Input interpretation
H_2SO_4 (sulfuric acid) + Fe (iron) ⟶ H_2O (water) + SO_2 (sulfur dioxide) + FeSO_4 (duretter)
Balanced equation
Balance the chemical equation algebraically: H_2SO_4 + Fe ⟶ H_2O + SO_2 + FeSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Fe ⟶ c_3 H_2O + c_4 SO_2 + c_5 FeSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Fe: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 2 c_4 + 4 c_5 S: | c_1 = c_4 + c_5 Fe: | c_2 = c_5 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + Fe ⟶ 2 H_2O + SO_2 + FeSO_4
Structures
+ ⟶ + +
Names
sulfuric acid + iron ⟶ water + sulfur dioxide + duretter
Equilibrium constant
![K_c = ([H2O]^2 [SO2] [FeSO4])/([H2SO4]^2 [Fe])](../image_source/fbc8fee315d0d51ee6fd94327cbf4f69.png)
K_c = ([H2O]^2 [SO2] [FeSO4])/([H2SO4]^2 [Fe])
Rate of reaction
![rate = -1/2 (Δ[H2SO4])/(Δt) = -(Δ[Fe])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/53cf45bdd2cbbaaabb39ee6c3599531e.png)
rate = -1/2 (Δ[H2SO4])/(Δt) = -(Δ[Fe])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[FeSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| sulfuric acid | iron | water | sulfur dioxide | duretter formula | H_2SO_4 | Fe | H_2O | SO_2 | FeSO_4 Hill formula | H_2O_4S | Fe | H_2O | O_2S | FeO_4S name | sulfuric acid | iron | water | sulfur dioxide | duretter IUPAC name | sulfuric acid | iron | water | sulfur dioxide | iron(+2) cation sulfate