A 245.7 g sample of metal at 75.2^C was placed in 115.43 g water at 22.6^C. The final temperature of the water and metal was 34.6^C. If no heat was lost to the surroundings what is the specific heat of the metal? Specific heat of water is 4.18 J/g^C.
Added by Vicente G.
Step 1
The formula for heat gained or lost is: \[ q = m \cdot c \cdot \Delta T \] Where: - \( q \) = heat (in joules) - \( m \) = mass (in grams) - \( c \) = specific heat capacity (in J/g°C) - \( \Delta T \) = change in temperature (in °C) For water: Show more…
Show all steps
Your feedback will help us improve your experience
Madhur L and 74 other Chemistry 101 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
Madhur L.
A 245.7 g sample of metal at 75.2 °C was placed in 115.43 g water at 22.6°C. The final temperature of water and metal was 34.6 °C. If no heat was lost to surrounding, what is the specific heat of the metal? [580.99 J/kg. °C]
Satyaki I.
When 18.0 g of an unknown metal at 79.0 ºC is placed in 112 g H2O at 22.2 ºC, the final temperature of the water is 24.9 ºC. What is the specific heat capacity of the metal? The specific heat of water is 4.184 J/g °C.
Shalini T.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD