How much energy is released when 2.55kg of diethyl ether freezes?
You need the latent heat of fusion. You may have been given it with the question.
http://en.wikipedia.org/wiki/Diethyl_ether_(data_page)
has 7.19 kJ mol-1
so calculate the number of moles of diethyl ether relative molecular mass = 74.14
then multiply the number of moles by the latent heat of fusion.
533.0666 kj
How much energy is released when 1.9 kg of diethyl ether freezes? In kj
1. Convert 2.55Kg to g
2.55Kg x 1000g = 2550g
———
1Kg
2. Convert g to mol using the molar mass then multiply the heat of fusion
2550g x 1mol x 7.27KJ = 250 KJ
——— ———-
74.14g 1mol
To determine the amount of energy released when a certain amount of diethyl ether freezes, we need to know the heat of fusion of diethyl ether. The heat of fusion is the amount of energy required to change a substance from a solid to a liquid at its melting point.
Unfortunately, the heat of fusion of diethyl ether is not readily available. However, we can use the heat of fusion of a similar substance as an estimate. The heat of fusion for a typical organic compound is approximately 40 kJ/mol.
To calculate the energy released when 2.55 kg of diethyl ether freezes, we need to convert the mass of diethyl ether into moles. The molar mass of diethyl ether is approximately 74.12 g/mol.
First, convert the mass from kg to grams:
2.55 kg = 2550 grams
Next, calculate the number of moles:
Number of moles = mass / molar mass
Number of moles = 2550 g / 74.12 g/mol
Now, we have the number of moles of diethyl ether. Multiply this by the heat of fusion of a similar compound to find an estimated energy release:
Energy release = (Number of moles) x (heat of fusion)
However, since we don't have the specific heat of fusion for diethyl ether, we cannot provide an accurate value for the energy released.