RATE OF REACTION / REACTION RATE
definition? don't go to wikipedia...
As a reaction progresses, the rate typically decreases over time. This is due to the depletion of reactants, which reduces their concentration and, consequently, the frequency of effective collisions between reactant molecules. Additionally, the formation of products can lead to changes in reaction conditions that further slow the rate. Eventually, the reaction may reach equilibrium, where the rates of the forward and reverse reactions are equal, and no net change occurs.
Because catalyst will reduce the activation energy of the reaction, thereby the speed of the reaction increases.
Yes, the reaction distances increases with speed while reaction time stays the same. for example the two-second rule.
A first-order reaction will never be completed because the reaction rate depends only on the concentration of one reactant. As the reaction progresses and the reactant is consumed, the concentration of the reactant decreases, causing the reaction rate to also decrease. This gradual decrease in reaction rate means that the reaction will continue indefinitely, given enough time.
The reactant concentrations decrease
The concentration of the reactants decreases.
The how much speed it takes for two substances to make one product. Many factors can affect this including the temperature, the surface area, the concentration, the catalyst and the pressure (only applies for gases)
The rate decreases as reactants are used up.
In general, and depending on the order of the reaction, the rate will decrease as the reaction progresses.
The reaction rate apex is the point of maximum reaction rate in a chemical reaction. It represents the fastest rate at which reactants are being converted into products. This point is often used to optimize reaction conditions for maximum yield or efficiency.
The concentration of the reactants decreases.
The relationship between potential energy and reaction progress is that potential energy changes as a reaction progresses. At the beginning of a reaction, potential energy is high as reactants are being converted into products. As the reaction progresses, potential energy decreases until it reaches a minimum at the point of maximum stability, known as the transition state.
There are fewer reactants left to collide.
The speed of a given chemical reaction is directly responsible for spontaneity of the reaction. The reaction force and effect is contingent upon the speed of the reaction. The faster the reaction, the more force will be produced.
Catalyst will reduce the activation energy of the reaction, thereby the speed of the reaction (or the rate of the reaction) increases.
As a reaction progresses, the rate typically decreases over time. This is due to the depletion of reactants, which reduces their concentration and, consequently, the frequency of effective collisions between reactant molecules. Additionally, the formation of products can lead to changes in reaction conditions that further slow the rate. Eventually, the reaction may reach equilibrium, where the rates of the forward and reverse reactions are equal, and no net change occurs.
Activation energy is lowered to speed up a chemical reaction.