How much heat is emitted when 4.55 g of water condenses at 25 degrees C? The heat of vaporization of water at 25 ∘C is 44.0 kJ/mole KJ/mole.
q= kJ
How much heat is emitted when 4.55 g of water condenses at 25 degrees C? The...
Suppose that 0.94 g of water condenses on a 85.0 g block of iron that is initially at 21 degrees Celsius. If the heat released during condensation goes only to warming the iron block, what is the final temperature,(in Celsius) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol.)
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
Suppose that 0.92 g of water condenses on a 85.0 g block of iron that is initially at 24 ∘C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in ∘C) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol.)
Part B Suppose that 0.48 g of water at 25° C condenses on the surface of a 55-g block of aluminum that is initially at 25°C. If the heat released during condensation goes only toward heating the metal, what is the final temperature (in degrees Celsius) of the metal block? (The specific heat capacity of aluminum, Cs,A1, is 0.903 J/(g. °C).) Express your answer in degrees Celsius to two significant figures. IVO ΑΣφ ? T = 22 C Submit Previous...
Suppose that 0.95 gg of water condenses on a 85.0 gg block of iron that is initially at 21 ∘C∘C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in ∘C) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol and a heat capacity for iron of 0.449 J⋅g−1⋅∘C−1.)
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).
Calculate the heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C. DHvap(water) = 40.66 kJ/mol.
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
suppose that 0.95g of water condenses on a 75.0g block of iron that is initially at 22 degree Celsius.if the heat released goes in to only warming the iron block.what is the final temperature of the iron block in degree Celsius.(assume the heat of enthalpy of vaporization for water of 44.0 kj/mol.
the heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 2.88 g of water boils at atmospheric pressure? ____kJ (show wrk)