Given that the heat of fusion of water is +6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -15 ∘C. Express your answer using two significant figures.
deltaH= ___?____ kJ/mol
heat capacity of H2O(l) = 75.2 J/mol⋅K = 0.0752 kJ/ mol.K
heat capacity of H2O(s) = 37.7 J/mol⋅K = 0.0377 kJ/ mol K
heat of fusion = -6.02 kJ / mole ( liquid to solid heat releases ) it is at 0oC
at -15 ∘C heat of fusion = -6.02 - (-15 x (0.0752 -0.0377 ))
= -6.02 + 0.5625
= -5.46 kJ
heat of fusion of water at -15∘C = - 5.5 kJ
Given that the heat of fusion of water is +6.02 kJ/mol, that the heat capacity of...
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -13 ∘C.
Given that the heat of fusion of water is 6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J>mol · K, and that the heat capacity of H2O(s) is 37.7 J/mol · K, calculate the heat of fusion of water at – 10 °C.
Given that the heat of fusion of water is +6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -14 ∘C.
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Two 20.0 g ice cubes at -12.0 °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 H2O(s) heat capacity of H2O(1) enthalpy of fusion of H,O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti =