Question
When 3.2 g of ammonium chloride is dissolved in 75 g of water, the temperature of the solution decreases from 22.8°C to 20.1°C. What is the energy of dissolution of NH4Cl per mole? (The molecular mass of NH4Cl = 53.49 g/mol, and the specific heat of water = 4.18 J/g°C.)
A. 14.8 kJ/mol
B. 0.88 kJ/mol
C. 390 kJ/mol
D. 125 kJ/mol
A. 14.8 kJ/mol
B. 0.88 kJ/mol
C. 390 kJ/mol
D. 125 kJ/mol
Answers
Dissolving NH4Cl in H2O is an endothermic solution process. You measure how much it cools the solution by the temperature of the H2O.
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
The q you measure is for 3.2g/53.4g or q/0.0599 mol. You want to convert that to q/1 mol.
Did you get the Ni/water problem straightened out? I think about 21 (answerD) was the right one? unless I'm not remembering right.
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
The q you measure is for 3.2g/53.4g or q/0.0599 mol. You want to convert that to q/1 mol.
Did you get the Ni/water problem straightened out? I think about 21 (answerD) was the right one? unless I'm not remembering right.
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24.8
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