A 150-g quantity of a certain metal, initially at 120°C, is dropped into an insulated beaker containing 100 g of water at 20°C. The final temperature of the metal and water in the beaker is measured as 35°C. Assume that the heat ca- pacity of the beaker can be ignored. a. How much heat has been transferred from the metal to the water? b. Given the temperature change and mass of the metal, what is the specific heat capacity of the metal? C. If the final temperature of the water and this metal is 70°C instead of 35°C, what quantity of this metal (ini- tially at 120°C) was dropped into the insulated beaker?
Latent heat and phase change
A physical process in which a conversion among the basic states or phases of matter, i.e., solid, liquid, and gas takes place under the effect of a certain temperature and pressure is referred to as a phase change. Generally, the phase change of a substance occurs when heat transfer takes place between the substance and its surroundings. Based on the direction in which heat transfer takes place, different types of phase changes can occur.
Triple Point of Water
The branch of physics in which observer deals with temperature related properties is called thermodynamics.
Boiling Point of Water
Everyday examples of boiling is, boiling milk, heating water. One would have observed that when we heat water it goes through various stages and at one point bubbles show in water, and water keeps splashing with bubbles bursting, we in layman terms say that water is boiling.
Freezing Point of Water
In general, the freezing point of water is 0° Celsius, or 32° Fahrenheit. This is the temperature at which water will ordinarily change from its liquid state to its solid state (ice). However, there are certain conditions that can affect the freezing point of water. For example, a liquid may be supercooled or contain impurities so that it does not freeze at the ordinary freezing point.
A 150-g quantity of a certain metal, initially at 120°C, is
dropped into an insulated beaker containing 100 g of water
at 20°C. The final temperature of the metal and water in
the beaker is measured as 35°C. Assume that the heat ca-
pacity of the beaker can be ignored.
a. How much heat has been transferred from the metal to
the water?
b. Given the temperature change and mass of the metal,
what is the specific heat capacity of the metal?
C.
If the final temperature of the water and this metal is
70°C instead of 35°C, what quantity of this metal (ini-
tially at 120°C) was dropped into the
insulated beaker?
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