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As concentration increases, the reaction rate increases B. As the surface area increases, the reaction rate remains relatively the same according to my group’s data, but in other circumstances increased surface should increase the reaction rate. C. As the temperature increases, the reaction rate increases due to higher number of collisions 3. Yes doubling the concentration did double the reaction rate. Because if you look at the debatable above, it took the 6. MM half the time that the 3. M to dissolve the metal, and this happened because with the higher concentration, you have more collisions, and with more collisions the reaction happens faster. 4. According to my table the flat piece of magnesium dissolved faster than the rest. Theoretically slivers should have come first because it has more surface area. The reaction might have happened slower because of human error, if we ad water left over in the test tube and we added the acid into that, so the acid was weaker, or any other type of human error. 5.
The slowest reaction rate was the 1 co. This is because this is near freezing and molecules are moving very slowly and there are very little collisions happening, so there is a slow reaction. 6. A. Reaction time for 4. MM hydrochloric acid, it’s at 6. 6 x g MGM/s B. Reaction time for ICC is 3. 0 x IOWA g Meg’s 7. By doubling the rate, yes you are doubling the reaction rate, because larger kinetic energy, more collisions and if you look at the temperature graph above, o can see the steep increase of the graph. Follow Questions 1.
Is it possible to vary the factors because, in terms of concentration, if we left water in a test tube and we add acid to it, the acidity is going to lower, and it will not be strong enough to react with the metal, and the collision will have already happened with the acid and H2O. In terms of surface area if we have not polished the metal enough then even if we cut it into little pieces, it’s still going to take the same amount of time, the acid molecules are trying to react with the metal, but the coating is preventing it.
And in terms of temperature, the higher the temperature the higher the collision rate but if we don’t have a high enough temperature then the collisions will not happen, and no reaction will result. 2. If we add a catalyst to this reaction, we will increase the reaction rate, thus causing the reaction to speed up. 3. We will be more successful in lighting a fire from kindling because this has more surface area than a log. 4. When you blow on a smoldering fire, you are adding more concentration of oxygen on that area, and since fire depends on oxygen to burn, it will make it burn better.
Conclusion After performing experiments on how different factors affect reaction rate. When there are an effective number of collisions that results in the formation of new particles then you have a successful reaction. The increase in the concentration showed us this, when the metal dissolved very quickly in a 6. MM. I conclude from my data, increasing the concentration will increase the reaction rate, cutting up the pieces of Magnesium to create more surface area, does not create a great difference in the reaction rate, and lastly we did not have sufficient time to finish part Ill.