A catalyst lowers the activation energy of a reaction, making it easier for the reactants to form products. It does not change the potential energy of the reactants or products, nor does it affect the overall heat of the reaction.
a catalyst lowers the activation energy for both the forward and reverse reaction. however, it does not change the potential energy of the reactants or products. it also does not affect the heat of reaction (delta h)
A catalyst lowers the energy of activation for a reaction by providing an alternative reaction pathway with lower activation energy. This allows the reactants to more easily overcome the energy barrier and proceed to form products at a faster rate.
Lowering the activation energy, Adding a cataylst
it is incorporated into the reactants
A catalyst lowers the activation energy of a reaction, making it easier for the reactants to form products. It does not change the potential energy of the reactants or products, nor does it affect the overall heat of the reaction.
a catalyst lowers the activation energy for both the forward and reverse reaction. however, it does not change the potential energy of the reactants or products. it also does not affect the heat of reaction (delta h)
A catalyst changes the path of reaction mechanism and decreases the activation energy required by the reactants.
A catalyst lowers the activation energy of a reaction.
The key factors that influence the rate of a chemical reaction are concentration of reactants, temperature, presence of a catalyst, surface area of reactants, and the nature of the reactants and products.
The difference between a homogeneous and a heterogeneous catalyst is that in a heterogeneous catalyst, it is in a different phase from the reactants. However, in a homogeneous catalyst, it is in the same phase as the reactants.
The factors that influence the activation energy of a chemical reaction include temperature, concentration of reactants, presence of a catalyst, and the nature of the reactants and their bonds.
A catalyst lowers the energy of activation for a reaction by providing an alternative reaction pathway with lower activation energy. This allows the reactants to more easily overcome the energy barrier and proceed to form products at a faster rate.
The correct answer is a simple one: The system is unaffected by a catalyst in a system in equilibrium.
In a combustion reaction between butane and oxygen, the products contain more energy than the reactants. This is because energy is released in the form of heat during the combustion process, increasing the total energy content of the products. The catalyst does not contribute to the overall energy content of the reaction.
Reactants are also known as substrates.
The heterogeneous catalyst is not mixed with the reactants.