In order to measure the enthalpy change for this reaction, 1.25 g of nh4no3 is dissolved in enough water to make 25.0 ml of solution. the initial temperature is 25.8 degrees c and the final temperature (after the solid dissolves) is 21.9 degrees c. calculate the change in enthalpy for the reaction. (use 1.0g/ml as the density of the solution and 4.18 j/g . degrees c as the specific heat capacity.) express the answer to two significant figures.

The change in enthalpy for the reaction is 27 kJ/mol.

Explanation:

Volume of the solution = v = 25.0 mL

Mass of the solution = m

Density of the solution = d = 1.0 g/mL

Heat capacity of the solution = C = 4.18 J/g°C

The initial temperature of solution, = 25.8°C

The final temperature of solution,  = 21.8°C

Heat loss of the solution = Q

Negative sign indicates that energy is released by the solution.

Energy gained by the ammonium nitrate  = Q'

Q'= -Q = 418 J (Conservation of energy)

Mass of ammonium nitrate = 1.25 g

Moles of ammonium nitrate ,n=

Enthalpy change of reaction =

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