Question

The enthalpy of fusion of solid n-butane is 4.66 kJ/mol. Calculate the energy required to melt 58.3 g of solid n-butane.

Answer 1

Answer : The energy required to melt 58.3 g of solid n-butane is, 4.66 kJ

Explanation :

First we have to calculate the moles of n-butane.

`\text{Moles of n-butane}=\frac{\text{Mass of n-butane}}{\text{Molar mass of n-butane}}`

Given:

Molar mass of n-butane = 58.12 g/mole

Mass of n-butane = 58.3 g

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

`\text{Moles of n-butane}=(58.3g)/(58.12g/mol)=1.00mol`

Now we have to calculate the energy required.

`Q=(\Delta H)/(n)`

where,

Q = energy required

`\Delta H` = enthalpy of fusion of solid n-butane = 4.66 kJ/mol

n = moles = 1.00 mol

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

`Q=(4.66kJ/mol)/(1.00mol)=4.66kJ`

Thus, the energy required to melt 58.3 g of solid n-butane is, 4.66 kJ