Chemists call the energy needed to get a reaction called activation energy. Activation energy was introduced in 1889 by the Swedish scientist Svante Arrhenius.
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Activation Energy :)
Activation energy
It varies with the differences in chemical reactions
Generally, yes. Unless the product of the reaction should be ammonia for example, where a decreased temperature is needed. A catalyst from the transition metals will speed up a reaction too, for example a nickel catalyst in the process of the hydrogenation of margerine as it lowers the activation energy needed for the reaction to start. Increased pressure will also speed up the reaction, no matter what reaction is occurring.
To produce water? Exothermic and very much so.Take a mixture, spark it and it will burn or explode. Heat energy is given off far in excess of whatever energy was needed to start the reaction.
For a reaction between oxygen molecule and hydrogen molecule to take place the bond between the two oxygen atom in O2 and the two hydrogen atom in H2 is required to be breaked. For this process a high temperature is needed which is not possible at room temperature. Since no bond breaks to make an reacting atom, the reaction does not takes place at room temperature
there will be a chemical reaction called combustion. potassium permanganate as the oxidant and oil obviously as fuel if the two were mixed they needed to release energy in form of heat.
The energy needed to start a chemical reaction is called the activation energy :)
activation energy
Potential energy
The energy needed to get a reaction started is called activation energy.
Activation energy
Energy needed to get a reaction started....
ACTIVATION ENERGY IS THE ENERGY WHICH IS REQUIRED FOR INITIALIZING OF ANY TYPE OF REACTION.
activation energy
Energy
Activation energy is the amount of energy needed to start a reaction.
The energy needed to statr a chemical reaction is the 'Activation Energy' , which is given the symbol (Ea).
The greater the temperature, the faster the rate of reaction. This is due to the fact that increasing temperature increases the activation energy, which is the amount of energy needed to get a reaction started.