E=*4. 18*8, E Heat Genies reaction will heat 295ml of drink to 63°C in only 2 minutes, this is about 50,400 joules of energy, hot can releases more energy but takes more time than heat genie. Bibliography 1. http://hamzhang. blogspot. co. uk/2009/03/self-heating-can. html 2. Chemical ideas AS|A2,Heinemann,2008 3. http://www. hot-can. com/Australia/howto.
html 4. http://www. stress. com/consumertier3. php? pid=307 5. CGP Chemistry OCR Gateway The revision guide Richard Parsons 2011 Part 2: Planning & Collecting Data Hypothesis I predict that as the amount calcium chloride (CaCl2 ) increases the temperature rise will increase. I have said this because the energy in chemicals is held in the bonds between elements, as the chemical bonds form energy is released. If there is more calcium chloride there will be more chemical bonds therefore more energy can be released as heat energy which means the temperature should increase.
Plan Apparatus Risk assessment Preliminary Test Using 25ml of water I am going to test what amounts of calcium chloride will give me a good measurable change in temperature. Preliminary Test Results Amount of calcium chloride Water start temperature(? C) Water end temperature(? C) Temperature Change (? C) 1 25 27 2 2 25 30 5 3 25 35 10 From the preliminary test we have concluded that it will be better to start from 2grams and use 4, 6, 8 and 10grams as well as. They will show us readable changes without using too much calcium chloride.
Method 1. Measure 25ml of water in a measuring cylinder, then add it to the polystyrene cup 2. Measure 2 grams of calcium chloride using a balance and a measuring boat 3. Measure the start temperature of the water then record the temperature 4. Add the calcium chloride into the water 5. Observe the temperature using a thermometer in a clamp and stand 6. When the temperature stops rising, stop and record the temperature. 7. Repeat this 2 times 8. Repeat steps 1-8 with different amounts of calcium chloride: 4, 6, 8, 10Grams Results