provide a proof of spontaneity of the following reaction
4Fe(s)+ 3O2(g)->2Fe2O3(s)
4Fe(s) + 3O2(g) -------> 2Fe2O3(s)
delta G0rkn = 2*(delta G0f Fe2O3) - 4*(delta G0f Fe) - 3*(delta G0f O2) = -2*(-741.0) - 4*(0) - 3*(0) = -1482 kJ
Since, delta G0rkn < 0 ; therefore the reaction is spontaneous.
provide a proof of spontaneity of the following reaction 4Fe(s)+ 3O2(g)->2Fe2O3(s)
4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Determine the number of electrons transferred for 1 g of fe (s) reacted
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 14.2 g of iron (Fe) is reacted with 18.1 g of oxygen (O2). Select the limiting reagent. Fe2O3 O2O2 FeFe Calculate the theoretical yield of iron(III) oxide (Fe2O3Fe2O3). theoretical yield = The reaction produces 5.40 g of Fe2O3. What is the percent yield of the reaction? percent yield =
Separate this redox reaction into its component half-reactions. 3O2 + 4Fe ---> 2Fe2O3 Oxidation half-rxn? Reduction half-rxn?
Consider the reaction, 4Fe+3O2-->2Fe2O3. could you correctly represent 3 molecules of oxygen as (O2)3? Explain your answer.
Separate the redox reaction into its component half‑reactions. 3O2+4Fe⟶2Fe2O3 Can you please include step by step explanation?
Calculate the enthalpy of reaction for the following reaction: 2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol ΔHfo(C(s)) = ? ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5 kJ/mol
Consider the following reaction. 2Fe2O3(s)+3C(s)−heat→−4Fe(s)+3CO2(g) Calculate the number of grams of Fe2O3 needed to react with 12.0 g C.
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...
Calculate ΔSo in J/K for the following reaction: 2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g) So(Fe2O3(s)) = 87.4 J/K/mol So(C(s)) = 5.7 J/K/mol So(Fe(s)) = 27.3 J/K/mol So(CO2(g)) = 213.7 J/K/mol
Consider the reaction: 4Fe(s) + 3O2(g) à2Fe2O3(s) DHo= -1652 kJHow much heat is involved in the process if 25.6 g of Fe(s) reacts with 13.5 g of O2(g)