The activation energy of a chemical reaction is analogous to the "hump" you have to overcome in order to get out of bed. Even energy-releasing (exergonic) processes require some energy input to get started before proceeding with their energy-releasing phases. The activation energy, abbreviated AE, is the initial energy input that is later paid back as the reaction progresses. Why would a negative G energy-releasing reaction require energy to proceed? To understand this, we must first examine what happens to reactant molecules during a chemical reaction. In order for the reaction to occur, some or all of the chemical bonds in the reactants must be broken, allowing new bonds, those of the reactants, to form.
To allow the bonds to break, the molecule must be twisted (deformed or bent) into an unstable condition known as the transition state. The transition state is a high-energy state, and some energy – the activation energy – must be provided to the molecule in order for it to reach there. Because the transition state is unstable, reactant molecules do not stay there for long before moving on to the next phase of the chemical process.
In general, the transition state of a reaction is always at a higher energy level than the reactants or products, and hence has a positive value — regardless of whether the process is overall endergonic or exergonic. If the reaction were to proceed in the reverse direction (endergonic), the transition state would remain the same, but the activation energy would be larger. This is because the product molecules are lower-energy and would thus need more energy added to reach the transition state at the top of the reaction “hill.”
Heat is often the source of activation energy, with reactant molecules receiving thermal energy from their surroundings. This heat energy accelerates the velocity of the reactant molecules, increasing the frequency and force of their collisions, and it also jostles the atoms and bonds inside the individual molecules, raising the likelihood of bonds breaking. Once a reactant molecule has absorbed enough energy to reach the transition state, it may proceed with the reaction.
Chains of enzyme reactions in a cell that regulate enzyme activity and energy flow are _____.
Answers & Comments
ACTIVATION ENERGY
Answer:
The activation energy of a chemical reaction is analogous to the "hump" you have to overcome in order to get out of bed. Even energy-releasing (exergonic) processes require some energy input to get started before proceeding with their energy-releasing phases. The activation energy, abbreviated AE, is the initial energy input that is later paid back as the reaction progresses. Why would a negative G energy-releasing reaction require energy to proceed? To understand this, we must first examine what happens to reactant molecules during a chemical reaction. In order for the reaction to occur, some or all of the chemical bonds in the reactants must be broken, allowing new bonds, those of the reactants, to form.
To allow the bonds to break, the molecule must be twisted (deformed or bent) into an unstable condition known as the transition state. The transition state is a high-energy state, and some energy – the activation energy – must be provided to the molecule in order for it to reach there. Because the transition state is unstable, reactant molecules do not stay there for long before moving on to the next phase of the chemical process.
In general, the transition state of a reaction is always at a higher energy level than the reactants or products, and hence has a positive value — regardless of whether the process is overall endergonic or exergonic. If the reaction were to proceed in the reverse direction (endergonic), the transition state would remain the same, but the activation energy would be larger. This is because the product molecules are lower-energy and would thus need more energy added to reach the transition state at the top of the reaction “hill.”
Heat is often the source of activation energy, with reactant molecules receiving thermal energy from their surroundings. This heat energy accelerates the velocity of the reactant molecules, increasing the frequency and force of their collisions, and it also jostles the atoms and bonds inside the individual molecules, raising the likelihood of bonds breaking. Once a reactant molecule has absorbed enough energy to reach the transition state, it may proceed with the reaction.
Chains of enzyme reactions in a cell that regulate enzyme activity and energy flow are _____.
brainly.ph/question/1541763
#LETSSTUDY