How much heat (kJ) is evolved when 4.50 g of Fe₂O₃ is reacted with excess carbon monoxide using the equation below?
Fe₂O₃(s) + 3CO(g) $\rarr$ 2 Fe(s) + 3 CO₂(g) $\Delta$ H^$\circ$_rxn = - 24.8 kJ/mol,

Question

How much heat (kJ) is evolved when 4.50 g of Fe₂O₃ is reacted with excess carbon monoxide using the equation below?
Fe₂O₃(s) + 3CO(g)

\rarr

2 Fe(s) + 3 CO₂(g)

\Delta

H^$\circ$_rxn = - 24.8 kJ/mol,

Quizplus · Accepted Answer

The correct answer is calculated by first determining the molar mass of FeS2 (pyrite), which is approximately 120 g/mol. Given 4.50 g of FeS2, this is equivalent to 4.50 g / 120 g/mol = 0.0375 mol. Since the reaction releases -24.8 kJ/mol, the total heat evolved for 0.0375 mol is 0.0375 mol * -24.8 kJ/mol = -0.93 kJ. However, due to the choices provided, it seems there might have been a calculation or transcription error in the question or answer choices. The closest correct choice based on the calculation method is 0.699 kJ, but this does not match the calculated value. Please ensure the values and choices are accurate.

How Much Heat (KJ) Is Evolved When 4 →\rarr→ 2 Fe(s) + 3 CO2(g)

How Much Heat (KJ) Is Evolved When 4 $\rarr$ 2 Fe(s) + 3 CO₂(g)