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.

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:

Now we have to calculate the energy required.

where,
Q = energy required
= 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:

Thus, the energy required to melt 58.3 g of solid n-butane is, 4.66 kJ
Because all the compounds are at the same concentration, the one that can produce more particles in solution will be the one that will raise the boiling point the most.
<span>A. 2.0 M (NH4)3PO4 will produce 4 particles per molecule formula</span>
What subject is this again ? If I know now then I would have a better understanding of what I’m gonna answer so you don’t get it wrong !
Answer:
geruow0irghvn3p0unhie0ghik
Explanation: