Chemistry 11 Learning Check How much energy (in kJ), is released when 1.80 g of steam...
How much energy (in kilojoules) is released when 12.6 g of steam at 110.5 ∘C is condensed to give liquid water at 67.0 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor.
1. How much energy (in kilojoules) is released when 16.4 g of steam at 116.5 ∘C is condensed to give liquid water at 60.5 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor. 2.What is the entropy of fusion, ΔSfusion [in J/(K⋅mol)] for sodium? The necessary data are the following: mp = 97.8 ∘C,bp = 883 ∘C, ΔHvap = 89.6kJ/mol, and...
How much heat (in kJ) is released when 125.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).
How much heat is released when 105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol • °C), and the molar heat capacity of ice is 36.4 J/(mol • °C). A)347 kJ B)54.8 kJ C)319 kJ D)273 kJ
how much heat is released when 10.0 g of steam (water vapor ) at 105.0 C is cooled to liquid water at 25 C? S(water) = 4.18 J/g.C. ... S(steam) = 2.01 j/ g.C the heat of fusion of water is 6.02 KJ/ mol. The heat of vaporization of water is 40.7 KJ/mol
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05 kg of water decreased from 121 °C to 43.5 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfusΔHfus 6.01 kJ/mol ΔHvapΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol ·°C cp (l) 75.3 J/mol ·°C cp (g) 33.6 J/mol ·°C
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.550 kg of water decreased from 109 °C to 38.5 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.850 kg of water decreased from 123 °C to 54.5 °C. Value 0 Property Melting point Boiling point Alfus Units С °C kJ/mol 100.0 6.01 40.67 37.1 AHvap kJ/mol Co (s) J/mol · °C coln 75.3 J/mol · °C J/mol · °C Cp (g) 33.6
5) How much heat is required to convert 0.05kg of water at 298 K to super-steam at 423 K. The boiling point of water is 373 K. Cm [H2O (l)] = 75.4 J/(mol. ℃) Cm [H2O (g)] = 33.6 J/(mol. ℃) ΔHvap = 40.67 75.4 J/mol
5. If 100 g of water cooled to -6°C) is allowed to freeze at -6°C, what is the entropy change? What is the entropy change of the surroundings? What is the entropy change of the universe? H2O() → H2O(1) AH = 6.008 kJ/mol Cp,solid = 33.8 J/(K mol) Cp.liquid = 75.3 J/(K mol)