Based on the thermodynamic properties provided for water, determine the amount of energy released for 155.0 g of water to go from 39.0 °c to -36.5°c. property melting point boiling point ahfus ahvap cp (s) value 0.0 100.0 6.01 40.67 37.1 75.3 33.6 units oc kj/mol kj/mol j/mol. oc j/mol c mol oc cp (g)

Answer : The amount of energy released will be, -88.39 kJ

Solution :

The process involved in this problem are :

The expression used will be:

where,

= heat available for the reaction = ?

m = mass of water = 155.0 g

= specific heat of solid water =

= specific heat of liquid water =

= enthalpy change for fusion =

Molar mass of water = 18 g/mole

Now put all the given values in the above expression, we get:

Therefore, the amount of energy released will be, -88.39 kJ

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.