The "certain amount of energy" you're referring to is typically called "activation energy."
To explain why a chemical reaction would "need" to have an activation energy, you could use an example of a living organism, for example a human. There's reactions involved in your metabolism that convert the food you eat into energy to allow you to move your arms and legs, to breathe in and out, or even something so important as keeping your heart beating. If these reactions didn't have an activation energy, you could expect yourself to literally "burn up" as any food you eat would be uncontrollably converted into energy.
There's two main controls to any chemical process: mass transfer control and kinetic control. Mass transfer control comes into play with things like if you didn't chew your food, it would be more difficult for your stomach/intestines to break down and absorb the food, so the reactions to metabolise your food are slowed. Kinetic control is related to activation energy, as described above, where given that all the reactants are present for a given reaction, e.g. metabolizing your food, the reaction needs to happen at a certain rate to sustain life.
As a fun connection, reaction kinetics can be related to the temperature of the environment in which the reaction takes place, which gives you an idea of why it's so important for your body to stay around 98.6 degrees Fahrenheit. That crappy feeling you get when you have a fever comes from all the reactions in your body that depend on a certain reaction rate being upset by the increase in temperature.
Chemical reactions that absorb energy need an input of energy in the form of heat, light, or electricity to overcome the activation energy barrier and initiate the reaction. This added energy allows the reactant molecules to surpass their energy threshold and transition into a higher-energy state, leading to the formation of products.
Chemical reactions that release energy often occur spontaneously because they lead to a decrease in the overall energy of the system. Exothermic reactions, which release heat energy, are usually spontaneous because they increase the randomness or entropy of the system, following the second law of thermodynamics. This decrease in energy and increase in entropy drive the reaction to proceed without the need for external energy input.
Chemical reactions are based on the interactions between atoms and molecules, specifically the rearrangement of chemical bonds. These interactions involve breaking existing bonds and forming new ones, resulting in the transformation of reactants into products with different chemical properties.
An exothermic reaction releases energy, usually to the surroundings. There is a net loss of energy from the reactants. However, exothermic reactions also need a little energy to get started, but this is less than the eventual amount given out. An endothermic reaction takes in energy, also usually from the surroundings. There is a net gain of energy into the reactions. Again, a little energy is lost, but this is hardly anything compared to the amount taken in.
Reactions in the body need a certain amount of energy, called activation energy. Most reactions don't take place because this activation energy is too high. The enzyme bonds to the molecule which diminguishes the activation energy, so the reaction can take place. These enzymes de-bond from the new formed molecule afterwards.
All chemical reactions need a certain amount of activation energy to get started.
Candle and all Chemical reactions
Candle and all Chemical reactions
Chemical reactions in living organisms require a source of energy to start. This energy is typically obtained from molecules such as ATP. Additionally, enzymes play a critical role in catalyzing these reactions by lowering the activation energy required for the reaction to occur.
yes they all need more or less start up energy
Chemical reactions that absorb energy need an input of energy in the form of heat, light, or electricity to overcome the activation energy barrier and initiate the reaction. This added energy allows the reactant molecules to surpass their energy threshold and transition into a higher-energy state, leading to the formation of products.
Light dependent reactions are reactions the capture light energy and convert it into chemical energy(ATP). It occur in the chloroplast of plant cells Light independent reactions are reactions capture energy and use it to produce food . It does not need sunlight
No, not all chemical reactions require heat to start. Some reactions can occur at room temperature or even at low temperatures. Heat is often used to speed up reactions or provide enough energy to overcome the activation energy barrier.
I wonder about a lot of things, yes.
Heat is a form of energy. All chemical reactions need to have an energy of some sort. Fire is a chemical reaction. You can figure out the rest. na sooooooo!
Chemical reactions that release energy often occur spontaneously because they lead to a decrease in the overall energy of the system. Exothermic reactions, which release heat energy, are usually spontaneous because they increase the randomness or entropy of the system, following the second law of thermodynamics. This decrease in energy and increase in entropy drive the reaction to proceed without the need for external energy input.
Endothermic reactions need heat.