A chemist carefully measures the amount of heat needed to raise the temperature of a 281.0g sample of a pure substance from 2.6°C to 13.2°C. The experiment shows that 700.J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.⋅J⋅g−1K−1
Question
A chemist carefully measures the amount of heat needed to raise the temperature of a 281.0g sample of a pure substance from 2.6°C to 13.2°C. The experiment shows that 700.J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.⋅J⋅g−1K−1
Solution
The specific heat capacity (c) of a substance can be calculated using the formula:
c = q / (m * ΔT)
where: q = heat energy absorbed or released (in joules) m = mass of the substance (in grams) ΔT = change in temperature (in Kelvin or Celsius, since the scale is the same)
Given: q = 700 J m = 281.0 g ΔT = 13.2°C - 2.6°C = 10.6°C
Substituting these values into the formula gives:
c = 700 J / (281.0 g * 10.6°C) = 0.235 J/g°C
So, the specific heat capacity of the substance is 0.235 J/g°C. This answer has three significant digits, which is appropriate given the number of significant digits in the original data.
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Specific heat capacity
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