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A chemical reaction whose products recombine to produce reactants is a?
reversible reaction. It is a reaction that can proceed in both the forward and reverse directions, creating a dynamic equilibrium where reactants and products are constantly interconverting.
Is this statement true Catalysts make chemical reactions proceed faster by reducing the activation energy?
yes!. the way the reaction gets faster is because the catalyst absorbs the reactant particles on its surface and weakens their bonds. Reactants particles colliding with weaker bonds actually overcomes the activation energy faster as it is now lower. The only thing a catalyst changes in a chemical reaction is the activation energy, keeping in mind that the catalyst increases the rate of reaction in both forward and backward reaction.
The direction in whick a reversible reaction will proceed can be predicted from the laws of?
Thermodynamics. Specifically, the reaction will proceed in the direction that leads to a decrease in Gibbs free energy. If the Gibbs free energy change of the reaction is negative, it is more likely to proceed in the forward direction.
What parameter involved in a chemical reaction will change with the addition of a catalyst?
The rate of a chemical reaction will change in the presence of a catalyst, unless the reaction is already at equilibrium.
What is a substance that enables a chemical reaction to proceed under different conditions?
A catalyst is a substance that enables a chemical reaction to proceed under different conditions. It lowers the activation energy required for the reaction to occur, allowing it to happen more quickly or at a lower temperature or pressure. The catalyst itself remains unchanged in the reaction and can be reused multiple times.
What does a double arrow mean in a chemical reaction?
A double arrow in a chemical reaction indicates that the reaction is reversible, meaning it can proceed in both the forward and reverse directions. The reaction can reach an equilibrium where the forward and reverse reactions occur at the same rate.
What is the significance of delta G prime in determining the spontaneity of a biochemical reaction?
The significance of delta G prime in determining the spontaneity of a biochemical reaction lies in its ability to indicate whether the reaction will proceed forward or backward. A negative delta G prime value indicates that the reaction is spontaneous and will proceed forward, while a positive value indicates that the reaction is non-spontaneous and will not proceed without external energy input.
What is the definition of an irreversible reaction and how does it differ from a reversible reaction?
An irreversible reaction is a chemical reaction that proceeds in one direction only, meaning it cannot be easily reversed. In contrast, a reversible reaction is a chemical reaction that can proceed in both forward and reverse directions, reaching a state of equilibrium where the rates of the forward and reverse reactions are equal.
What is the significance of equilibrium arrows in chemical reactions?
Equilibrium arrows in chemical reactions indicate that the reaction can proceed in both forward and reverse directions. This signifies that the reaction has reached a balance point where the rates of the forward and reverse reactions are equal, leading to a stable state known as chemical equilibrium.
A chemical reaction whose products recombine to produce reactants is a?
reversible reaction. It is a reaction that can proceed in both the forward and reverse directions, creating a dynamic equilibrium where reactants and products are constantly interconverting.
A reaction that can be made to go either direction from reactants to products or from products to reactants is called an?
equilibrium reaction. It represents a balanced state where the rate of the forward reaction is equal to the rate of the reverse reaction, allowing the reaction to proceed in both directions.
When is activation energy the same for forward and reverse reactions?
Activation energy is the same for the forward and reverse reactions at equilibrium, where the rates of the forward and reverse reactions are equal. At this point, the activation energy represents the energy barrier that must be overcome in either direction to proceed with the reaction.
What makes a leaving group the best choice in a chemical reaction?
A leaving group is the best choice in a chemical reaction because it can easily detach from the molecule, allowing the reaction to proceed efficiently. The leaving group's ability to stabilize negative charge and leave the molecule helps in forming new bonds and driving the reaction forward.
Is this statement true Catalysts make chemical reactions proceed faster by reducing the activation energy?
yes!. the way the reaction gets faster is because the catalyst absorbs the reactant particles on its surface and weakens their bonds. Reactants particles colliding with weaker bonds actually overcomes the activation energy faster as it is now lower. The only thing a catalyst changes in a chemical reaction is the activation energy, keeping in mind that the catalyst increases the rate of reaction in both forward and backward reaction.
Which type of chemical reaction needs to absorb energy to proceed?
endothermic
What is it endothermic?
It is a chemical reaction which requires heat - possibly from the environment - to proceed.
What is equilibrium-limited reactions?
Equilibrium-limited reactions refer to chemical reactions that are limited by the establishment of an equilibrium between reactants and products. This means that the reaction may not proceed to completion because the system reaches a dynamic equilibrium where the rate of the forward reaction is equal to the rate of the reverse reaction.
