What quantity of heat is required to melt 2.00 kg of iron at its melting point (1809 K)? For iron, ΔH_fus = 13.80 kJ/mol. A) 0.385 kJ B) 6.90 kJ C) 27.6 kJ D) 494 kJ E) 771 kJ

Question

Quizplus · Accepted Answer

To calculate the heat required to melt iron, we use the following formula:

q = n*ΔHfus

Where:
q = heat required
n = number of moles of iron
ΔHfus = molar enthalpy of fusion

First, we need to calculate the number of moles of iron:

n = mass/molar mass
n = 2.00 kg / (55.85 g/mol)
n = 35.8 mol

Now we can use the formula to calculate q:

q = n*ΔHfus
q = 35.8 mol * 13.80 kJ/mol
q = 494 kJ

Therefore, the heat required to melt 2.00 kg of iron is 494 kJ. The correct answer is (D).

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