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A chemist carefully measures the amount of heat needed to raise the temperature of a 0.47 kg sample of C6H7N from 30.5 degrees C to 48.4 degrees C. The experiment shows that 1.65 x 10^4 J of heat are needed. What can the chemist report for the molar heat capacity of C6H7N? Be sure your answer has the correct number of significant digits.

Respuesta :

[tex]\bull\sf m=0.47kg[/tex]

[tex]\bull\sf \Delta T=T_f-T_i=48.4-30.5=17.9°C[/tex]

[tex]\bull\sf Q=1.65\times 10^4J[/tex]

We know according to thermodynamics

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

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

[tex]\\ \sf\longmapsto c=\dfrac{1.65\times 10^4}{0.47\times 17.9}[/tex]

[tex]\\ \sf\longmapsto c=\dfrac{1.65\times 10^4}{8.413}[/tex]

[tex]\\ \sf\longmapsto c=0.1961\times 10^4J/kg°C[/tex]

[tex]\\ \sf\longmapsto c=1961J/kg°C[/tex]

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