If the literature value for the ΔHfus of water is 6.01 kJ/mol, how many kJ of heat energy would be required to completely melt 130 g of ice at 0°C?
mols Ice = 130g/molar mass H2O
mols ice x 6.01 kJ/mol = ? kJ.
43 but not sure how
To calculate the heat energy required to completely melt 130 g of ice at 0°C, we can use the equation:
q = m × ΔHfus
where:
q = heat energy (in kJ)
m = mass of ice (in grams)
ΔHfus = heat of fusion of water (in kJ/mol)
First, we need to convert the mass of ice from grams to moles. We can use the molar mass of water (18.015 g/mol) to do this.
130 g ÷ 18.015 g/mol = 7.216 mol
Now, we can calculate the heat energy required:
q = 7.216 mol × 6.01 kJ/mol
q = 43.401 kJ
Therefore, approximately 43.401 kJ of heat energy would be required to completely melt 130 g of ice at 0°C.
To calculate the amount of heat energy required to completely melt a given mass of ice, you can use the equation:
q = m × ΔHfus
where:
q is the heat energy (in joules or kilojoules),
m is the mass of the substance being melted (in grams or moles), and
ΔHfus is the enthalpy of fusion for the substance (in joules or kilojoules per gram or mole).
In this case, we are given the mass of ice, 130 g, and the literature value for the enthalpy of fusion of water, 6.01 kJ/mol.
First, let's convert the mass of ice from grams to moles. To do this, we need to know the molar mass of water, which is approximately 18.015 g/mol.
moles = mass (g) / molar mass (g/mol)
moles = 130 g / 18.015 g/mol ≈ 7.212 mol
Now that we have the number of moles, we can use the equation to calculate the heat energy required:
q = m × ΔHfus
q = 7.212 mol × 6.01 kJ/mol
q ≈ 43.337 kJ
Therefore, approximately 43.337 kJ of heat energy would be required to completely melt 130 g of ice at 0°C.