A 2.83 g piece of zinc (density = 7.14 g/ml) is added to a graduated cylinder that contains 12.13 ml H2O. What will be the final
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<u>Answer:</u> The enthalpy change of the reaction is -27. kJ/mol
<u>Explanation:</u>
To calculate the mass of water, we use the equation:
Density of water = 1 g/mL
Volume of water = 25.0 mL
Putting values in above equation, we get:
To calculate the heat released by the reaction, we use the equation:
where,
q = heat released
m = Total mass = [1.25 + 25] = 26.25 g
c = heat capacity of water = 4.18 J/g°C
= change in temperature =
Putting values in above equation, we get:
To calculate the number of moles, we use the equation:
Given mass of ammonium nitrate = 1.25 g
Molar mass of ammonium nitrate = 80 g/mol
Putting values in above equation, we get:
To calculate the enthalpy change of the reaction, we use the equation:
where,
q = amount of heat released = -0.428 kJ
n = number of moles = 0.0156 moles
= enthalpy change of the reaction
Putting values in above equation, we get:
Hence, the enthalpy change of the reaction is -27. kJ/mol