Final answer:
Using the equation q = mcΔT, we calculate the final temperature after transferring 1.00 kcal of heat into 1.00 kg of a substance, initially at 20.0°C. For water, with a specific heat of 1 kcal/kg°C, the final temperature would be 21.0°C. For other substances like concrete, steel, and mercury, similar calculations can be done using the specific heat capacities found in reference tables. Option D is correct.
Step-by-step explanation:
The question is about the specific heat capacity of substances and how it affects the rise in temperature when heat is applied. Let's go step by step to calculate the final temperature for different materials when 1.00 kcal of heat is transferred into 1.00 kg of the substance originally at 20.0°C.
We use the equation q = mcΔT, where q is the heat transfer, m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT (delta T) is the temperature change. To find the final temperature (Tfinal), we rearrange the equation to Tfinal = Tinitial + ΔT.
For water, the specific heat capacity (c) is approximately 1.00 kcal/kg°C. Thus, when 1.00 kcal is added to 1.00 kg of water, the temperature change (ΔT) is 1.00°C, making the final temperature 21.0°C.
For concrete, steel, and mercury, the process is similar, but the specific heat capacity will be different for each and can be found in reference tables such as Table 5.1 mentioned in the original question. With their specific heat capacities, we can apply the same equation to determine the final temperatures for each material.