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Changes in temperature and activation energy have opposite effects on reaction rate.
Changes in temperature and activation energy have opposite effects on reaction rate.
The reaction will not occur unless the activation energy is met.
as activation energy decreases, reaction will finish faster (length of reaction decreases)
As kinetic energy, and therefore temperature increases, the number of effective collisions which result in sufficient activation energy also increases, which is why reactions happen at a faster rate at higher temperatures.
The Arrhenius equation is: Ea = -RT ln(k/A) where Ea - activation energy R - universal gas constant ln - logarithm k - speed constant T - temperature in kelvins
yes. lowers it.
The activation energy is reduced.
The number of collisions with enough energy to react increases.
An enzyme is a catalyst that speeds up a chemical reaction. It functions by lowering the activation energy required for a reaction to occur, and by reducing the activation energy, the reaction speeds up.
Activation energy is the energy required by a reaction for the reaction to occur. The catalyst lowers the activation energy, making it easier for the reaction to happen.Improvement:A catalyst don't lowers the activation energy. A catalyst creates a alternative route (*) for the same reaction with a lower activation energy.* = as a result of the interaction of the reagents with the catalyst.
It lowers it, so the reaction is faster.