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How much heat energy is required to raise the temperature of 0.368 kg of copper from 23.0 ∘C to 60.0 ∘C? The specific heat of copper is 0.0920 cal/(g⋅∘C) .

Respuesta :

Yipes
[tex]c_{Cu}=0,092\frac{cal}{g^{o}C}\\ \Delta T=60^{o}C-23^{o}C=37^{o}C\\ m=0,368kg=368g\\\\ Q=c\Delta Tm=0,092\frac{cal}{g^{o}C}*37^{o}C*368g=1252,672cal\\\\ Q=1252,672*4,184\approx 5241,2J[/tex]
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Answer:

1252.67 calories or 1.25Kcal

Explanation:

From

H= mcθ

m= mass of the body

c= specific heat capacity of the body

θ= change in temperature

m= 0.368K= 368g

c= 0.0920

θ= 60°C-23°C= 37°C

H= 368× 0.0920× 37

H= 1252.67 calories or 1.25Kcal

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