H2SO4 + H2O2 + MgI2 = H2O + I2 + MgSO4

Input interpretation

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H_2SO_4 sulfuric acid + H_2O_2 hydrogen peroxide + MgI_2 magnesium iodide ⟶ H_2O water + I_2 iodine + MgSO_4 magnesium sulfate

Balanced equation

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Balance the chemical equation algebraically: H_2SO_4 + H_2O_2 + MgI_2 ⟶ H_2O + I_2 + MgSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2O_2 + c_3 MgI_2 ⟶ c_4 H_2O + c_5 I_2 + c_6 MgSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, I and Mg: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 2 c_2 = c_4 + 4 c_6 S: | c_1 = c_6 I: | 2 c_3 = 2 c_5 Mg: | c_3 = c_6 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + H_2O_2 + MgI_2 ⟶ 2 H_2O + I_2 + MgSO_4

+ + ⟶ + +

Names

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sulfuric acid + hydrogen peroxide + magnesium iodide ⟶ water + iodine + magnesium sulfate

Equilibrium constant

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Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2O_2 + MgI_2 ⟶ H_2O + I_2 + MgSO_4 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: H_2SO_4 + H_2O_2 + MgI_2 ⟶ 2 H_2O + I_2 + MgSO_4 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2SO_4 | 1 | -1 H_2O_2 | 1 | -1 MgI_2 | 1 | -1 H_2O | 2 | 2 I_2 | 1 | 1 MgSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) H_2O_2 | 1 | -1 | ([H2O2])^(-1) MgI_2 | 1 | -1 | ([MgI2])^(-1) H_2O | 2 | 2 | ([H2O])^2 I_2 | 1 | 1 | [I2] MgSO_4 | 1 | 1 | [MgSO4] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([H2SO4])^(-1) ([H2O2])^(-1) ([MgI2])^(-1) ([H2O])^2 [I2] [MgSO4] = (([H2O])^2 [I2] [MgSO4])/([H2SO4] [H2O2] [MgI2])

Rate of reaction

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Construct the rate of reaction expression for: H_2SO_4 + H_2O_2 + MgI_2 ⟶ H_2O + I_2 + MgSO_4 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: H_2SO_4 + H_2O_2 + MgI_2 ⟶ 2 H_2O + I_2 + MgSO_4 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2SO_4 | 1 | -1 H_2O_2 | 1 | -1 MgI_2 | 1 | -1 H_2O | 2 | 2 I_2 | 1 | 1 MgSO_4 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) MgI_2 | 1 | -1 | -(Δ[MgI2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) MgSO_4 | 1 | 1 | (Δ[MgSO4])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[H2SO4])/(Δt) = -(Δ[H2O2])/(Δt) = -(Δ[MgI2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[I2])/(Δt) = (Δ[MgSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)