🤓 Based on our data, we think this question is relevant for Professor Blake's class at UCI.

Recall:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{\u2206}}{\mathbf{T}}}$

where m = mass in g

c = heat capacity in J/g°C

ΔT = change in temperature

**Isolating c (heat capacity):**

$\frac{\mathbf{q}}{\mathbf{m}\mathbf{\u2206}\mathbf{T}}{\mathbf{=}}\frac{\overline{)\mathbf{m}}\mathbf{c}\overline{)\mathbf{\u2206}\mathbf{T}}}{\overline{)\mathbf{m}\mathbf{\u2206}\mathbf{T}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{c}}{\mathbf{=}}\frac{\mathbf{q}}{\mathbf{m}\mathbf{\u2206}\mathbf{T}}}$

The heat capacity of water is **4.186 J/g°C**.

An average rock has a heat capacity of **2.0 J/g°C**.

Suppose you are cold-weather camping and decide to heat some objects to bring into your sleeping bag for added warmth. You place a large water jug and a rock of equal mass near the fire. Over time, both the rock and the water jug warm to about 38 ^{o}C (100 ^{o}F). If you could bring only one into your sleeping bag, which one should you choose to keep you the warmest?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calorimetry concept. You can view video lessons to learn Calorimetry. Or if you need more Calorimetry practice, you can also practice Calorimetry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Blake's class at UCI.