Part B: Observations: Temperature Changes Upon Dissolution of Salts 1/g.C, and t

Question

Part B: Observations: Temperature Changes Upon Dissolution of Salts 1/g.C, and the density of water is Use Table 2 to record your observations for this part of the exercise. (Assume the specific heat of water is 4.18 0.997 g/mL. Enter all masses to two decimal places. Enter all temperatures to one decimal place) Table 2 Mass Ionic Compound C°C) (3/mol) ammonium nitrate 25.02 calcium chloride 23419 6.0 sodium carbonale 16.0 16.72 Check the number of significant figures Provide a Sample Calculation Complete the following sample calculation for andan and '.don for calcium chloride. (The values you enter for your sample calculation should exactly match the corresponding values you entered above.) X Your answer cannot be understood or graded. reintrmation J

Explanation / Answer

Enthalpy calculation

q(reaction) = mCpdT

First row,

m = 5 g

Cp = 4.184 J/g.oC

dT = 10-16 = -6 oC

So,

q(reaction) = 5 x 4.184 x -6 = -125.52 J

dH(reaction) = -(q(reaction)) = -(-125.52) = 125.62 J

moles ammonium nitrate = 5 g/80.043 g/mol

molar mass of ammonium nitrate = 80.043 g/mol

dH(reaction) = 125.52 J/moles of ammonium nitrate

                     = 125.52 J x 80.043 g/mol/5 g

                     = 2009.40 J/mol

Similary other calculations can be performed.

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