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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

they both need two options
for temperture concentration and surface area have decreased and increased
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)

1 answer

It looks like you're conducting a series of experiments on the effect of different variables on the rate of a chemical reaction. Here’s how you might set up your observations based on the sequence you provided:

Data Table

| Condition | Option 1 | Option 2 | |--------------------|---------------------------------------------------|-------------------------------------------------| | Control | All A + B react to form C | Graph is directly proportional | | Decrease Temperature| Particles collide slower (lower slope) | Some reactants remain, only some product is formed | | Increase Temperature| Particles collide faster (steeper slope) | All A + B react to form C | | Decrease Concentration| Particles collide slower (lower slope) | Some reactants remain, only some product is formed | | Increase Concentration| Particles collide faster (steeper slope) | All A + B react to form C | | Decrease Surface Area| Particles collide slower (lower slope) | Some reactants remain, only some product is formed | | Increase Surface Area| Particles collide faster (steeper slope) | All A + B react to form C | | Add Catalyst | Particles collide faster (steeper slope) | All A + B react to form C |

Explanation:

  1. Control: The baseline condition where all reactants A and B are reacting completely to form product C, indicating a directly proportional relationship.

  2. Decrease Temperature: Lower temperatures generally lead to slower particle movement, hence fewer collisions, and resulting in lower product formation with some reactants remaining.

  3. Increase Temperature: Higher temperatures increase particle energy and movement, resulting in more collisions and a steeper reaction slope as all reactants are converted to products.

  4. Decrease Concentration: When the concentration of reactants is decreased, collisions become less frequent, leading again to slower reaction rates and unreacted reactants.

  5. Increase Concentration: Conversely, increasing concentration increases the frequency of collisions, resulting in quicker reaction rates and complete conversion of A and B to product C.

  6. Decrease Surface Area: Reducing surface area (like using larger pieces of solid reactants) decreases the number of available collision sites, slowing the reaction.

  7. Increase Surface Area: Increasing surface area allows more collisions between reactants, speeding up the reaction.

  8. Add Catalyst: Catalysts increase the rate of reaction without being consumed, typically leading to faster collisions and completing the reaction.

Feel free to modify or adjust these points as necessary based on your specific experiment or observations!