# A 5.82-kg piece of copper metal is heated from 21.5°C to 328.3°C. What is the heat absorbed (in kJ) by the metal?

Jul 18, 2017

The heat absorbed is $= 687.4 k J$

#### Explanation:

The heat absorbed is

$E = m \cdot C \cdot \Delta T$

The mass is $= 5.82 k g$

The specific heat of copper is C=0.385kJkg^-1ºC^-1

The change in temperature is

$\Delta T = 328.3 - 21.5 = 306.8$

Therefore,

$E = 5.82 \cdot 0.385 \cdot 306.8 = 687.4 k J$

Jul 18, 2017

Here are all informations that we have :

• Mass of copper(m) $= 5.82 g$
• Specific Heat Capacity (I will just name it SHC) of copper =0.385 J(g°C)^-1 $\rightarrow$ simpler way to write 0.385 J/g°C
• Change in temperature ($\Delta C$) =328.3°C-21.5°C=306.8°C

Then we start

Firstly the formula,

SHC $= \frac{H e a t}{m \cdot \Delta C}$

Then we replace the values and calculate it

0.385=(Heat)/(5.82*306.8°C)

Heat=0.385*(5.82*306.8°C)

Therefore, heat absorbed$= 687.44676 J = 687 \left(3 s . f\right)$

(I put the answer at 3 significant figures (s.f) but for further calculations use the first value obtained)