In order for energy to be conserved during a chemical reaction where the reactants contain 385 kJ of chemical energy and the products contain 366 kJ, the difference of 19 kJ must be released to the surroundings. This energy is typically lost as heat, light, or sound, indicating that the reaction is exothermic. The law of conservation of energy states that energy cannot be created or destroyed, only transformed, so the released energy accounts for the discrepancy between the energy of reactants and products.
Gibbs free energy (G) represents the maximum reversible work that can be performed by a system at constant temperature and pressure. In a spontaneous reaction, the system tends to move towards a state of lower energy and increased entropy, which corresponds to a decrease in Gibbs free energy. A negative change in Gibbs free energy (ΔG < 0) indicates that the reaction can occur spontaneously, driving the system towards equilibrium. Therefore, for a reaction to be spontaneous, Gibbs free energy must decrease.
For an atom to lose an electron, it must undergo the process of ionization where it gains enough energy to overcome the attraction of the nucleus and the electron is released. This can happen through various means such as exposure to high-energy radiation or collisions with other particles.
glycolysis, krebs, electron transport chain, alcoholic fermentation, and lactic acid fermentation
for a state change to happen it must lose or gain or loose kinetic energy
There must be an input of energy from ATP.
you must except the choice of freedom to be free.
you must except the choice of freedom to be free.
Fission
Its energy level must be increased.
Digestion is necessary because for energy from the food to be released and carried into the cells in our body the food must be broken down into soluble molecules for it to diffuse into the cells. Then energy is released during respiration.
In order for energy to be conserved during a chemical reaction where the reactants contain 385 kJ of chemical energy and the products contain 366 kJ, the difference of 19 kJ must be released to the surroundings. This energy is typically lost as heat, light, or sound, indicating that the reaction is exothermic. The law of conservation of energy states that energy cannot be created or destroyed, only transformed, so the released energy accounts for the discrepancy between the energy of reactants and products.
Gibbs free energy (G) represents the maximum reversible work that can be performed by a system at constant temperature and pressure. In a spontaneous reaction, the system tends to move towards a state of lower energy and increased entropy, which corresponds to a decrease in Gibbs free energy. A negative change in Gibbs free energy (ΔG < 0) indicates that the reaction can occur spontaneously, driving the system towards equilibrium. Therefore, for a reaction to be spontaneous, Gibbs free energy must decrease.
For an atom to lose an electron, it must undergo the process of ionization where it gains enough energy to overcome the attraction of the nucleus and the electron is released. This can happen through various means such as exposure to high-energy radiation or collisions with other particles.
In a chemical reaction, enthalpy, entropy, and free energy are related. Enthalpy is the heat energy exchanged during a reaction, entropy is the measure of disorder or randomness, and free energy is the energy available to do work. The relationship between these three factors is described by the Gibbs free energy equation: G H - TS, where G is the change in free energy, H is the change in enthalpy, S is the change in entropy, and T is the temperature in Kelvin. This equation shows that for a reaction to be spontaneous, the change in free energy must be negative, meaning that the enthalpy change and entropy change must work together in the right direction.
For energy to be conserved, it must neither be created nor destroyed but only transferred or converted from one form to another. This principle is known as the Law of Conservation of Energy. Energy can change from potential to kinetic, thermal, or other forms, but the total amount of energy must remain constant in a closed system.
For the potential energy of fossil fuels to change into other forms of energy, combustion must take place. In this process, heat energy is released, which can be transformed into other forms of energy like electrical energy in power plants or mechanical energy in engines.