Question

The chemical reaction that causes iron to corrode in air is given by 4Fe(s)+3O2(g)→2Fe2O3(s) 4 F e ( s ) + 3 O 2 ( g ) → 2 F e 2 O 3 ( s ) and ΔrH∘ Δ r H ∘ = −1684 kJ mol−1 = − 1684 k J m o l − 1 ΔrS∘ Δ r S ∘ = −543.7 J K−1 mol−1 = − 543.7 J K − 1 m o l − 1

part a: What is the standard Gibbs energy change for this reaction? Assume the commonly used standard reference temperature of 298 K K . Express your answer as an integer and include the appropriate units.

part b: What is the Gibbs energy for this reaction at 3652 K K ? Assume that ΔrH∘ Δ r H ∘ and ΔrS∘ Δ r S ∘ do not change with temperature. Express your answer to two decimal places and include the appropriate units.

part c: The standard Gibbs energy change, ΔrG∘ Δ r G ∘ , applies only when the reactants and products are in their standard states. Assume that the above corrosion reaction is carried out in a flask where the reactants and products are in their standard states and the values of ΔrH∘ Δ r H ∘ and ΔrS∘ Δ r S ∘ do not change with temperature. At what temperature, Teq T e q , do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units.

Answer 1

Given data: AH = -1684 kJ molt osº = -543.7 J K' molt = -0.5437 KJ Ki molt Paret a At T = 298K SG=AH-TAS = -1684 - (298x-0.5437) TAG = - 1521.98 kJ mol Part b At T = 3652K BG = DH - TAS 2-1684-(3652% -0.5437) DG = 301.59 kJ mol! Parte For Teq, AG=0 до = Дн°-тд." => O = DHO - TOS =) DH =TAS - T=AH = -1684 AS -0.5437 =T= 3097.3K