Four ice cubes at exactly 0°C with a total mass of 53.5 g are combined with 115 g of water at 75°C in an insulated container.If no heat is lost to the surroundings, what is the final temperature of the mixture?

Two 20.0 g ice cubes at -14.0 °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= °C

An 8.7- g ice cube is placed into 275 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water and that the ice cube has a temperature of 0 ∘C .

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, T;, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol·K) Tf = heat capacity of H,O(l) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 kJ/mol

Two 20.0 g ice cubes at -18.0 °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 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 = °C

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Ice actually has negative caloric content. How much energy, in each of the following units, does your body lose from eating (and therefore melting) 67 g of ice? Heat of fusion for water is 6.02 kJ/mol. Express your answer in joules .

The standard enthalpy of fusion of silver at 1234 K is 11.30 kJ/mol. How much energy, in kJ, is required to completely melt 283.67 g of silver at 1234K? Report your answer to two decimal places. Do not include units in your response.

How much heat is required to convert 42.0 g of ethanol at 20 ∘C to the vapor phase at 78 ∘C?