A hot lump of 33.8 g of iron at an initial temperature of 51.8 C is placed in 50.0 mL H,0 initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g-°C)? Assume no heat is lost to surroundings. °C Trinal %3D

A hot lump of 33.8 g of iron at an initial temperature of 51.8 C is placed in 50.0 mL H,0 initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g-°C)? Assume no heat is lost to surroundings. °C Trinal %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 64E: A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed...

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