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°_rxn = - 24.8 kJ/mol, A)0.699 kJ B)2.10 kJ C)17.9 kJ D)24.8 kJ E)112 kJ

Question

Quizplus · Accepted Answer

Explanation:The balanced chemical equation is:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)ΔH°rxn = -24.8 kJ/molTo calculate the heat evolved, we need to use the following formula:Heat evolved = -ΔH°rxn × moles of Fe2O3First, we need to convert the mass of Fe2O3 to moles:moles of Fe2O3 = 4.50 g / 159.69 g/mol = 0.0282 molNow we can calculate the heat evolved:Heat evolved = -(-24.8 kJ/mol) × 0.0282 mol = 0.699 kJTherefore, the correct answer is A) 0.699 kJ.

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)