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- Module 2 Practice Problems
- 1. Convert 15.0 oC into Fahrenheit.
- 59.0 oF
- 2. The temperature of deep space is 3.5 K. What is that in Celsius? In Fahrenheit?
- -269.5 oC -453.1 oF
- 3. Some parts of the western United States regularly reach temperatures of 115 oF in the summer.
- What is that in oC?
- 46 oC
- 4. The average person uses 2,500.0 Cal of energy per day. How many Joules is that? Remember that
- a food calorie (Cal) is 1,000 chemistry calories (cal).
- 1.046 x 107
- 5. How many Joules does it take to heat up 15.1 kg of glass from 15 oC to 45 oC? (refer to Table 2.1)
- 379,251.6 J
- 6. 124.1 g of an unknown substance absorbs 50.0 kJ of heat and increases its temperature by 36.3 oC.
- What is its specific heat? (Remember that “k” is the abbreviation for “kilo,” so “kJ” stands for
- kiloJoules.)
- 11.1J/g oC
- 7. A 245 g piece of copper at room temperature (25 oC) loses 456.7 Joules of heat. What will its new
- temperature be?
- -4.8 oC
- 8. Review question #7 mentioned that drinking ice-cold water is a way of burning excess Calories.
- Calculate how many Calories are burned when a 12-ounce (3.40 x 102 g) glass of water at 0.0 oC is
- warmed up to body temperature (37.0 oC).
- 12.58 Cal
- 9. A calorimeter is filled with 150.0 g of water at 24.1 oC. A 50.0 g sample of a metal at 100.0 oC is
- dropped in this calorimeter and causes the temperature to increase a total of 5.4 oC. What is the
- specific heat of the metal? Ignore the calorimeter in this problem.
- 0.96 J/g oC
- 10. A 345.1 g sample of copper at 100.0 oC is dropped into a 4.5 g calorimeter made of an unknown
- substance. If the calorimeter has 150.0 grams of water in it and the temperature changed from 24.2 oC
- to 25.1 oC, what is the specific heat of the calorimeter? (refer to Table 2.1)
- 169 J/g oC
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