Answer:
1.A catalyst speeds up a chemical reaction, without being consumed by the reaction. It increases the reaction rate by lowering the activation energy for a reaction. ... Remember that with a catalyst, the average kinetic energy of the molecules remains the same but the required energy decreases.
2.Increasing the concentration of one or more reactants will often increase the rate of reaction. This occurs because a higher concentration of a reactant will lead to more collisions of that reactant in a specific time period.
3.An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision.
1. 2KC102KCI + 302-Decomposition having one reactant decomposed forming two or more product.
2. 2Na + C122Naci-Synthesis reaction having two or more reactant forming one product.
3. 2NH3-N2 + 3H2-Decomposition having one reactant decomposed forming two or more product.
4. 4Na + 02- 2Na2O-Synthesis reactions having two or more reactant forming one product.
5. H2 + Brz-2HBr-Synthesis reaction having two or more reactant forming one
