Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that $\Delta$H_fus = 13.80 kJ/mol. A)494 kJ B)27,600 kJ C)27.6 kJ D)27,600 J E)25,000 kJ

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To calculate the heat needed, use the formula: $ q = n \times \Delta H_{fus} $. First, find the number of moles of iron: $ n = \frac{2000 \, \text{g}}{55.85 \, \text{g/mol}} \approx 35.8 \, \text{mol} $. Then, $ q = 35.8 \, \text{mol} \times 13.80 \, \text{kJ/mol} = 494.04 \, \text{kJ} $.

Calculate the Amount of Heat Needed to Melt 2 Δ\DeltaΔ Hfus = 13

Calculate the Amount of Heat Needed to Melt 2 $\Delta$ H_fus = 13