The molar heat of fusion of iron is #14.9# kJ/mol. What is the energy (in kJ) needed to melt #4.50g# of iron?
The energy needed is
We make a table:
Therefore to melt down the 4.50 gram of iron we need 1.20 kJ energy.
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To calculate the energy needed to melt 4.50 grams of iron, you can use the formula:
Energy = (mass * molar heat of fusion) / molar mass
First, convert the mass of iron from grams to moles using the molar mass of iron (Fe), which is approximately 55.85 g/mol.
Number of moles = mass / molar mass Number of moles = 4.50 g / 55.85 g/mol ≈ 0.0805 mol
Now, use the molar heat of fusion of iron (14.9 kJ/mol) to calculate the energy needed:
Energy = (0.0805 mol * 14.9 kJ/mol) / 1 mol Energy ≈ (1.19545 kJ) / 1 mol ≈ 1.20 kJ
Therefore, the energy needed to melt 4.50 grams of iron is approximately 1.20 kJ.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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