When 100 cal (418 J) of heat is applied to a 125 g sample, the temperature increases by 28 °C. Calculate the specific heat of the sample and compare your answer to the values in Table 1.10. What is the identity of the sample?

Use the heat equation to calculate the energy, in joules and calories, for each of the following (see TABLE 3.11):

c. lost when 15.0 g of ethanol, C₂H₆O, cools from 60.5 °C to −42.0 °C

Calculate the energy to heat two cubes (gold and aluminum) each with a volume of 10 cm³ from 15 °C to 25 °C. Refer to Tables 2.8 and 3.11.

Calculate the specific heat of copper if it takes 23 cal (96 J) to heat a 5.0 g sample from 25 °C to 75 °C.

The specific heat of fat is 0.45 cal/(g ⋅ °C) (1.9 J/g °C) and the density of fat is 0.94 g/cm³. How much energy (in calories and joules) is needed to heat 10 cm³ of fat from room temperature (25 °C) to its melting point (35 °C)?

On a hot day, the beach sand gets hot but the water stays cool. Would you predict that the specific heat of sand is higher or lower than that of water? Explain.

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A metal is thought to be titanium or aluminum. When 4.7 g of the metal absorbs 11 J, its temperature rises by 4.5 °C.

b. Would you identify the metal as titanium or aluminum (see TABLE 3.11)?

A metal is thought to be copper or gold. When 18 g of the metal absorbs 58 cal, its temperature rises by 35 °C.

a. What is the specific heat, in cal/g °C, of the metal?

When 1.0 tablespoon of butter is burned or used by our body, it releases 100 kcal (100 food Calories or 418.4 kJ) of energy. If we could use all the energy provided, how many tablespoons of butter would have to be burned to raise the temperature of 3.00 L of water from 18.0 ℃ to 90.0 ℃