A 192 g piece of copper is heated to 100.0 deg C and then droppedinto a coffee-c
ID: 675881 • Letter: A
Question
A 192 g piece of copper is heated to 100.0 deg C and then droppedinto a coffee-cup calorimeter containing 750.0 mL of water at 4.0deg C. What is the final temperature (in degrees C) of the copperand water after they come to thermal equilibrium? (Assume that noheat is lost to the surroundings and that the density of water is1.00 g/mL. Also, the specific heat of water is 4.184 J/g-deg C, andthe specific heat of copper is 0.385 J/g-deg C.)a. 15.2
b. 77.1
c. 38.6
d. 22.8
e. 6.2
Explanation / Answer
A 192 g piece ofcopper is heated to 100.0 deg C and then dropped into a coffee-cupcalorimeter containing 750.0 mL of water at 4.0 deg C. What is thefinal temperature (in degrees C) of the copper and water after theycome to thermal equilibrium? (Assume that no heat is lost to thesurroundings and that the density of water is 1.00 g/mL. Also, thespecific heat of water is 4.184 J/g-deg C, and the specific heat ofcopper is 0.385 J/g-deg C.) a. 15.2 b. 77.1 c. 38.6 d. 22.8 (e)6.2 EXPLANATION: {Heat Lost By Copper Object} = {Heat Gained ByWater} ----> (m_copper)*(C_copper)*(T_copper) = (m_water)*(C_water)*(T_water) ----> (192 g)*(0.385)*((100) -(T_final)) = (750 g)*(4.184)*((T_final) - (4)) ----> (73.92)*((100) - (T_final)) = (3138)*((T_final) - (4)) ----> (T_final) = 6.21degC .
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