what can you use exothermic or endothermic reactions in daily life?
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Exothermic reactions are very common.  Most oxidation reactions are exothermic.  This would include rusting iron as well as burning just about any kind of fuel: gas, oil, wax, gasoline or alcohol.  In all of these reactions something is reacting with oxygen and the reaction gives off heat.\nEndothermic reactions are much less common. Commercially available cold packs usually consist of 2 inner containers, one with urea and the other containing ammonium chloride within a plastic bag.  When the containers are broken (usually by bending) the compounds react and absorb heat from the environment.  This makes the bag get cold.
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Hi Kitty,\nHere is what, I think, you need.\n\nExothermic, dH < 0, Entropy increases (dS > 0), Reaction is spontaneous and dG < 0\n\nExothermic, dH < 0, Entropy decreases (dS < 0), Reaction is spontaneous only at low temps, if |T dS| < |dH|\n\nEndothermic, dH > 0, Entropy increases (dS > 0), Reaction is spontaneous only  at high temps, if T dS > dH\n\nEndothermic, dH > 0, Entropy decreases (dS < 0), Reaction is not spontaneous, dG > 0
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Completely exothermic. The atoms are losing energy to get to a solid state. Gases have most energy since they are free and unbonded to neighbouring molecules. Liquids have enough energy to stay together but still move about one another. In solids they have just enough energy just to vibrate about in a fixed point, closely bonded to neighbouring atoms. As you can there is an energy loss as you go from gas state to solid state. Loss of energy is exothermic.\n\nYes it is a reaction to change of heat.
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In chemistry, an exothermic reaction is one that releases heat. It is the opposite of an endothermic reaction. Expressed in a chemical equation:\n   reactants -->product + energy\n\nWhen using a calorimeter, the change in heat of the calorimeter is equal to the opposite of the change in heat of the system. This means that when the solution in which the reaction is taking place gains heat, the reaction is exothermic.\n\nIn an exothermic reaction the total energy absorbed in bond breaking is less than the total energy released in bond making.\n\nThe absolute amount of energy in a chemical system is extremely difficult to measure or calculate. The enthalpy change, ΔH, of a chemical reaction is much easier to measure and calculate. A bomb calorimeter is very suitable for measuring the energy change, ΔH, of a combustion reaction. Measured and calculated ΔH values are related to bond energies by:\n\nΔH = energy used in bond breaking reactions - energy released in bond making products.\n\nFor an exothermic reaction, this gives a negative value for ΔH as a larger value is subtracted from a smaller value. For example, when hydrogen burns:\n\n\nIn Chemistry an endothermic reaction is one in which the products have more energy than the reactants, and thus a net input of energy, usually in the form of heat, is required. Endothermic reactions are often described as reactions that "feel cold", and contrast with exothermic reactions, in which heat is released.\n\nAlthough the process of bond breaking amongst reactants in a chemical process requires an initial input of energy (the activation energy), in the case of an endothermic reaction, the energy released when bonds are formed to create reactants is less than that required to break the bonds in the products; bonding electrons in the products are therefore at a higher energy than the reactants. Heat energy from the material surrounding the reactants is usually what breaks their bonds, so as heat energy is transferred from the surroundings to the reactants, the surroundings get colder. This is often summarized in a chemical equation as follows:\n\nReactants + Energy → Products
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"A thermite reaction (a type of aluminothermic reaction) is one in which aluminium metal is oxidized by the oxide of another metal, most commonly iron oxide. The name thermite is also used to refer to a mixture of two such chemicals. The products are aluminium oxide, free elemental iron, and a great deal of heat. The reactants are commonly powdered and mixed with a binder to keep the material solid and prevent separation."\n\n"Uses:Thermite reactions have many uses. It was originally used for repair welding in-place such things as locomotive axle-frames where the repair can take place without removing the part from its installed location. Thermite grenades are used in war to destroy sensitive equipment or documents when at imminent risk of capture by the enemy. Thermite grenades and bombs have been used in combat as incendiary devices, able to burn through heavy armor or other fireproof barriers. Thermite can also be used for quickly cutting or welding metal such as rail tracks, without requiring complex or heavy equipment. It also enables infantry to destroy enemy artillery without the use of loud explosive charges and therefore operate with stealth. The mixture has been sold for many years under the trademark name Thermit for use in railroad welding."
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Here's a way to turn a common household chemical reaction into some fun.\n\nhttp://www.torgo.org/bpsubs/
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if you go from A to be and then B to A you should have no overall energy change. one will be an exothermic reacion and the other should be endothermic reaction
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id say reactions can occur at any temperature above 0k. so 0.00000000000000000000000000000001K, the reaction would happen but really really really really relaly slowly. but thatz in theory. i have no clue bout pracitcally. i think the lowest temp theyve got to so far is either 4K or 0.6K. so ya.
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U CAN MAKE A PROJ ON REACTIONS ON THE FOLLOWING PTS  .\n INTRO OF REACTIONS\nDEFINITION OF A REACTION\n TYPES OF REACTIONS\n THEN, DESCRIBE THEM SEPARATELY
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rubbing 2 things together to create heat.\nRub yor hands together really fast and see what happens.
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Yes, provided the conditions are right. For example if the reaction\n\nA + B -> c + d\n\nis exothermic, the reaction in reverse will be endothermic, i.e. you will have to supply the heat.
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Find out how thermodynamics can improve daily life. Industrial apllications too.
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endothermic is energy taken in, exothermic is energy given out you should be able to do the rest
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Add heat.\nAdd a catalyst.
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many chemical reactions happen at the interface between different phases of solid, liquid, or gas.  the reaction rate is often limited by the surface area - so to increase the rate, you can increase the surface area. \n\n an example of this is in batteries - the ion-exchange process that batteries use happens at the surface of the electrode, where the solid metal electrode exchanges ions with the electrolyte solution.  lots of newer batteries use highly-porous materials for the electrode - all those little pores can increase the surface area by several orders of magnitude, allowing the reaction to run much faster.\n\nso, if you know how to drive it out of the rocks, then you're in good shape.  a simple answer to increase the rate is to crush the rocks into small grains.  this will allow for a much greater surface area, so water diffusing through the rock will make it to the surface sooner.\n\nalso, many reaction rates are sped up by increased temperature.  so you could build a fire and heat the rocks.  an increase in temperature means, on the molecular scale, that the atoms are moving faster - this means your reaction goes faster - and the water comes out faster.
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Exothermic\n\nSugar(with yeast)--->\nalcohol+carbondioxyde+heat
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An acid and a base react to form a salt and water.  For example:  NaOH + HCl ==> NaCl + H20.  The products will always include some sort of salt, as well as water, and the reation will always be exothermic, meaning energy is released.