Question
A 50.0 -g sample of copper is at $25.0^{\circ} \mathrm{C}$ . If 1200 $\mathrm{J}$ of energy is added to it by heat, what is the final temperature of the copper?
Step 1
0^{\circ} \mathrm{C}$, the mass of the copper ($m$) is $50.0 \, \mathrm{g}$, and the amount of heat added ($Q$) is $1200 \, \mathrm{J}$. We are asked to find the final temperature of the copper ($T_f$). Show more…
Show all steps
Your feedback will help us improve your experience
Shoukat Ali and 100 other Physics 101 Mechanics educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
A $70.0-\mathrm{g}$ piece of copper metal at $54.0^{\circ} \mathrm{C}$ is placed in $50.0 \mathrm{~g}$ of water at $26.0^{\circ} \mathrm{C}$. If the final temperature of the water and metal is $29.2^{\circ} \mathrm{C},$ what is the specific heat $\left(\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}\right)$ of copper? (3.6)
Matter and Energy
Changes of State
A $70.0-\mathrm{g}$ piece of copper metal at $54.0^{\circ} \mathrm{C}$ is placed in $50.0 \mathrm{~g}$ of water at $26.0{ }^{\circ} \mathrm{C}$. If the final temperature of the water and metal is $29.2^{\circ} \mathrm{C}$, what is the specific heat $\left(\mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}\right)$ of copper? (3.5)
Energy and Nutrition
If a $50.0$ -gram piece of copper is heated to $100.0^{\circ} \mathrm{C}$ and then put into a vessel containing $250.0$ milliliters of water at $1.5^{\circ} \mathrm{C}$, what will be the final temperature of the water? Take the molar heat capacity of copper to be $24.4 \mathrm{~J} \cdot \mathrm{K}^{-1} \cdot \mathrm{mol}^{-1}$ and that of $\mathrm{H}_{2} \mathrm{O}(l)$ to be $75.3 \mathrm{~J} \cdot \mathrm{K}^{-1} \cdot \mathrm{mol}^{-1}$
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD