Challenge Problem!!! Two 20.0 g ice cubes at -11.0 °C are placed into 245 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 H₂O(s) heat capacity of H₂O(1) 37.7 J/(mol·K) 75.3 J/(mol-K) T₁ = enthalpy of fusion of H₂O 6.01 kJ/mol C

What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water at 100C is 40.66 kJ/mol.

he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?

(a) If 83.0 g of ice at 0.0oC is placed in 235mL of water at 28.0oC, find the final temperature of water when all of the ice melts.  DHfus=6.01 kJ/mol and assume for liquid water density= 1.00 g/mL        HINT: you have two parts to find the heat.(remember that the heat lost must equal the heat gained). Part a- find the heat for 83 g of ice melting and then the heat for the liquid to warm up Part b- find the heat for 235 mL H2O to cool down   (b) What is the interpretation/finding from this problem?

Two 20.0 g ice cubes at -20.0 °C are placed into 245 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 H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol T₁ = °C

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Two 20.0 g ice cubes at -20.0 °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 H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol T₁ = 51.35 Incorrect

Two 20.0 g ice cubes at -20.0 °C are placed into 245 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 H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Tf = x10 TOOLS °C

Two 20.0 g ice cubes at -20.0 °C are placed into 295 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 H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Tf = 17.25 Incorrect °C

Two 20.0 g ice cubes at -18.0 C are placed into 225 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) heat capacity of H, O(1) T = 21.1598 75.3 J/(mol-K) "C enthalpy of fusion of H,0 6.01 kJ/mol Incerrect