H2SO4 + KMnO4 + C8H10 = H2O + K2SO4 + MnSO4 + C8H6O4

H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + C_6H_5C_2H_5 ethylbenzene ⟶ H_2O water + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + C_6H_4(COOH)_2 phthalic acid

Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + C_6H_5C_2H_5 ⟶ H_2O + K_2SO_4 + MnSO_4 + C_6H_4(COOH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 C_6H_5C_2H_5 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 MnSO_4 + c_7 C_6H_4(COOH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn and C: H: | 2 c_1 + 10 c_3 = 2 c_4 + 6 c_7 O: | 4 c_1 + 4 c_2 = c_4 + 4 c_5 + 4 c_6 + 4 c_7 S: | c_1 = c_5 + c_6 K: | c_2 = 2 c_5 Mn: | c_2 = c_6 C: | 8 c_3 = 8 c_7 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 18/5 c_2 = 12/5 c_3 = 1 c_4 = 28/5 c_5 = 6/5 c_6 = 12/5 c_7 = 1 Multiply by the least common denominator, 5, to eliminate fractional coefficients: c_1 = 18 c_2 = 12 c_3 = 5 c_4 = 28 c_5 = 6 c_6 = 12 c_7 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 18 H_2SO_4 + 12 KMnO_4 + 5 C_6H_5C_2H_5 ⟶ 28 H_2O + 6 K_2SO_4 + 12 MnSO_4 + 5 C_6H_4(COOH)_2

+ + ⟶ + + +

sulfuric acid + potassium permanganate + ethylbenzene ⟶ water + potassium sulfate + manganese(II) sulfate + phthalic acid

Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + C_6H_5C_2H_5 ⟶ H_2O + K_2SO_4 + MnSO_4 + C_6H_4(COOH)_2 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: 18 H_2SO_4 + 12 KMnO_4 + 5 C_6H_5C_2H_5 ⟶ 28 H_2O + 6 K_2SO_4 + 12 MnSO_4 + 5 C_6H_4(COOH)_2 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 | 18 | -18 KMnO_4 | 12 | -12 C_6H_5C_2H_5 | 5 | -5 H_2O | 28 | 28 K_2SO_4 | 6 | 6 MnSO_4 | 12 | 12 C_6H_4(COOH)_2 | 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 | 18 | -18 | ([H2SO4])^(-18) KMnO_4 | 12 | -12 | ([KMnO4])^(-12) C_6H_5C_2H_5 | 5 | -5 | ([C6H5C2H5])^(-5) H_2O | 28 | 28 | ([H2O])^28 K_2SO_4 | 6 | 6 | ([K2SO4])^6 MnSO_4 | 12 | 12 | ([MnSO4])^12 C_6H_4(COOH)_2 | 5 | 5 | ([C6H4(COOH)2])^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])^(-18) ([KMnO4])^(-12) ([C6H5C2H5])^(-5) ([H2O])^28 ([K2SO4])^6 ([MnSO4])^12 ([C6H4(COOH)2])^5 = (([H2O])^28 ([K2SO4])^6 ([MnSO4])^12 ([C6H4(COOH)2])^5)/(([H2SO4])^18 ([KMnO4])^12 ([C6H5C2H5])^5)

Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + C_6H_5C_2H_5 ⟶ H_2O + K_2SO_4 + MnSO_4 + C_6H_4(COOH)_2 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: 18 H_2SO_4 + 12 KMnO_4 + 5 C_6H_5C_2H_5 ⟶ 28 H_2O + 6 K_2SO_4 + 12 MnSO_4 + 5 C_6H_4(COOH)_2 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 | 18 | -18 KMnO_4 | 12 | -12 C_6H_5C_2H_5 | 5 | -5 H_2O | 28 | 28 K_2SO_4 | 6 | 6 MnSO_4 | 12 | 12 C_6H_4(COOH)_2 | 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 | 18 | -18 | -1/18 (Δ[H2SO4])/(Δt) KMnO_4 | 12 | -12 | -1/12 (Δ[KMnO4])/(Δt) C_6H_5C_2H_5 | 5 | -5 | -1/5 (Δ[C6H5C2H5])/(Δt) H_2O | 28 | 28 | 1/28 (Δ[H2O])/(Δt) K_2SO_4 | 6 | 6 | 1/6 (Δ[K2SO4])/(Δt) MnSO_4 | 12 | 12 | 1/12 (Δ[MnSO4])/(Δt) C_6H_4(COOH)_2 | 5 | 5 | 1/5 (Δ[C6H4(COOH)2])/(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 = -1/18 (Δ[H2SO4])/(Δt) = -1/12 (Δ[KMnO4])/(Δt) = -1/5 (Δ[C6H5C2H5])/(Δt) = 1/28 (Δ[H2O])/(Δt) = 1/6 (Δ[K2SO4])/(Δt) = 1/12 (Δ[MnSO4])/(Δt) = 1/5 (Δ[C6H4(COOH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | potassium permanganate | ethylbenzene | water | potassium sulfate | manganese(II) sulfate | phthalic acid formula | H_2SO_4 | KMnO_4 | C_6H_5C_2H_5 | H_2O | K_2SO_4 | MnSO_4 | C_6H_4(COOH)_2 Hill formula | H_2O_4S | KMnO_4 | C_8H_10 | H_2O | K_2O_4S | MnSO_4 | C_8H_6O_4 name | sulfuric acid | potassium permanganate | ethylbenzene | water | potassium sulfate | manganese(II) sulfate | phthalic acid IUPAC name | sulfuric acid | potassium permanganate | ethylbenzene | water | dipotassium sulfate | manganese(+2) cation sulfate | phthalic acid