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A chemist carefully measures the amount of heat needed to raise the temperature of a 1.05 kg sample of a pure substance from 1.9 °C to 19.7 °C. The
experiment shows that 4.39 kJ 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.
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Answer :

  • Mass=m=1.05kg
  • initial temperature=1.9°C
  • Final temperature=19.7°C
  • ∆T=19.7-19.7=17.8°C
  • Heat=Q=4.39KJ=4390J

Now

[tex]\\ \sf\longmapsto Q=mc\Delta T[/tex]

[tex]\\ \sf\longmapsto c=\dfrac{Q}{m\Delta T}[/tex]

[tex]\\ \sf\longmapsto c=\dfrac{4390}{1.95(17.8)}[/tex]

[tex]\\ \sf\longmapsto c=\dfrac{4390}{18.69}[/tex]

[tex]\\ \sf\longmapsto c=234.8J/kg°C[/tex]

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