Measuring Heat Energy in a Potato Chip

Experiment Overview

Objective: Determine the heat energy present in a potato chip by burning it and measuring the heat absorbed by water.
Method: Burn the potato chip and capture the heat in a water container above it. Measure the temperature change of the water to infer the heat energy released by the chip.

Heat Transfer: Heat is transferred from the burning potato chip to the water, raising the water's temperature.
Equation Used: ( Q = m \times C \times \Delta T )
- Q: Heat absorbed by the water (calories)
- m: Mass of the water (grams)
- C: Specific heat of water (calories per gram per degree Celsius)
- (\Delta T): Temperature change of water (degrees Celsius)

Define Variables:
- Mass of water (m): 150 grams (since 1 ml of water = 1 gram)
- Initial Temperature: 21°C
- Final Temperature: 85°C
- Specific heat of water (C): 1 calorie/g°C
Calculate Temperature Change ((\Delta T)):
- ( \Delta T = 85°C - 21°C = 64°C )
Calculate Heat Absorbed (Q):
- ( Q = 150 \times 1 \times 64 = 9600 \text{ calories} )
Convert to Food Calories:
- 9600 small calories = 9.6 kilocalories (food calories)
- Conversion: 1000 small calories = 1 kilocalorie

Calories per Gram:
- Mass of Potato Chip: 1.75 grams
- Calculation: ( \frac{9.6 \text{ food calories}}{1.75 \text{ grams}} = 5.5 \text{ calories per gram} )
Calories Per Serving:
- Serving Size: 34 grams
- Calculation: 34 grams ( \times 5.5 \text{ calories per gram} = 190 \text{ calories} )
- Package Value: 210 calories per serving

Formula: [ \text{Percent Error} = \frac{|\text{Actual Value} - \text{Measured Value}|}{\text{Actual Value}} \times 100% ]
- Calculation: ( \frac{|210 - 190|}{210} \times 100% = 11% \text{ error} )

Why Was There Error?
- Not all the energy from the burning chip is absorbed by the water; some heat energy is lost to the surrounding air.
- This results in a measured energy value that is lower than the actual energy content of the potato chip.