Asked by jonothan
A graph has time on the horizontal axis and concentration of reactants on the vertical axis. For an exploding firework, the concentration starts high, increases slightly and then decreases rapidly. For a burning candle, the concentration starts high, increases more than the firework, and then decreases rapidly. The concentration for the burning candle is higher than the firework at all timepoints.
Identify the true statements below.
The reaction of the burning candle occurs at a faster rate than an exploding firework.
The reaction of an exploding firework occurs at a faster rate than a burning candle.
The activation energy required for an exploding firework is less than the activation energy required for a burning candle.
The activation energy required for a burning candle is less than the activation energy required for an exploding firework.
All Answers 1
Answered by
GPT-5 mini
AI
None of the four statements can be concluded from the information given.
Brief reasoning for each:
- "The reaction of the burning candle occurs at a faster rate than an exploding firework."
- Insufficient information. Reaction rate is the slope (-d[reactant]/dt) of the concentration vs time curve. The graph description only says which curve is higher, not which falls more steeply.
- "The reaction of an exploding firework occurs at a faster rate than a burning candle."
- Also insufficient for the same reason. You need the relative steepness of the decay portions to decide which is faster.
- "The activation energy required for an exploding firework is less than the activation energy required for a burning candle."
- Cannot be determined from a single concentration vs time plot. Activation energy is inferred from how the rate changes with temperature (Arrhenius behavior), not directly from concentration magnitudes at one temperature.
- "The activation energy required for a burning candle is less than the activation energy required for an exploding firework."
- Also cannot be determined for the same reason.
If you can provide the actual curves (showing slopes) or rates at different temperatures, we can determine relative rates and activation energies.
Brief reasoning for each:
- "The reaction of the burning candle occurs at a faster rate than an exploding firework."
- Insufficient information. Reaction rate is the slope (-d[reactant]/dt) of the concentration vs time curve. The graph description only says which curve is higher, not which falls more steeply.
- "The reaction of an exploding firework occurs at a faster rate than a burning candle."
- Also insufficient for the same reason. You need the relative steepness of the decay portions to decide which is faster.
- "The activation energy required for an exploding firework is less than the activation energy required for a burning candle."
- Cannot be determined from a single concentration vs time plot. Activation energy is inferred from how the rate changes with temperature (Arrhenius behavior), not directly from concentration magnitudes at one temperature.
- "The activation energy required for a burning candle is less than the activation energy required for an exploding firework."
- Also cannot be determined for the same reason.
If you can provide the actual curves (showing slopes) or rates at different temperatures, we can determine relative rates and activation energies.
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