A greater the surface area will cause the reaction will proceed faster because there are more available sites where another reagent or catalyst can "attack" the reactant.
Unlike reactants, catalysts are not used up during a reaction. They merely speed up the reaction (or allow it to proceed).
If you continuously add reactants even after the reaction has attained the equilibrium then according to Le Chatelier's principle, the reaction will again proceed in forward direction in order to neutralise the reactants and once again the attain the state of equilibrium.
In a reversible reaction, the reactants and products become to a dynamic equilibrium after some time. after gaining this equilibrium, when more reactants are added the equilibrium breaks. So according to the Le Chetelier principle, the reaction will proceed until the equilibrium is gained.
it dependes upon the initial ratio of molar concentration of products to reactants higher the ratio reaction will proceed in the reverse direction and vice versa
As a chemical reaction proceed the concentration of the reactants keep on decreasing while those of the products keep on increasing how ever the rate of the reaction is also found to decrease this show that the rate of the reaction is directly related to the concentration of reactants
The concentration of one or more of the products is small, the reaction will not proceed very far to the right, and the reaction will generally form more reactants than products.
The concentration of one or more of the products is small, the reaction will not proceed very far to the right, and the reaction will generally form more reactants than products.
When reactants are joined by a catalyst, they no longer have to collide with much energy to react. Thus, with the catalyst present the reaction can proceed at very low temperatures.
The powdered form of a solid reactant has an aggregate surface area that is many times greater than the solid blockfrom which it came. This makes any reaction proceed faster and more efficiently, usually resulting in enhanced yield as well.
The reaction happens by itself.
Changing the temperature of the reaction can speed it up by increasing molecular collisions and kinetic energy. Adding a catalyst can speed up a reaction by lowering the activation energy required for the reaction to proceed. Increasing the concentration of reactants can speed up a reaction by providing more reactant molecules to collide and react. Changing the surface area of solid reactants can speed up a reaction by exposing more reactant surface area for collisions to occur. Adjusting the pH of the reaction environment can speed up or slow down a reaction by affecting the ionization state of reactants and the reaction rate.
An exergonic reaction