Question
Asked Feb 11, 2020
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166. 40.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 20.0°C in a
coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss
or gain from the surroundings. (Data: specific heat capacity of H20(1), c = 4.18 J/g.°C;
H2O(s) → H2O(1)
A) 0.0
%3D
НаО()
B) 10.6
AH= 6.02 kJ/mol)
C) 30.7 D) 43.2 E) 56.4
%3D
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166. 40.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 20.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H20(1), c = 4.18 J/g.°C; H2O(s) → H2O(1) A) 0.0 %3D НаО() B) 10.6 AH= 6.02 kJ/mol) C) 30.7 D) 43.2 E) 56.4 %3D

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Expert Answer

Step 1

The molar mass of water is 18.015 g/mol. The number of moles of water in the 40.0 g sample is calculated below.

Chemistry homework question answer, step 1, image 1

Step 2

The heat needed to change from solid at 0C to liquid at 0C is calculated below.

Chemistry homework question answer, step 2, image 1

Step 3

The heat lost by water is calculated below.

Chemistry homework question answer, step 3, image 1

...

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