H2SO4 + KMnO4 + NH4I = H2O + K2SO4 + I2 + MnSO4 + (NH4)2SO4

H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + NH_4I ammonium iodide ⟶ H_2O water + K_2SO_4 potassium sulfate + I_2 iodine + MnSO_4 manganese(II) sulfate + (NH_4)_2SO_4 ammonium sulfate

Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + NH_4I ⟶ H_2O + K_2SO_4 + I_2 + MnSO_4 + (NH_4)_2SO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 NH_4I ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 I_2 + c_7 MnSO_4 + c_8 (NH_4)_2SO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn, I and N: H: | 2 c_1 + 4 c_3 = 2 c_4 + 8 c_8 O: | 4 c_1 + 4 c_2 = c_4 + 4 c_5 + 4 c_7 + 4 c_8 S: | c_1 = c_5 + c_7 + c_8 K: | c_2 = 2 c_5 Mn: | c_2 = c_7 I: | c_3 = 2 c_6 N: | c_3 = 2 c_8 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 8 c_2 = 2 c_3 = 10 c_4 = 8 c_5 = 1 c_6 = 5 c_7 = 2 c_8 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2SO_4 + 2 KMnO_4 + 10 NH_4I ⟶ 8 H_2O + K_2SO_4 + 5 I_2 + 2 MnSO_4 + 5 (NH_4)_2SO_4

sulfuric acid + potassium permanganate + ammonium iodide ⟶ water + potassium sulfate + iodine + manganese(II) sulfate + ammonium sulfate

Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + NH_4I ⟶ H_2O + K_2SO_4 + I_2 + MnSO_4 + (NH_4)_2SO_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: 8 H_2SO_4 + 2 KMnO_4 + 10 NH_4I ⟶ 8 H_2O + K_2SO_4 + 5 I_2 + 2 MnSO_4 + 5 (NH_4)_2SO_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 | 8 | -8 KMnO_4 | 2 | -2 NH_4I | 10 | -10 H_2O | 8 | 8 K_2SO_4 | 1 | 1 I_2 | 5 | 5 MnSO_4 | 2 | 2 (NH_4)_2SO_4 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 8 | -8 | ([H2SO4])^(-8) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) NH_4I | 10 | -10 | ([NH4I])^(-10) H_2O | 8 | 8 | ([H2O])^8 K_2SO_4 | 1 | 1 | [K2SO4] I_2 | 5 | 5 | ([I2])^5 MnSO_4 | 2 | 2 | ([MnSO4])^2 (NH_4)_2SO_4 | 5 | 5 | ([(NH4)2SO4])^5 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])^(-8) ([KMnO4])^(-2) ([NH4I])^(-10) ([H2O])^8 [K2SO4] ([I2])^5 ([MnSO4])^2 ([(NH4)2SO4])^5 = (([H2O])^8 [K2SO4] ([I2])^5 ([MnSO4])^2 ([(NH4)2SO4])^5)/(([H2SO4])^8 ([KMnO4])^2 ([NH4I])^10)

Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + NH_4I ⟶ H_2O + K_2SO_4 + I_2 + MnSO_4 + (NH_4)_2SO_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: 8 H_2SO_4 + 2 KMnO_4 + 10 NH_4I ⟶ 8 H_2O + K_2SO_4 + 5 I_2 + 2 MnSO_4 + 5 (NH_4)_2SO_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 | 8 | -8 KMnO_4 | 2 | -2 NH_4I | 10 | -10 H_2O | 8 | 8 K_2SO_4 | 1 | 1 I_2 | 5 | 5 MnSO_4 | 2 | 2 (NH_4)_2SO_4 | 5 | 5 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 | 8 | -8 | -1/8 (Δ[H2SO4])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) NH_4I | 10 | -10 | -1/10 (Δ[NH4I])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) I_2 | 5 | 5 | 1/5 (Δ[I2])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(Δt) (NH_4)_2SO_4 | 5 | 5 | 1/5 (Δ[(NH4)2SO4])/(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 = -1/8 (Δ[H2SO4])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/10 (Δ[NH4I])/(Δt) = 1/8 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/5 (Δ[I2])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) = 1/5 (Δ[(NH4)2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | potassium permanganate | ammonium iodide | water | potassium sulfate | iodine | manganese(II) sulfate | ammonium sulfate formula | H_2SO_4 | KMnO_4 | NH_4I | H_2O | K_2SO_4 | I_2 | MnSO_4 | (NH_4)_2SO_4 Hill formula | H_2O_4S | KMnO_4 | H_4IN | H_2O | K_2O_4S | I_2 | MnSO_4 | H_8N_2O_4S name | sulfuric acid | potassium permanganate | ammonium iodide | water | potassium sulfate | iodine | manganese(II) sulfate | ammonium sulfate IUPAC name | sulfuric acid | potassium permanganate | | water | dipotassium sulfate | molecular iodine | manganese(+2) cation sulfate |