I will pay for the following essay Chemical KInetics Chemistry. The essay is to be 6 pages with three to five sources, with in-text citations and a reference page.The theory states that when appropria

I will pay for the following essay Chemical KInetics Chemistry. The essay is to be 6 pages with three to five sources, with in-text citations and a reference page.

The theory states that when appropriate molecules of a reactant collide against each other, it is only a definite proportion of the collisions that result in a perceptible chemical change (Goldberger and Watson, 2004). These collisions are termed successful collisions, and possess activation energy. The idea of activation energy was introduced by Svante Arrhenius in 1889, and is the amount of energy needed to be gained by the reactant molecules to form the product. During the exact instant of collision, the pre-existing bonds are broken and new bonds formed. This results in the formation of the products of the reaction.

The higher the temperature the higher the rate at which its constituent particles move. This increased particular motion increases the chances of the particles colliding, resulting in more successful collisions that lead to bonds being broken and new ones forming, resulting in the formation of new products, and thereby increasing the reaction rate. This is proven in the graph above, which shows that the molecules that have higher kinetic energies resulting from high temperatures have higher reaction rates, since the increased motion between the molecules results in increased molecular collisions that raises the reaction rates.

Pressure has an effect on the rate of various chemical reactions, only involving gases. Raising it leads to a corresponding increase in the rate of the reaction. Raising or lowering the pressure of a reaction system involving liquids or solids leads to no change in the rate of the reaction.

For a specific amount of gas, to raise the pressure of the gas one would have to compress the gas so that it would be contained in a lesser volume. Doing so would mean the same amount of gas is found in a much smaller volume, resulting in a higher concentration. Since the gas particles are closer to each other, their random motions result in more frequent collisions. These