Question

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) .

Answer 1

`c_(Cu)=0,092(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(cal)/(g^(o)C)*37^(o)C*368g=1252,672cal\\\\ Q=1252,672*4,184\approx 5241,2J`

Answer 2

1252.67 calories or 1.25Kcal

Step-by-step 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