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Chemistry PP

Module 2 - Practice Problems

2.1 Convert 15.0 °C into Fahrenheit. 59 °F
2.2 The temperature of deep space is 3.5 K. What is that in Celcius? In Fahrenheit? -269.5 °C -453.1 °F
2.3 Some parts of the western United States regularly reach temperatures of 115 °F in the summer. What is that in °C? 46 °C
2.4 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
2.5 How many Joules does it take to heat up 15.1 kg of glass from 15 °C to 45 °C? (refer to Table 2.1) 379,251.6 J
2.6 124.1 g of an unknown substance absorbs 50.0 kJ of heat and increases its temperature by 36.3 °C. What is its specific heat? 11.1 J/g∙°C
2.7 A 245 g piece of copper at room temperature (25 °C) loses 456.7 Joules of heat. What will its new temperature be? -4.8 °C
2.8 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 10²g) glass of water at 0.0 °C is warmed up to body temperature (37.0 °C). 12.58 Cal
2.9 A calorimeter is filled with 150.0 g of water at 24.1 °C. A 50.0 g sample of a metal at 100.0 °C is dropped in this calorimeter and causes the temperature to increase a total of 5.4 °C. What is the specific heat of the metal? 0.96 J/g∙°C
2.10 A 345.1 g sample of copper at 100.0 °C is dropped into a 4.5 g calorimeter made of an unknown substance. If the calorimeter has 150.0 g of water in it and the temperature changed from 24.2 °C to 25.1 °C, what is the specific heat of the calorimeter? -169 J/g∙°C
Created by: LiseBrinkley
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