Copper specific heat capacity

A llO.-g sample of copper (specific heat capacity = 0.20 J °C-1 g-1) is heated to 82.4°C and then placed in a container of water at 22.3°C. The final temperature of the water and copper is 24.9°C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water ... 

Heat capacities, C, are also reported for pure substances, not just for the complicated assembly of substances that makes up a typical calorimeter. For instance, we can report the heat capacity of water or of copper. More heat is needed to raise the temperature of a large sample of a substance by a given amount than is required to raise the temperature of a small sample by the same amount, so heat capacity is an extensive property the larger the sample, the greater its heat capacity (Fig. 6.15). It is therefore common to report either the specific heat capacity (often called just specific heat ), Cs, which is the heat capacity divided by the mass of the sample (Cs = dm), or the molar heat capacity, Cm, the heat capacity divided by the number of moles in the sample (Cm = dn). Specific heat capacities and molar heat capacities are intensive properties. 

Self-Test 6.7A A piece of copper of mass 19.0 g was heated to 87.4°C and then placed in a calorimeter that contained 55.5 g of water at 18.3°C. The temperature of the water rose to 20.4°C. What is the specific heat capacity of copper ... 

A piece of copper of mass 20.0 g at 100.0°C is placed in an insulated vessel of negligible heat capacity but containing 50.7 g of water at 22.0°C. Calculate the final temperature of the water. Assume that all the energy lost by the copper is gained by the water. The specific heat capacity of copper is 0.38 J-(°C) 1-g 1. 

While the procedure for this experiment is provided with a fair amount of detail, students can have input into the design of the calorimeter and, although a list of materials is provided, different materials can be made available and they can choose the ones they think would be most effective. The inquiry aspect of this experiment lies primarily in the detailed analysis of their results required to suggest an appropriate interstitial material and the need to assess sources of error. If, for example, students have a large error in the determination of the specific heat capacity of copper, they must decide what could contribute to the error and then try to redesign their calorimeter or their technique in order to limit the error. 

O The specific heat capacity of aluminum is 0.902 J/g°C. The specific heat capacity of copper is 0.389 J/g°C. The same amount of heat is applied to equal masses of these two metals. Which metal increases more in temperature Explain. 

Exactly three grams of carbon were burned to CO2 in a copper calorimeter. The mass of the calorimeter is 1 500 g, and the mass of water in the calorimeter is 2 000 g. The initial temperature was 20.0 °C and the final temperature 31.3 °C. Calculate the heat of combustion of carbon in joules per gram. Specific heat capacity of copper is 0.389 J/g - K. 

Furthermore, diamond exhibits the largest thermal conductivity among all naturally occurring materials. With 20 Wcm K , it is about five times higher than that of copper. At the same time it expands only to small extents, which reflects in a coefficient of thermal expansion of 1.06 x 10 K (mK ). The specific heat capacity at 25 °C is 6.12 J mol- K-. ... 

SAMPLE PROBLEM 6.3 Finding Quantity of Heat from Specific Heat Capacity Problem A layer of copper welded to the bottom of a skillet weighs 125 g. How much heat is needed to raise the temperature of the copper layer from 25°C to 300.°C The specific heat capacity (c) of Cu is 0.387 J/g-K. 

General Zod has sold Lex Luthor what Zod claims to be a new copper-colored form of kryptonite, the only substance that can harm Superman. Lex, not believing in honor among thieves, decided to carry out some tests on the supposed kryptonite. From previous tests. Lex knew that kryptonite is a metal having a specific heat capacity of 0.082 J/g °C, and a density of 9.2 g/cm. ... 

Lex Luthor s first experiment was an attempt to find the specific heat capacity of kryptonite. He dropped a 10 g 3 g sample of the metal into a boiling water bath at a temperature of 100.0°C 0.2°C. He waited until the metal had reached the bath temperature and then quickly transferred it to 100 g 3 g of water that was contained in a calorimeter at an initial temperature of 25.0°C 0.2°C. The final temperature of the metal and water was 25.2°C. Based on these results, is it possible to distinguish between copper and kryptonite Explain. 

Taking the specific heat capacities of copper and water to be 385 and 4185 Jkg respectively, a balance of the heat losses gives... 

The specific heat capacity of Cu-l.6Fe-9.9Ni (mass%) and Cu-0.8Fe-30.9Ni (mass%) alloys was measured by [1986Ric] in the temperature interval from 59 to 946°C. Both alloys show nearly the same specific heat capacity as copper. In Cu-l.6Fe-9.9Ni (mass%) alloy an additional contribution, due to the precipitation of nickel-iron particles is found. It should be noted that investigated alloys contained up to 0.03 mass% C and 0.81 mass% Mn. 

The quantity of heat energy required to raise the temperature of a piece of materi depends upon the type of material and its mass. Thus equal masses of two different materials will require different amounts of heat energy to raise their temperature by the same amount e.g. 1 kg of water with a specific heat capacity of 4200J/(kg °C) will require 4200 joules of heat energy to raise its temperature by 1 C. Similarly, 1 kg of copper of specific heat capacity 386J/(kg °C) will require 386 joules to raise its temperature by 1°C. 

A 40.0-g sample of copper at 200°C is dropped into a well-insulated vessel containing 100.0 g of H2O initially at 25°C. Calculate the final temperature of the system given that the specific heat capacity of water is 4.184 J g °C and the specific heat capacity of copper is 0.385 J g °C. ... 

The above Eq. 6.4 has two heat loss constants that can be converted into single heat loss constant by using the thermal mass relationship between the copper and composite. For a body of uniform composition, thermal mass, C , can be approximated by Cfh = m Cp, where m is the mass of the body and Cp is the isobaric specific heat capacity of the material averaged over temperature range in question. Thus, the equivalent thermal mass for a copper plate to aerogel composite for a constant cross-sectional area (Axz) will be as follows ... 

Equation 6.5 shows the equivalent thickness of a copper plate that will have the same thermal mass as the aerogel composite. Table 6.1 shows the specific heat capacities of the materials used in the experiment. The specific heat capacity for the aerogel composite is estimated using the mle of mixmre as shown where x is the weight fraction of the aerogels and y is the weight fraction of FMWNT. Where there... 

The choice of materials for plate heat exchanger/reactors also depends on the desired dynamic properties of the microsystem. One important parameter is the energy demand for fuel processor start-up, which results from the product of specific heat capacity and density of the construction material. For a given geometry and volume of the device, aluminum is favored over copper and stainless steel. 

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. 

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