Exploring Rates of Change Lab
Exploring Rates, Equilibrium, and Organic Chemistry
Brandon Sher
SCH 4U
For: Ms. Merhai
Due date: June 1st,2013
Introduction:
Organic chemistry. Two quantities one could measure with the presence of organic chemicals are chemical equilibrium and rate of reaction. Chemical equilibrium is the ratio between the forward and reverse process of a reaction. This is represented by the equation: K = products / reactants. When a reaction has reached equilibrium, the rate of the forward and reverse reactions are equal.
Hypothesis/Prediction:
Experiment 1:
All of the kernels will pop due to the increase in temperature, presence of a catalyst and pressure.
Experiment 2:
The Ka value is going to be high.
Experiment 3:
If the concentration of HCl increases, then the dissolving of magnesium in the solution will occur faster. The decreasing of temperature will cause the magnesium to take longer to dissolve. When using pieces of magnesium as opposed to a strip, it will dissolve faster and lead to a faster reaction time as more surface area is present , and the use of copper will not affect the reaction in any sort of way.
Materials:
Experiment 1: As per lab manual (given)
Experiment 2: As per lab manual (given)
Experiment 3: As per lab manual (given)
Procedure:
Experiment 1: As per lab manual (given)
Experiment 2: As per lab manual (given)
Experiment 3: As per lab manual (given)
Results:
Experiment 1:
|Substance |Size |Colour |Shape/Texture |
|Unpopped Kernel |Small |Golden yellow |-Smooth |
| | | |-Hard |
|Popped Kernel |Large |Off white |-Rigid
Brandon Sher
SCH 4U
For: Ms. Merhai
Due date: June 1st,2013
Introduction:
Organic chemistry. Two quantities one could measure with the presence of organic chemicals are chemical equilibrium and rate of reaction. Chemical equilibrium is the ratio between the forward and reverse process of a reaction. This is represented by the equation: K = products / reactants. When a reaction has reached equilibrium, the rate of the forward and reverse reactions are equal.
Hypothesis/Prediction:
Experiment 1:
All of the kernels will pop due to the increase in temperature, presence of a catalyst and pressure.
Experiment 2:
The Ka value is going to be high.
Experiment 3:
If the concentration of HCl increases, then the dissolving of magnesium in the solution will occur faster. The decreasing of temperature will cause the magnesium to take longer to dissolve. When using pieces of magnesium as opposed to a strip, it will dissolve faster and lead to a faster reaction time as more surface area is present , and the use of copper will not affect the reaction in any sort of way.
Materials:
Experiment 1: As per lab manual (given)
Experiment 2: As per lab manual (given)
Experiment 3: As per lab manual (given)
Procedure:
Experiment 1: As per lab manual (given)
Experiment 2: As per lab manual (given)
Experiment 3: As per lab manual (given)
Results:
Experiment 1:
|Substance |Size |Colour |Shape/Texture |
|Unpopped Kernel |Small |Golden yellow |-Smooth |
| | | |-Hard |
|Popped Kernel |Large |Off white |-Rigid