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What does an enzyme do to the activation energy needed to start a chemical reaction?
Enzymes are catalysts, they reduce the activation energy.
Is it true that catalysts increase the activation energy needed to start a chemical reaction?
Catalysts actually lower the activation energy needed to start a chemical reaction. This makes the reaction happen more easily.
What it the term used to describe the energy needed to get a reaction started?
The energy needed to get a reaction started is called activation energy.
What increases the rate of a reaction by lowering the activation energy?
A catalyst can increase the rate of a reaction by lowering the activation energy needed for the reaction to occur. Catalysts provide an alternative reaction pathway with a lower activation energy, allowing the reaction to happen more quickly.
What does the activation energy for a reaction represent?
Activation energy is the amount of energy needed to start a reaction.
What energy is the energy needed to start a reaction?
Activation Energy.
The energy that is needed to get a reaction started?
activation energy
What activation energy is needed for a chemical reaction is decreased by?
The activation energy is decreased by a catalyst.
A reaction in which it seems no activation energy is needed?
a spontaneous reaction
What effect does an enzyme have on a activation energy needed to start a reaction?
In chemistry it is called a catalyst. Enzymes decrease the activation energy needed to start a reaction.
What is the minimum amount of energy needed to start a chemical reaction?
The minimum amount of energy needed to start a chemical reaction is called the activation energy. It is the energy required to break the bonds in reactant molecules and initiate the reaction. Once this energy barrier is overcome, the reaction proceeds without additional energy input.
The smallest amount of energy needed to start a chemical reaction is called?
Technically, it isn't "heat" that makes a chemical reaction happen. "Heat" is merely the flow of energy from one place to another. It is the energy itself that causes a reaction to occur. As an increase in temperature occurs, there is an increase in the energy in a group of molecules by making them mover around faster and bum into each other more. This energy is called "Activation energy", and is defined as the amount of energy required to make the reaction start and carry on spontaneously. Higher activation energy implies that the reactants need more energy to start than a reaction with a lower activation energy. With that being said, activation energy is the answer
