was about, by doing four different experiments. In part I “Effect of Particle Size on Reaction Rate”, that lab mostly about surface area with Zn+2HCl ZCl 2 + H 2 and CaCO 3 + HCl CaCl2 + H 2 CO 3 . Breaking down a substance, in this case it would be are powdered zinc is one of the ways to increase the rate of reaction. But, it was strange, in Table I., the powdered did not have much of a reaction as the solid zinc did. The solid zinc piece began to dissolve and started forming bubbles. For part II. “Effect of Temperature”, this experiment was about how if you were to manipulate the change in temperature then it will affect the rate of reaction of the Alka Seltzer. Increasing the average kinetic energy of the particles is what causes a fast reaction rate to occur. Also,
Factors Affecting Reaction Rates Brianna Collier March 30, 2015 April 8, 2015 8 reacting particles collide more frequently at a higher temperatures. For example, in Table II., the cold water temperature sat at about 19.9degrees Celsius and the completion time was about 1:03:51 while the warm water temperature was at 71.5 degrees Celsius and the completion time was about 0:15:15. And, being that the room temperature water was at 25.7 degrees Celsius the completion time for that was still higher than the cold water. In part III. “Effect of Concentration”, this experiment focused on if the concentration of HCl were to be increased it then would speed up the reaction rate of the zinc piece. One of the key principles in the collision theory is that particles must collide to react. The number of particles in a reaction makes a difference in the rate of the reaction. For example, in table III, the molarity of HCl was 6M and the completion time was 10:07 being the first zinc piece to completely break apart. While the other two had a much longer time to complete. For the 3M its completion time was estimated to 4o minutes and more, while the 1M was an ongoing reaction. For the last experiment pat IV “Effect of a Catalyst”, demonstrated which substances will act as a catalyst for to the hydrogen peroxide. A catalyst is a type of enzyme, a substance that increases the rate of a chemical reaction without being consumed. But, as shown in table IV, all of the chemical compounds did not have any reaction. But, for Fe(NO 3 ) 3 and CaCl 2 there was a slow reaction that had taken place but it was hard to tell so that could have been an error in the data. Even though catalyst are very important they do not yield more product and is not part of the products of a reaction.
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