Ammonium nitrate is soluble in water. 16.50 g of ammonium nitrate is added to an

Question

Ammonium nitrate is soluble in water. 16.50 g of ammonium nitrate is added to an adiabatic calorimeter containing 100.0 g of water initially at 22.0 degree C. The final temperature of the solution is 14.1 degree C. Assuming the heat capacity of the solution is 4.08 J/g degree C, calculate the molar enthalpy of solvation of ammonium nitrate. Using the table of thermodynamic values at the back of your textbook, calculate the theore value of the molar enthalpy of solvation. Calculate the percent error for this experimental result.

Explanation / Answer

Let the molar enthalpy of solvation of (NH4)(NO3) be X.

Then by an energy balance;

116.5 * (4.08) *(14.1 - 22) - X * 16.5 = 0
Hence;

X = -227.577 J/mol

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