Calculate the amount of heat energy in kj required to convert 45.0 g of ice at -15.5'c to steam at 124.0°c. (cwater 118 jig'c, gee 2.03 jig c, g team jig c, molar heat of fusion of ice 6.01 * 10 j/mol; molar heat of vaporization of liquid water 4.07 * 10*j/mol 202 short answer toolbar navigation b i v s e 1 e a a this question will be sent to your instructor for grading

Answer : The enthalpy change or heat required is, 139.28775 KJ

Solution :

The conversions involved in this process are :

Now we have to calculate the enthalpy change.

where,

= enthalpy change or heat required = ?

m = mass of water = 45 g

= specific heat of solid water =

= specific heat of liquid water =

= specific heat of liquid water =

n = number of moles of water =

= enthalpy change for fusion = 6.01 KJ/mole = 6010 J/mole

= enthalpy change for vaporization = 40.67 KJ/mole = 40670 J/mole

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

    (1 KJ = 1000 J)

Therefore, the enthalpy change is, 139.28775 KJ

answer: your mm

explanation:

the millers tale is the answer.