Silver specific heat capacity

Use the empirical rule of Dulong and Petit stated in Problem 7 to estimate the specific heat capacities of vanadium, gallium, and silver. 

Q.9.10 After reaching 327.5°C, a large section of the metal chunk melts, demonstrating tliat the metal chunk is a mixture of at least two different metals. A 0.8 kg dull silver chunk has a specific heat capacity of 0.13 kJ/kg-K. Can the specific heat capacity of the remaining chunk be determined without directly measuring it If yes, calculate it. 

Table 10.1 shows that silver has a specific heat capacity of 0.24 J/g °C. The metal is silver. 

Adiabatically operated single scanning calorimeters were used for determinations of the specific heat capacities of copper and brass (Sykes, 1935) and of silver, nickel, brass, quartz, and quartz glass (Moser, 1936). Sykes calorimeter is shown schematically in Figure 7.35. 

The specific heat capacity of silver is 0.24 J/g °C. Express this in terms of calories per gram per Celsius degree. 

Systems may be in chemical or mechanical equilibrium, and they may also exhibit thermal equilibrium. If a hot object is placed in contact with a colder mass of the same material inside an insulated container, heat flows from the hot object into the colder object until the temperatures of the two are equal. Heat lost by the warm object is equal to the amount gained by the cold object. The amount of heat needed to raise the temperature of an object a certain amount is equal to the amount which that object would lose in cooling by the same amount. The amount of heat needed to warm or the amount lost when cooling equals the product of the specific heat (or heat capacity) of the substance, the mass, and the change in temperature. For example, if a 50-gram (1.8-ounce) piece of silver at 70°C (158°F) is placed in 50 grams (1.8 ounces) of water at 15°C (59°F), the principle of thermal equilibrium can be used to calculate the final temperature of the water and silver ... 

Latent heats of evaporation of liquefied gases at low temperatures have been determined by various methods. Dewar, and Behn, dropped pieces of metal of known specific heat into the liquid and measured the gas evolved. Estreicher heated the liquid in a double Dewar vessel electrically and measured the volume of gas evolved. In Donath s apparatus (Fig. 4.VIII L) the gas passed through a copper spiral in a block of lead A, so assuming a constant temperature about 2° above the temperature in the metal calorimeter B. The gas then passed to a vessel inside B connected by a thin German-silver tube. The calorimeter was in two parts, between which was a platinum heating spiral for determining the thermal capacity. Outside was an adiabatic mantle C. The whole was in a vacuous copper jacket D. The temperature differences between A and B, and B and C, were determined by thermocouples. The rise in temperature... 

Calorimetric studies of the type done by Lavoisier and Laplace (Figure 212) were continued by others including Pierre Louis Dulong (1785-1838) and Alexis Therese Petit (1791-1820). They discovered the law that bears their names the product of the specific heat and the atomic weight of solid elements (e.g., lead, gold, tin, silver, and sulfur) is constant. This really implies that all atoms (independent of their identities) have the same capacity for heat. This result was later extended to solid compounds and ultimately cleared up confusions such as whether the binary oxides of copper were really CuO and CUO2 or CU2O and CuO. 

A piece of silver of mass 362 g has a heat capacity of 85.7 J/°C. What is the specific heat of sUvct ... 

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