Posted by **Matthew** on Monday, December 5, 2011 at 1:29pm.

Calculate the heat (in kJ) required to transform 58.60 g of dinitrogen tetraoxide from a solid at a

temperature of -9.3 °C to a gas at 47 °C. Report your answer to one decimal place. Data:

Molar mass of dinitrogen tetraoxide, N2O4

= 92.011 g/mol

Melting point = -9.3 °C Boiling point = 21°C.

Enthalpy of fusion = 14.65 kJ/mol

Enthalpy of vaporization = 38.12 kJ/mol.

Molar heat capacity of the liquid phase = 142.7 J/mol•K

Molar heat capacity of the gas phase= 77.3 J/mol•K

- Chemistry -
**DrBob222**, Monday, December 5, 2011 at 1:35pm
Here is how you do it.

For temperature changes in the same phase( all solid, all liquid, all gas),

q = mass x specific heat in that phase x (Tfinal-Tinitial).

For changing phases (from solid to liquid of liquid to gas),

q = mass x heat fusion (at melting point)

q = mass x heat vaporization (at boiling point)

Then add each q together to arrive at the total Q from the starting point to the ending point.

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