Specific heat capacity, table

In addition to the thermal conductivity, the heat transfer of the compound into the material of the mold wall is an important factor. The heat penetration is determined by the thermal conductivity, density, and specific heat capacity. Table 3.12 shows the values of various commonly used mold materials. BeCu alloys showa very good... 

These expressions may be rearranged to calculate the specific or molar heat capacity from the measured temperature rise caused by a known quantity of heat. The specific heat capacity of a dilute solution is normally taken to be the same as that of the pure solvent (which is commonly water). Table 6.2 lists the specific and molar heat capacities of sume common substances. 

The development and application of the method can be illustrated by considering the problem of integrating the utilisation of energy between 4 process streams. Two hot streams which require cooling, and two cold streams that have to be heated. The process data for the streams is set out in Table 3.3. Each stream starts from a source temperature Ts, and is to be heated or cooled to a target temperature Tt. The heat capacity of each stream is shown as CP. For streams where the specific heat capacity can be taken as constant, and there is no phase change, CP will be given by ... 

Calculate the specific enthalpy of water at a pressure of 1 bar and temperature of 200 °C. Check your value using steam tables. The specific heat capacity of water can be calculated from the equation ... 

From the steam tables in the Appendix, the latent heat of vaporisation of water at 312 K is 2410 kl/kg. Again from steam tables, the specific heat capacity of water vapour = 1.88 kJ/kg K and that of the solids will be taken as 2.18 kl/kg K. 

The amount of energy that is needed to raise the temperature of one gram of a substance 1°C (or 1 K) is the specific heat capacity, c, of the substance. Specific heat capacity is usually expressed in units of J/g C. The specific heat capacities of several substances are given in Table 5.2. Figure 5.12 shows that you can often predict the relative specific heat capacities of familiar substances. 

Table 5.2 Specific Heat Capacities of Selected Substances...

You can use the specific heat capacity of a substance to calculate the amount of energy that is needed to heat a given mass a certain number of degrees. You can also use the specific heat capacity to determine the amount of heat that is released when the temperature of a given mass decreases. The specific heat capacity of liquid water, as shown in Table 5.2, is 4.184 J/g °C. This relatively large value indicates that a considerable amount of energy is needed to raise or lower the temperature of water. 

If a substance is heated without a change of state, the amount of heat required to change the temperature of 1 gram by 1° C is called the specific heat capacity of the substance. Similarly, the molar heat capacity is the amount of heat needed to raise the temperature of 1 mole of a substance by 1° C. Table 7-2 shows the heat capacities of several elements and compounds. 

Groundwater has a huge capacity to store heat (4181 J/kg/K). Rocks and minerals have a lesser (around 800 J/kg/K Mellon 2001), but still significant, heat capacity. They also have a certain thermal conductivity and these properties allow them to act as enormous subsurface heat storage and exchange reservoirs. Table 1 provides some examples of specific heat capacities and thermal conductivities. This heat, stored in the geological environment, can be extracted, manipulated and utilized. 

The specific and molar heat capacities of some common substances are given in Table 6.1. Note that, although the values of the specific heat capacities are listed in joules per degree Celsius per gram (J-(°C) 1 -g 1), they could equally well be reported in joules per kelvin per gram (J-K 1-g ) with the same numerical values, because the size of the Celsius degree and the kelvin are the same. We can calculate the heat capacity of a substance from its mass and its specific heat capacity by rearranging the definition Cs = dm into C = mCs. Then we can use... 

Determine the temperature change when 10.0 g of (a) KCl (b) MgBr2 (c) KN03 (d) NaOH dissolves in 100.0 g of water Assume that the specific heat capacity of the solution is 4.18 J-K, -g 1 and that the enthalpies of solution in Table 8.6 are applicable. 

Table 2.2 Typical values of specific heat capacities.

Water has a relatively high specific heat capacity, whereas inorganic compounds have lower heat capacities. Organic compounds are in the medium range (Table 2.2). 

In this expression, Q represents the specific energy of the reaction or of the decomposition. The specific heat capacities given in Table 2.2 can be used. However, as a first approximation, the following specific heat capacities may be useful ... 

Table 7.1 Specific heat capacity of a polyamide 6 thermoplastic.

Table 7.2 Interpolated specific heat capacity (J/kg/K) for each temperature.

The transition of a protein or a single cooperative domain from the native to the denatured state is always accompanied by a significant increase of its partial heat capacity (see, for reviews, Sturtevant, 1977 Privalov, 1979). The denaturationaJ increment of heat capacity A JCP = C° Cp amounts to 25-50% of the partial heat capacity of the native protein and does not depend noticeably on the environmental conditions under which denaturation proceeds (Fig. 1) or on the method of denaturation. However, it is different foi different proteins and seems to correlate with the number of contacts between nonpolar groups in native proteins (Table I). On the other hand, the partial specific heat capacities of denatured states of different proteins appear to be rather similar (Tiktopulo et... 

The specific heat capacity of water is relatively large 4.184 J/g-°C. This value helps to explain how water can absorb and release enough energy to moderate Earth s temperature. Examine the values in Table 14.2. Notice that the specific heat capacities of most substances are much lower than the specific heat capacity of water. 

You have enough information to solve this problem using Q = me AT. Use the initial and final temperatures to calculate AT. You need the specific heat capacity (c) of liquid water. This is given in Table 14.2 (4.184 J/g-°C). Because you are only concerned with the water, you will not use the mass of the ice. 

In Part A of the ThoughtLab on page 594, the students added ice to 120.0 g of water in beaker 2. Calculate the heat lost by the water. Use the information given for beaker 2, as well as specific heat capacities in Table 14.2. 

TABLE 1.11. Specific Heat Capacity of Water Relative to Other Substances... 

We also need to know the heat required to raise the temperature of a given amount of water by 1°C. Table 9.3 lists the specific heat capacity of water as 4.18 J °C 1 g-1. This means that 4.18 J of energy is required to raise the temperature of 1 g of water by 1°C. 

High-quality audio amplifiers generate large amounts of heat. To dissipate the heat and prevent damage to the electronic devices, manufacturers use heat-radiating metal fins. Would it be better to make these fins out of iron or aluminum Why (See Table 9.3 for specific heat capacities.)... 

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