The heat required to melt the compound is 2.56kJ.
Why?
To calculate the heat required to melt 25.7 g of solid methanol, we need to calculate its molar mass, know its chemical formula, its molar heat of fusion, and calculate how many moles represent 25.7g of the same compound.
Then, we need to use the following formula to calculate the heat:
[tex]Q=N*u[/tex]
Where,
N is the moles of the compound
u, is the molar heat of fusion of the compound (J/mol)
We know that the molar mass of methanol is :
[tex]32.042\frac{g}{mol}[/tex]
So, we can calculate the number of moles that represents 25.7g of the same compound:
[tex]N=\frac{mass(g)}{molarmass(\frac{g}{mol}} \\\\N=\frac{25.7g}{32.042\frac{g}{mol}}=0.8mol(methanol)[/tex]
Also, the molar heat of fusion of methanol is:
[tex]u_{methanol}=3200\frac{J}{mol}=3.2\frac{kJ}{mol}[/tex]
Now, substituting into the first equation and calculating, we have:
[tex]Q=N*u[/tex]
[tex]Q=0.8mol*3.2\frac{kJ}{mol}=2.56kJ[/tex]
Hence, we have that the heat required to melt the compound is 2.56kJ.
Have a nice day!
We have that for the Question,it can be said that the heat required to melt 25.7 g of solid methanol at its melting point is
Q=2.6kJ
From the question we are told
Calculate the heat required to melt 25.7 g of solid methanol at its melting point
Generally the equation for Heat is mathematically given as
Q=N*u
Where
mass of methanol is 32.04g/mol
molar heat of fusion of methanol is 3200J/mol
Therefore
number of moles in 25.7g
n=\frac{ 25.7g}{32.04}
n=0.8mol
Hence
the heat required to melt 25.7 g of solid methanol at its melting point is
Q=0.8*3.2
Q=2.6kJ
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