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Answer :
Final answer:
Using the formula q=m*c*ΔT, the amount of energy required to raise the temperature of 14.6 grams of liquid mercury from 21.3 °C to 36.6 °C was calculated to be approximately 31 J. As such, none of the given choices are correct. Also, there is an energy change in this process, which is the energy absorbed by the mercury.
Explanation:
The subject of this question is calorimetry which belongs to Physics, particularly thermodynamics. This problem is about calculating the amount of energy required to change the temperature of a given mass of mercury. In the physical sciences, we use the formula q=m*c*ΔT to calculate the heat energy (q) involved in changing the temperature (ΔT) of a specific mass (m) of a substance. Each substance has a characteristic specific heat (c), which is the amount of heat per unit mass required to raise the temperature by one degree Celsius.
Mercury has a specific heat capacity of about 0.14 J/g°C. By substituting m = 14.6 g, c = 0.14 J/g°C, and ΔT = (36.6-21.3)°C = 15.3°C into the formula, we get q = 14.6g * 0.14 J/g°C * 15.3°C ≈ 31 J. Thus from our calculations, none of the options provided seems correct.
Regarding the second part of your question, "What is the energy change during this process?", it can be said that energy change refers to the difference in the amount of energy present at the beginning of a process and at the end. In this context, it is the heat energy absorbed by the mercury, which we calculated as approximately 31 J. So, true, there is an energy change during the process.
Learn more about Heat Energy Calculation here:
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