Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol·K) °C heat capacity of H,O(1) 75.3 J/(mol-K) - TOOLS x10 enthalpy of fusion of H,O 6.01 kJ/mol

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Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, Tf, of the water after all the ice melts.
heat capacity of H,0(s)
37.7 J/(mol·K)
Tf =
°C
heat capacity of H,O(1)
75.3 J/(mol-K)
と TOOLS
x10
enthalpy of fusion of H,O
6.01 kJ/mol
Transcribed Image Text:Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,0(s) 37.7 J/(mol·K) Tf = °C heat capacity of H,O(1) 75.3 J/(mol-K) と TOOLS x10 enthalpy of fusion of H,O 6.01 kJ/mol
Expert Solution
Step 1

Given 

System is isolated that means Heat is not transferred from the system on surrounding .

When we mix the both sample 

Then Heat Loss by water = Heat gain by ice  

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