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What is term used for the height of the energy barrier the reactants must overcome in order to form products in a reaction?
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What type of energy starts a reaction to overcome an energy barrier between reactants and products?
Activation energy
Why does a catalyst cause a reaction to proceed faster?
It decreases the activation energy, or the energy barrier the reactants must go through to form products. This is the same thing as the energy of the transition state. By decreasing the activation energy necessary for the reaction to occur, more reactants are able to form products since not as much energy is needed. See the Web Links to the left of this answer for more information.
What ar five factors that affect the rate of a chemical reaction?
The rate of a Chemical reaction is affected by a number of factors, here are the commonly taught "Five factors of reaction rates":1-Nature of the Reactants (Based on the atomic structure, ie. the stability of the reactants vs. the stability of the proposed products)2-Ability of the Reactants to meet ( the state of the reactants: gases and liquids are more likely to react, AND the Surface area: powders have a greater surface area and therefore react quickly)3- Concentration of the Reactants (the higher the concentration, the more likely the reactants are able to meet and react, thus increasing the reaction rate)4- Temperature (the higher the temperature of the system, the faster the particles are moving (Kinetic Molecular Theory) and the faster they will collide, thus increasing the reaction rate)5- Presence of Catalysts (Catalysts increase the reaction rate by overcoming the activation energy. They work by decreasing the reaction barrier of the Rate determining step, which is the slowest step of a chemical reaction)Of course, there are other factors which affect the reaction rate of a given system, but these are the 5 commonly cited ones they teach you in high school. If you're interested, I'd suggest reading about Collision Theory and Transition State Theory.huifhyiusdyhtrfu0er8ut09o79retgvkghvvyhogiyhvoufysyo8yiySurface areaconcentrationcatalyststemperatureinhibitors
Is activation energy for thermal and photochemical reactions same?
The definition of the activation energy is exactly the same -- the thermodynamic energy barrier that the reactant must pass over to convert to products. The difference between a thermal and a photochemical reaction is only where the reactants get the energy to get over this barrier. In a thermal reaction, that energy is given by the temperature, and is carried in excited rotational modes, higher kinetic energies and if hot enough, excited vibrational states. In a photochemical reaction, the activation energy is provided by photons, usually in the form of electronic excited states, but could also be vibrational or rotational. The concept of the activation barrier is identical in both cases.
Explain why an investment of activation energy is necessary to initiate a spontaneous reaction?
haha...no idea. I have the same question...... But after reading my text, I'm pretty sure its to do with the fact that there is an energy barrier between the reactant and products that must be overcome in order for the reaction to proceed, which is what activation energy basically is, the amount of energy needed to jumpstart the process. ! I'm studying for Finals too!
What type of energy starts a reaction to overcome an energy barrier between reactants and products?
Activation energy
Reactants capable of interacting to form products in a chemical reaction must first overcome a thermodynamic barrier known as the reaction's?
activation energy
What reactants are capable of interacting to form products in a chemical reaction that must first overcome a thermodynamic barrier?
Fast moving reactant molecules or basically reactant molecules with a lot of kinetic energy.
How does a chemical reaction starts?
A reaction occurs when 2 particles collide with sufficient energy to overcome the activation barrier and then react.
What term is used to describe the minimum amount of energy required in order for a reaction to proceed?
This energy is called "energy of activation", it is used to overcame the energy barrier between reactants and products.
Activation energy barriers?
The activation energy is the amount of energy needed to start a reaction. If the reactants have less than that amount the reaction will not occur. In this way it acts as a barrier that prevents a reaction unless there is enough energy to break it.
Why does a catalyst cause a reaction to proceed faster?
It decreases the activation energy, or the energy barrier the reactants must go through to form products. This is the same thing as the energy of the transition state. By decreasing the activation energy necessary for the reaction to occur, more reactants are able to form products since not as much energy is needed. See the Web Links to the left of this answer for more information.
Why is the activation energy pictured as a hill in two diagrams?
The activation energy diagram is drawn as a hill because there is a large amount of energy needed to form the unstable transition state (viewed as the upward slope on the diagram). The difference between this peak energy and the rectants' energy is the activation energy. When this state decomposes in to more stable products (which are more stable than the reactants), the energy of the molecules is lower, thus the downward slope after the peak. ----------------------------- Activation energy is the energy at the potential barrier between the two fields with low energy (at left and at right) representing the sum of energies of reactants and products; the reaction is possible if the activation energy can exceed this barrier. And in a graphic this is the pic of a hill.
What must happen to reactant particles for a reaction to take place?
In order for two molecules to react they must: 1) Have sufficient energy to overcome whatever kinetic barrier exists to form a product in a realistic time period. We call this the activation energy. 2) Form a product which is at a lower total energy state than the two initial molecules.
What ar five factors that affect the rate of a chemical reaction?
The rate of a Chemical reaction is affected by a number of factors, here are the commonly taught "Five factors of reaction rates":1-Nature of the Reactants (Based on the atomic structure, ie. the stability of the reactants vs. the stability of the proposed products)2-Ability of the Reactants to meet ( the state of the reactants: gases and liquids are more likely to react, AND the Surface area: powders have a greater surface area and therefore react quickly)3- Concentration of the Reactants (the higher the concentration, the more likely the reactants are able to meet and react, thus increasing the reaction rate)4- Temperature (the higher the temperature of the system, the faster the particles are moving (Kinetic Molecular Theory) and the faster they will collide, thus increasing the reaction rate)5- Presence of Catalysts (Catalysts increase the reaction rate by overcoming the activation energy. They work by decreasing the reaction barrier of the Rate determining step, which is the slowest step of a chemical reaction)Of course, there are other factors which affect the reaction rate of a given system, but these are the 5 commonly cited ones they teach you in high school. If you're interested, I'd suggest reading about Collision Theory and Transition State Theory.huifhyiusdyhtrfu0er8ut09o79retgvkghvvyhogiyhvoufysyo8yiySurface areaconcentrationcatalyststemperatureinhibitors
How do you overcome lack of feedback as a barrier to communication?
we overcome lack of feedback by repeating the message
Is activation energy for thermal and photochemical reactions same?
The definition of the activation energy is exactly the same -- the thermodynamic energy barrier that the reactant must pass over to convert to products. The difference between a thermal and a photochemical reaction is only where the reactants get the energy to get over this barrier. In a thermal reaction, that energy is given by the temperature, and is carried in excited rotational modes, higher kinetic energies and if hot enough, excited vibrational states. In a photochemical reaction, the activation energy is provided by photons, usually in the form of electronic excited states, but could also be vibrational or rotational. The concept of the activation barrier is identical in both cases.
