Two 20.0 g ice cubes at −15.0 ∘C−15.0⁢ ∘C are placed into 285 g285 g of water at 25.0 ∘C.25.0⁢ ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, ?f,Tf, of the water after all the ice melts.

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Two 20.0 g ice cubes at −15.0 ∘C−15.0⁢ ∘C are placed into 285 g285 g of water at 25.0 ∘C.25.0⁢ ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, ?f,Tf, of the water after all the ice melts.

 
Two 20.0 g ice cubes at –15.0 °C are placed into 285 g of water at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, T¡, of the water after all the ice melts.
heat capacity of H,O(s)
37.7 J/ (mol·K)
heat capacity of H,O(1)
75.3 J/ (mol·K)
Tf =
°C
enthalpy of fusion of H,O
6.01 kJ/mol
Transcribed Image Text:Two 20.0 g ice cubes at –15.0 °C are placed into 285 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T¡, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/ (mol·K) heat capacity of H,O(1) 75.3 J/ (mol·K) Tf = °C enthalpy of fusion of H,O 6.01 kJ/mol
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