endothermic: or energy absorbing reactions
Energy is required to break bonds between atoms in reactant molecules, allowing them to rearrange into new products. This energy is called activation energy. Some reactions release energy, called exothermic reactions, while others absorb energy, called endothermic reactions. Overall, energy is essential for driving chemical reactions and determining whether they proceed or not.
Exothermic, meaning they release energy in the form of heat or light. These reactions tend to occur spontaneously because they result in a decrease in the overall energy of the system.
False. Not all chemical reactions require catalysis. Some reactions occur spontaneously, while others may require an initial input of energy in the form of activation energy. Catalysis is a process that lowers the activation energy required for a reaction to occur, but it is not necessary for all reactions.
Favorable chemical reactions are those that release energy, produce a decrease in entropy, or result in the formation of more stable products. These reactions typically proceed in the direction of equilibrium and are thermodynamically spontaneous. Examples include combustion reactions and exothermic reactions.
An 'exothermic' reaction gives of energy, and an 'endothermic' reaction absorbs energy.
Energy is required to break bonds between atoms in reactant molecules, allowing them to rearrange into new products. This energy is called activation energy. Some reactions release energy, called exothermic reactions, while others absorb energy, called endothermic reactions. Overall, energy is essential for driving chemical reactions and determining whether they proceed or not.
Exothermic, meaning they release energy in the form of heat or light. These reactions tend to occur spontaneously because they result in a decrease in the overall energy of the system.
False. Not all chemical reactions require catalysis. Some reactions occur spontaneously, while others may require an initial input of energy in the form of activation energy. Catalysis is a process that lowers the activation energy required for a reaction to occur, but it is not necessary for all reactions.
Favorable chemical reactions are those that release energy, produce a decrease in entropy, or result in the formation of more stable products. These reactions typically proceed in the direction of equilibrium and are thermodynamically spontaneous. Examples include combustion reactions and exothermic reactions.
These are not chemical reactions but thermonuclear reactions.
An 'exothermic' reaction gives of energy, and an 'endothermic' reaction absorbs energy.
No, chemical reactions can be endothermic or exothermic.
Spontaneous chemical reactions are those that release energy and result in a decrease in free energy. They typically involve exothermic reactions where the products are more stable than the reactants, leading to a natural tendency for the reaction to occur without the input of additional energy. Examples include combustion reactions and some types of oxidation-reduction reactions.
These are called exothermic reactions.
Chemical reactions occur spontaneously when the free energy of the product is less than the free energy of the reactants. Free energy is a combination of thermal energy (heat) and entropy. If thermal energy is absorbed during a reaction, there must be an exceptionally large increase in entropy to give a net reduction in free energy.
false
This is true. Energy is required to begin all reactions.