Use the link above to 'run' the experiment. Go through each test in the suggested order and select the options from the list that best fit your observations. Each box should have two solutions when you complete this portion. To run a test click "Run Reaction". Use the drop down on the simulation to select a new variable and the choose to decrease. Next click "start over" to reset and choose the next condition. The sequence below matches your data table. Control Decrease Temperature Increase Temperature Decrease Concentration Increase Concentration Decrease Surface Area Increase Surface Area Add Catalyst

Question

option, particles collide faster(steeper slope)
all a+b react to form c
control graph is directly proportional
some reactants remain only some product is formed
particles collide slower(lower slope)

Answer 1

To complete the experiment and analyze the effects of various conditions on the reaction, you can organize the observations according to the sequences of tests and their expected outcomes. Here's a structured response based on the mentioned conditions.

1. Control

   • Observation: Control graph is directly proportional
   • Reasoning: In the control, the reaction proceeds without any manipulation, demonstrating a steady increase in product formation.

2. Decrease Temperature

   • Observation: Particles collide slower (lower slope)
   • Reasoning: Lowering the temperature typically decreases the kinetic energy of the particles, leading to fewer effective collisions.

3. Increase Temperature

   • Observation: Particles collide faster (steeper slope)
   • Reasoning: Increasing the temperature raises the energy of the particles, resulting in more frequent and effective collisions.

4. Decrease Concentration

   • Observation: Some reactants remain; only some product is formed
   • Reasoning: Reducing the concentration of the reactants means fewer particles are available to collide, leading to incomplete reaction.

5. Increase Concentration

   • Observation: All a + b react to form c
   • Reasoning: Higher concentration increases the number of particles available for collisions, promoting complete reaction.

6. Decrease Surface Area

   • Observation: Particles collide slower (lower slope)
   • Reasoning: A smaller surface area reduces the opportunity for collisions, which slows down the overall reaction rate.

7. Increase Surface Area

   • Observation: Particles collide faster (steeper slope)
   • Reasoning: Increasing the surface area provides more opportunities for collisions among reactants, enhancing the rate of reaction.

8. Add Catalyst

   • Observation: Particles collide faster (steeper slope)
   • Reasoning: A catalyst lowers the activation energy, allowing more collisions to result in a reaction, thus increasing the reaction rate.

You can compile these observations into a data table summarizing the respective outcomes for each test condition. This way, you'll have a clear view of how each variable affects the reaction rate.