Question

How much heat energy is required to raise the temperature of 0.367 kg of copper from 23.0 C to 60.0 C ? The specific heat of copper is 0.0920 cal/(g x C)



If 125 cal of heat is applied to a 60.0 g - piece of copper at 23.0 C, what will the final temperature be? The specific heat of copper is 0.0920 cal /(g x C)

Answer 1

To both of these you need to know the formula \[q=ms \Delta T\]
Where:
q= energy
m=mass
s= specific heat of substance
\[\Delta T \] =change in temperature.

Notice that the specific heat of Cu is given in cal/g x C. This means our answer will be in calories and that we need to convert 0.367 kg to grams.

0.367 kg (1000g/1kg) = 367 g

Now we just plug and chug.

q=367 x 0.0920 x (60.0-23.0)

q= 1249.27 cal

since there are 3 sig figs the answer should be 1250 cal

B. is a similar concept using the same equation but looking for a different variable (Delta T)

q= 125
m=60.0
s=0.0920
Delta T =?

Solve for Delta T

125=60.0 x0.0920 x (delta T)

(delta T) = 22.6449 or 22.6 (sig figs)

We know know that the temperature rose 22.6 degrees from the initial temp (23) Adding these will give you the final temp.

22.6 + 23= 45.6 C