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The specific protein molecule in a cell acts as a catalyst, facilitating the chemical reaction to occur more efficiently or at a faster rate. The protein molecule binds with the reactants, stabilizes the transition state, and lowers the activation energy required for the reaction to proceed. Without the presence of this protein molecule, the reaction may occur, but at a significantly slower rate.
its metabolism
Enzymes reduce the activation energy required for a chemical reaction to occur by stabilizing the transition state of the reaction. This allows the reaction to proceed more rapidly than if it were to occur without the enzyme present.
Activation energy. The kinetic energy from collisions between particles is used to reach the transition state
A positive cell potential indicates that the redox reaction is spontaneous under standard conditions. This means that the reactants have a higher free energy than the products, leading to a favorable reaction that can occur without external energy input. Additionally, it suggests that the reduction half-reaction has a greater tendency to gain electrons compared to the oxidation half-reaction losing them.
The specific protein molecule in a cell acts as a catalyst, facilitating the chemical reaction to occur more efficiently or at a faster rate. The protein molecule binds with the reactants, stabilizes the transition state, and lowers the activation energy required for the reaction to proceed. Without the presence of this protein molecule, the reaction may occur, but at a significantly slower rate.
it is the place for the biochemical reaction to occur.
The reaction will occur naturally
its metabolism
The reaction is spontaneous.
Enzymes reduce the activation energy required for a chemical reaction to occur by stabilizing the transition state of the reaction. This allows the reaction to proceed more rapidly than if it were to occur without the enzyme present.
The energy barrier is the minimum amount of energy required for a chemical reaction to occur. It represents the energy difference between the reactants and the transition state of the reaction. Overcoming this barrier allows the reaction to proceed.
Activation energy. The kinetic energy from collisions between particles is used to reach the transition state
The term that refers to the difference between the energy of the transition state and the energy of the reactants is activation energy. It represents the energy threshold that must be overcome for a chemical reaction to occur.
The presence of a catalyst can speed up a reaction by providing an alternate pathway with lower activation energy, allowing the reaction to occur more quickly. Catalysts work by facilitating the formation of transition states and by stabilizing reaction intermediates.
Enzymes alter the equilibrium of a chemical reaction by lowering the activation energy required for the reaction to occur, thus speeding up the rate at which the reaction reaches equilibrium. This is achieved by stabilizing the transition state of the reaction, making it easier for the reactants to form products.
Enzymes lower the activation energy required for a reaction to occur by stabilizing the transition state of the reaction, making it easier for the reaction to proceed. This lowering of activation energy allows the reaction to happen more quickly and efficiently. Enzymes achieve this by binding to the substrates and facilitating the formation of the transition state.