. (a) We place 77.7 g of a metal at 10.00 ◦C in 333.3 g of water at 70.00 ◦C. The water is in a beaker that is also at 70.00 ◦C. The specifific heat capacity of water is 4.184 J K−1 g−1 and that of the metal is 0.555 J K−1 g−1 . The heat capacity of the beaker is 0.666 kJ K−1 . What is the fifinal temperature of the metal, the water, and the beaker?
. (a) We place 77.7 g of a metal at 10.00 ◦C in 333.3 g of water at 70.00 ◦C. The water is in a beaker that is also at 70.00 ◦C. The specifific heat capacity of water is 4.184 J K−1 g−1 and that of the metal is 0.555 J K−1 g−1 . The heat capacity of the beaker is 0.666 kJ K−1 . What is the fifinal temperature of the metal, the water, and the beaker?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g...
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7. (a) We place 77.7 g of a metal at 10.00 ◦C in 333.3 g of water at 70.00 ◦C. The water is in a
beaker that is also at 70.00 ◦C. The specifific heat capacity of water is 4.184 J K−1 g−1 and that of
the metal is 0.555 J K−1 g−1 . The heat capacity of the beaker is 0.666 kJ K−1 . What is the fifinal
temperature of the metal, the water, and the beaker?
(b) Calculate the enthalpy change for the reaction C(graphite) + 2 H2(g) → CH4(g) with the
help of the enthalpy changes of the following reactions:
C(graphite) + O2(g) → CO2(g) ∆H= -393.5 kJmol−1
H2(g) +1/2O2(g) → H2O(l) ∆H = -285.8 kJmol−1
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.4 kJmol−1
The temperature is 25 ◦C in all instances.
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