To analyze the data and draw conclusions, let's look closely at the relationship between the amount of ice added and the resulting temperature change in the samples of water.
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Sample 1: Initial = 20.2°C, Final = 16.0°C, Ice added = 60g
- Temperature change = 20.2 - 16.0 = 4.2°C
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Sample 2: Initial = 48.1°C, Final = 44.2°C, Ice added = 59.9g
- Temperature change = 48.1 - 44.2 = 3.9°C
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Sample 3: Initial = 6.1°C, Final = 1.0°C, Ice added = 71.1g
- Temperature change = 6.1 - 1.0 = 5.1°C
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Sample 4: Initial = 14.6°C, Final = 3.3°C, Ice added = 122.6g
- Temperature change = 14.6 - 3.3 = 11.3°C
From the data:
- As the amount of ice added increases, there is an observable trend that the temperature decreases more significantly. Sample 4, which had the most ice added (122.6g), resulted in the largest temperature drop (11.3°C).
Now let's evaluate the options:
- As the temperature increases, the kinetic energy of the water molecules decreases: This is incorrect because higher temperatures correlate to higher kinetic energy.
- As the temperature decreases, the kinetic energy of the sample increases: This is incorrect; typically, lower temperature signifies lower kinetic energy.
- As the amount of ice added decreases, the temperature decreases: This statement is misleading; the temperature does decrease, but the trend shows that larger amounts of ice added correspond to more significant decreases in temperature.
- As the amount of ice added increases, the change in temperature increases: This conclusion seems to hold true based on the data.
Therefore, the correct conclusion is: As the amount of ice added increases, the change in temperature increases.