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What are 6 ways the number of effective collision in a chemical reaction can be controlled?
Wiki User
∙ 11y ago
- Increase concentration of the reactants
- Decrease concentration of the products
- Add a catalyst
- Increase the temperature
- Increase the pressure
- Stir
Of course... do the opposite of these things if you are trying to slow it down.
Wiki User
∙ 11y ago
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When will a collision lead to a chemical reaction?
When the collision is hard and fast enough. Increasing the kinetic energy will increase the likelihood of hard and fast collisions, which will ultimately increase the rate of the reaction. (This is called collision theory.)
Molecules involved in a chemical reaction must collide to react What is this concept called?
Collision Theroy
What is the effect of a catalyst on the required energy to achieve effective collisions?
catalyst decreases the activation energy of a chemical reaction, thereby increasing the effective collisions and hence the rate of the chemical reaction
According to collision theory what best explains how a catalyst increases the reaction rate for a chemical reaction?
A catalyst decreases the threshold energy for a chemical reaction. A catalyst decreases energy required for two particles to react. A catalyst lowers the amount of energy needed to reach the transition state.
What is a control in chemistry?
A controlled chemistry is authoritarian rule over science departments a controlled chemical reaction is when a chemical reaction can be ceased easily by either removing a reactant or changing conditions such as temperature or PH.
In the enzymatically controlled chemical reaction A B plus C the letter A stands for?
in the enzymatically controlled chemical reaction a to b plus c, the letter a stands for what?
When will a collision lead to a chemical reaction?
When the collision is hard and fast enough. Increasing the kinetic energy will increase the likelihood of hard and fast collisions, which will ultimately increase the rate of the reaction. (This is called collision theory.)
Molecules involved in a chemical reaction must collide to react What is this concept called?
Collision Theroy
In the enzymatically controlled chemical reaction A B C the A stands for what?
substrate
Cars and motorcycle engines are controlled by what chemical reaction?
This is the burning of the fuel.
What is the effect of a catalyst on the required energy to achieve effective collisions?
catalyst decreases the activation energy of a chemical reaction, thereby increasing the effective collisions and hence the rate of the chemical reaction
Why did Dalton say that a chemical reaction is a rearrangement of atoms?
because the llamas controlled his mind
According to collision theory increasing the concentration of the reactants in a chemical reaction increases?
A.the rate of collisions between two particles.
Why does heat speed up a chemical reaction?
It provides energy to overcome the activation energy.
According to collision theory what best explains how a catalyst increases the reaction rate for a chemical reaction?
A catalyst decreases the threshold energy for a chemical reaction. A catalyst decreases energy required for two particles to react. A catalyst lowers the amount of energy needed to reach the transition state.
Why does hot water increase the rate of reaction?
In order for a chemical reaction to occur, there must be a certain amount of energy to break, and then reform chemical bonds. The collision of particles must also occur at the correct angle for a chemical reaction to occur. Heat is essentially the energy a substance has, so the higher the temperature, the higher the energy of of the particles. If the particles have a higher energy, they move around faster, therefore increasing the probability of a successful collision. The energy (or velocity) of particles is also higher, therefore creating higher chance that there is enough energy in the chemical collision for the reaction to occur.
Nearly every chemical reaction in the body is activated - assisted - and controlled by?
Enzymes of literally all 'descriptions'.
