91Ó°ÊÓ

What is the specific heat of a \(500-g\) metal sample that rises \(4.8{ }^{\circ} \mathrm{C}\) when \(307 \mathrm{~J}\) of heat is added to it?

You wish to heat \(250 \mathrm{~g}\) of water to make a hor cup of coffee. If the water starts at \(20^{\circ} \mathrm{C}\) and you want your coffee to be \(95^{\circ} \mathrm{C}\), calculate the minimum amount of heat required. SSM

In a thermodynamically sealed container, \(20 \mathrm{~g}\) of 15 \({ }^{\circ} \mathrm{C}\) water is mixed with \(40 \mathrm{~g}\) of \(60^{\circ} \mathrm{C}\) water. Calculate the final equilibrium temperature of the water.

How much heat is transferred to the environment when the temperature of \(2.00 \mathrm{~kg}\) of water drops from 88 \({ }^{\circ} \mathrm{C}\) to \(42^{\circ} \mathrm{C}\) ?

A copper pot has a mass of \(1.0 \mathrm{~kg}\) and is at \(100^{\circ} \mathrm{C}\). How much heat must be removed from it to decrease its temperature to precisely \(0^{\circ} \mathrm{C}\) ? The specific heat of copper is \(387 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K})\).

A lake has a specific heat of \(4186 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K})\). If we transferred \(1.7 \times 10^{14} \mathrm{~J}\) of heat to the lake and warmed the water from \(10^{\circ} \mathrm{C}\) to \(15^{\circ} \mathrm{C}\), what is the mass of the water in the lake? Neglect heat released to the surroundings. SSM

A 50 -g calorimeter cup made from aluminum contains \(100 \mathrm{~g}\) of water. Both the aluminum and the water are at \(25^{\circ} \mathrm{C}\). A \(300-\mathrm{g}\) cube of some unknown metal is heated to \(150{ }^{\circ} \mathrm{C}\) and placed into the calorimeter; the final equilibrium temperature for the water, aluminum and metal sample is \(41^{\circ} \mathrm{C}\). Calculate the specific heat of the unknown metal and make a guess as to its composätion.

A sealed container (with negligible heat capacity) holds \(30 \mathrm{~g}\) of \(120^{\circ} \mathrm{C}\) steam. Describe the final state if \(100,000 \mathrm{~J}\) of heat is removed from the steam.

Suppose \(20 \mathrm{~g}\) of ice at \(-10^{\circ} \mathrm{C}\) is placed into \(300-\mathrm{g}\) of water in a 200-g copper calorimeter. If the final temperature of the water and copper calorimeter is \(18{ }^{\circ} \mathrm{C}\), what was the initial common temperature of the water and copper?

What mass of ice at \(-20^{\circ} \mathrm{C}\) must be added to 50 g of steam at \(120^{\circ} \mathrm{C}\) to end up with water at \(40^{\circ} \mathrm{C}\) ?