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Why rate constant decrease when activation increase in arrhenius equation?
The rate constant in the Arrhenius equation decreases as the activation energy increases because a higher activation energy means that fewer molecules possess the required energy to overcome the energy barrier and react. This results in a lower frequency of successful collisions between reacting molecules, leading to a decrease in the rate constant.
What happens when you add a catalyst to the rate constant k?
Adding a catalyst typically increases the rate constant k by providing an alternative reaction pathway with lower activation energy. This allows the reactants to more easily convert to products, resulting in a faster reaction rate.
What happens to the kinetic energy when you increase the speed but keep the mass constant?
When you increase the speed while keeping mass constant, the kinetic energy increases. Kinetic energy is directly proportional to the square of the velocity, so as speed increases, kinetic energy increases even more rapidly.
What happens to the energy of a particle if the mass is constant and the speed increases?
The kinetic energy of the particle increases as the speed increases, following the equation ( KE = \frac{1}{2} mv^2 ) where ( KE ) is the kinetic energy, ( m ) is the mass of the particle, and ( v ) is the speed of the particle. The energy of the particle is converted to kinetic energy as its speed increases.
Is it true that when an enzyme promotes a chemical reaction by lowering the activation energy it only affects the rate of the reaction?
No, enzymes do not alter the equilibrium of a reaction. They accelerate both the forward and backward reactions equally, which keeps the equilibrium constant unchanged. The activation energy reduction increases the rate of the reaction but does not affect the overall equilibrium.
What happens to the rate constant as activation energy increase?
The rate constant decreases.
Will affect the rate of the constant according to the Arrhenius equation changing which factors?
The rate constant in the Arrhenius equation is impacted by temperature and activation energy. Increasing temperature generally increases the rate constant as molecules have more energy to overcome activation barriers. Similarly, lowering the activation energy required can lead to a higher rate constant.
What happens to the rate constant as energy increases?
The rate constant decreases.
Why rate constant decrease when activation increase in arrhenius equation?
The rate constant in the Arrhenius equation decreases as the activation energy increases because a higher activation energy means that fewer molecules possess the required energy to overcome the energy barrier and react. This results in a lower frequency of successful collisions between reacting molecules, leading to a decrease in the rate constant.
What happens to the reaction rate if the activation energy gets smaller?
If the activation energy decreases, the reaction rate typically increases because a lower activation energy makes it easier for the reactant molecules to overcome the energy barrier and form products. This allows the reaction to proceed more rapidly at a given temperature.
What happens when you add a catalyst to the rate constant k?
Adding a catalyst typically increases the rate constant k by providing an alternative reaction pathway with lower activation energy. This allows the reactants to more easily convert to products, resulting in a faster reaction rate.
How does activation energy affect chemical reactions?
Activation energy is the minimum amount of energy required to initiate a chemical reaction. Higher activation energy means the reaction is less likely to occur, whereas lower activation energy makes the reaction proceed more easily. By overcoming the activation energy barrier, molecules can collide and react to form new products.
What happens to the kinetic energy when you increase the speed but keep the mass constant?
When you increase the speed while keeping mass constant, the kinetic energy increases. Kinetic energy is directly proportional to the square of the velocity, so as speed increases, kinetic energy increases even more rapidly.
What effects the rate constant of a reaction?
The temperature of the system
Material that increases the rate of a reaction by lowering the activation energy?
A catalyst
If the activation energy is increased what happens to the number of effective collisions?
If the activation energy is increased, the number of effective collisions will decrease because fewer collisions will possess the required energy to overcome the higher activation energy barrier. This can slow down the rate of reaction as fewer collisions are successful in forming products.
According to the Arrhenius equation changing which factors will affect the rate constant?
The factors that can affect the rate constant in the Arrhenius equation are temperature and activation energy. Increasing the temperature will increase the rate constant, as reactions occur more rapidly at higher temperatures. Similarly, changing the activation energy required for the reaction will also impact the rate constant.
