Homework Help: Integrated Physics and Chemistry

Posted by Kaitlin on Monday, March 21, 2011 at 11:18am.

A 5.0-gram sample of gold and a 5.0-gram sample of iron both absorb exactly 25 calories of energy. The specific heat of gold is 0.03 cal/g°C. The specific heat of iron is 0.11 cal/g°C. Which of the following statements is true?

A) The gold sample will experience a greater increase in temperature.
B) The iron sample will experience a greater increase in temperature.
C) Both samples will experience the same increase in temperature.

How would i figure this one out?

Integrated Physics and Chemistry - Damon, Monday, March 21, 2011 at 11:21am
A. It takes only .03 cal to heat a gram of gold a degree but much more to heat the same mass of iron a degree.
Integrated Physics and Chemistry - drwls, Monday, March 21, 2011 at 11:24am
Think about the equation that defines specific heat:

Q = M*C*(delta T)

In your case, Q (the added heat) and M (the mass) are the same for gold and iron.

That means delta-T (the change in termperature) is inversely proportional to C, the specific heat.

delta T = (Q/M)*(1/C)

You should be able to figure it out from there.
Integrated Physics and Chemistry - Kaitlin, Monday, March 21, 2011 at 11:28am
So the gold sample will experience a greater increase in temperature?
Integrated Physics and Chemistry - drwls, Monday, March 21, 2011 at 11:36am
Yes. Because gold has a lower specific heat (per unit mass), its temperature rises more.
Integrated Physics and Chemistry - Kaitlin, Monday, March 21, 2011 at 11:38am
Okay. Thank you for the help (:
Integrated Physics and Chemistry - Kaitlin, Monday, March 21, 2011 at 11:38am
Thanks to both of you (:

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