20. Heat and Temperature

When equal amounts of heat are applied to equal masses of iron and silver, which metal warms up faster, and which one has the lower specific heat capacity ($c$)?

When a 290-g piece of iron at 180°C is placed in a 95-g aluminum calorimeter cup containing 250 g of glycerin at 10°C, the final temperature is observed to be 38°C. Estimate the specific heat of glycerin.

When equal amounts of $Q$ (heat) are applied to equal masses $m$, which substance warms up fastest: water, copper, sand, or ethanol?

Which of the following phenomena can be attributed to water's high $c$ (specific heat capacity)?

How does the $c$ (specific heat capacity) of water affect the climates of coastal regions?

Which of the following substances normally warms up faster when the same amount of heat is applied to equal masses?$\text{Q}=mc\Delta T$

Samples of copper, aluminum, and water experience the same temperature rise when they absorb the same amount of heat. What is the ratio of their masses? [Hint: See Table 19–1.]

When a thin metal wire is heated, how does its temperature change compare to that of a thicker wire made of the same material and heated with the same amount of energy ($Q$)?

In very cold weather a significant mechanism for heat loss by the human body is energy expended in warming the air taken into the lungs with each breath. On a cold winter day when the temperature is -20°C, what amount of heat is needed to warm to body temperature (37°C) the 0.50 L of air exchanged with each breath? Assume that the specific heat of air is 1020 J/kg K and that 1.0 L of air has mass 1.3 × 10^-3 kg.

Which statement correctly describes the specific heat capacity of water, given as $4.18 J/g °C$?