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oogle Chrome yct/itemView?offset-next&assignmentProblemlD-88441813; nhanced - with Feedback Resources « previous | 8 of 13 |next Part A Calculate the change in enthalpy for the reaction. (Use 1.0 g/mL as the density of the solution and 4.18 J/(g. °C) as the specific heat capacity.) Express the enthalpy change in kilojoules per mole to two significant figures. 0 k.J/mol Submit My Answers Give Up Incorrect; Try Again You have calculated the heat of the reaction (arx.) in kilojoules, but you should report the change in enthalpy in kilojoules per mole. Use the given mass of ammonium nitrate and its

Explanation / Answer

6.76

heat absorbed dH = -mCpdT

m = 25 ml x 1 g/ml + 1.25 g = 26.25 g

Cp = 4.18 J/g.oC

dT = 21.9 - 25.8 = -3.9 oC

So,

dH = -(26.25 x 4.18 x -3.9) = 428 J

moles of NH4NO3 = 1.25 g/80.043 g/mol = 0.01562 mol

So,

enthalpy change (kJ/mol) = 428/0.01562 x 1000 = 27.41 kJ/mol

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