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) 27,600 J B) 27.6 kJ C) 494 kJ D) 25,000 kJ E) 27,600 kJ

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To calculate the heat needed to melt 2.00 kg of iron at its melting point, we use the formula $q = n\Delta H_{fus}$, where $q$ is the heat required, $n$ is the number of moles, and $\Delta H_{fus}$ is the heat of fusion. First, we convert the mass of iron to moles using its molar mass (approximately 55.85 g/mol for iron): $2000 \, \text{g} \div 55.85 \, \text{g/mol} = 35.8 \, \text{mol}$. Then, we multiply the number of moles by the heat of fusion (given as 13.80 kJ/mol): $35.8 \, \text{mol} \times 13.80 \, \text{kJ/mol} = 494 \, \text{kJ}$.

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