1.00 kg of ice at -10 °c is heated using a bunsen burner flame until all the ice melts and the temperature reaches 95 °c. a) how much energy in kj is required to effect this transformation?

Answer : The energy required is, 574.2055 KJ

Solution :

The conversions involved in this process are :

Now we have to calculate the enthalpy change or energy.

where,

= energy required = ?

m = mass of ice = 1 kg  = 1000 g

= specific heat of solid water =

= specific heat of liquid water =

n = number of moles of ice =

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

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

    (1 KJ = 1000 J)

Therefore, the energy required is, 574.2055 KJ

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