A chemist carefully measures the amount of heat needed to raise the temperature of a 677.0mg sample of a pure substance from 16.6°C to 24.1°C . The experiment shows that 9.4J 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.
Use the calorimetry formula: \(\sf q=m*C_p*\Delta T\) where q is the heat absorbed/released m is the mass of the substance of what the temp is recorded Cp is the specific heat capacity \(\Delta T\) is the change in temp, \(\Delta T=T_f-T_i\)
\[q=677.0 \times C_p \times 7.5\] Would q in this case be 9.4?
yep that's right. the units you'll end up with will be "\(mg ~C^o/J\)" but if you want "\(g ~C^o/J\)" (which are more common) you'll need to convert the mass from mg to grams.
Alright, thank you!
no problem
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