How much energy is released when 15.3g of steam at 125.0 degress celsius is condensed to give liquid water at 25.0 degrees celsius? Use the constants provided: Delta Hvap enthalpy of vaporization of liquied water is 40.67 kj/mol; Delta Hfus, enthalpy of fusion for ice is 6.02 kj/mol; specific heat capacity for water is 4.184 J/(g * degress celsius); specific heat capacity for vapor is 1.87 J/(g * degrees celsius).

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Asked Oct 17, 2019
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How much energy is released when 15.3g of steam at 125.0 degress celsius is condensed to give liquid water at 25.0 degrees celsius? Use the constants provided: Delta Hvap enthalpy of vaporization of liquied water is 40.67 kj/mol; Delta Hfus, enthalpy of fusion for ice is 6.02 kj/mol; specific heat capacity for water is 4.184 J/(g * degress celsius); specific heat capacity for vapor is 1.87 J/(g * degrees celsius). 

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Expert Answer

Step 1

Determine heat released when temperature is reduced from 125oC to 100oC steam:

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100°C vapor 125°C vapor AT T-T (100°C-125°C)25°C Heat, q mcAT = (15.3 g) x (1.87 J/g°C)x(-25°C) -715.275 J 715.275 J of heat is released when temperature is reduced

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Step 2

Determine heat released during the condensation of steam:

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100°C vapor 100°C water vapor to liquid) Mass Noof moles of H,O = Molar mass 15.3 g = 0.849 mol 11 18.02 g/mol [AHndA 0.849 mol x (-40.67 x 103 kJ/g = -AHap Heat, q, nAH ΔΗ, cond cond = -34528.83 J 34528.83 J heat is released during condensation.

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Step 3

Determine heat released when temperature is reduced f...

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