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.
[tex]\text{Moles of n-butane}=\frac{\text{Mass of n-butane}}{\text{Molar mass of n-butane}}[/tex]
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:
[tex]\text{Moles of n-butane}=\frac{58.3g}{58.12g/mol}=1.00mol[/tex]
Now we have to calculate the energy required.
[tex]Q=\frac{\Delta H}{n}[/tex]
where,
Q = energy required
[tex]\Delta H[/tex] = 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:
[tex]Q=\frac{4.66kJ/mol}{1.00mol}=4.66kJ[/tex]
Thus, the energy required to melt 58.3 g of solid n-butane is, 4.66 kJ
