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H2O + KMnO4 + MnSO4 = H2SO4 + O2 + K2SO4 + MnO2

Input interpretation

H_2O water + KMnO_4 potassium permanganate + MnSO_4 manganese(II) sulfate ⟶ H_2SO_4 sulfuric acid + O_2 oxygen + K_2SO_4 potassium sulfate + MnO_2 manganese dioxide
H_2O water + KMnO_4 potassium permanganate + MnSO_4 manganese(II) sulfate ⟶ H_2SO_4 sulfuric acid + O_2 oxygen + K_2SO_4 potassium sulfate + MnO_2 manganese dioxide

Balanced equation

Balance the chemical equation algebraically: H_2O + KMnO_4 + MnSO_4 ⟶ H_2SO_4 + O_2 + K_2SO_4 + MnO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 MnSO_4 ⟶ c_4 H_2SO_4 + c_5 O_2 + c_6 K_2SO_4 + c_7 MnO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn and S: H: | 2 c_1 = 2 c_4 O: | c_1 + 4 c_2 + 4 c_3 = 4 c_4 + 2 c_5 + 4 c_6 + 2 c_7 K: | c_2 = 2 c_6 Mn: | c_2 + c_3 = c_7 S: | c_3 = c_4 + 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_5 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1 + 2 c_3 = (3 c_1)/2 + 1 c_4 = c_1 c_5 = 1 c_6 = c_1/2 + 1 c_7 = (5 c_1)/2 + 3 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 4 c_3 = 4 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 4 KMnO_4 + 4 MnSO_4 ⟶ 2 H_2SO_4 + O_2 + 2 K_2SO_4 + 8 MnO_2
Balance the chemical equation algebraically: H_2O + KMnO_4 + MnSO_4 ⟶ H_2SO_4 + O_2 + K_2SO_4 + MnO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 MnSO_4 ⟶ c_4 H_2SO_4 + c_5 O_2 + c_6 K_2SO_4 + c_7 MnO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn and S: H: | 2 c_1 = 2 c_4 O: | c_1 + 4 c_2 + 4 c_3 = 4 c_4 + 2 c_5 + 4 c_6 + 2 c_7 K: | c_2 = 2 c_6 Mn: | c_2 + c_3 = c_7 S: | c_3 = c_4 + 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_5 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1 + 2 c_3 = (3 c_1)/2 + 1 c_4 = c_1 c_5 = 1 c_6 = c_1/2 + 1 c_7 = (5 c_1)/2 + 3 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 4 c_3 = 4 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 8 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 4 KMnO_4 + 4 MnSO_4 ⟶ 2 H_2SO_4 + O_2 + 2 K_2SO_4 + 8 MnO_2

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

water + potassium permanganate + manganese(II) sulfate ⟶ sulfuric acid + oxygen + potassium sulfate + manganese dioxide
water + potassium permanganate + manganese(II) sulfate ⟶ sulfuric acid + oxygen + potassium sulfate + manganese dioxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + MnSO_4 ⟶ H_2SO_4 + O_2 + K_2SO_4 + MnO_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: 2 H_2O + 4 KMnO_4 + 4 MnSO_4 ⟶ 2 H_2SO_4 + O_2 + 2 K_2SO_4 + 8 MnO_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_2O | 2 | -2 KMnO_4 | 4 | -4 MnSO_4 | 4 | -4 H_2SO_4 | 2 | 2 O_2 | 1 | 1 K_2SO_4 | 2 | 2 MnO_2 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) KMnO_4 | 4 | -4 | ([KMnO4])^(-4) MnSO_4 | 4 | -4 | ([MnSO4])^(-4) H_2SO_4 | 2 | 2 | ([H2SO4])^2 O_2 | 1 | 1 | [O2] K_2SO_4 | 2 | 2 | ([K2SO4])^2 MnO_2 | 8 | 8 | ([MnO2])^8 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 = ([H2O])^(-2) ([KMnO4])^(-4) ([MnSO4])^(-4) ([H2SO4])^2 [O2] ([K2SO4])^2 ([MnO2])^8 = (([H2SO4])^2 [O2] ([K2SO4])^2 ([MnO2])^8)/(([H2O])^2 ([KMnO4])^4 ([MnSO4])^4)
Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + MnSO_4 ⟶ H_2SO_4 + O_2 + K_2SO_4 + MnO_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: 2 H_2O + 4 KMnO_4 + 4 MnSO_4 ⟶ 2 H_2SO_4 + O_2 + 2 K_2SO_4 + 8 MnO_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_2O | 2 | -2 KMnO_4 | 4 | -4 MnSO_4 | 4 | -4 H_2SO_4 | 2 | 2 O_2 | 1 | 1 K_2SO_4 | 2 | 2 MnO_2 | 8 | 8 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) KMnO_4 | 4 | -4 | ([KMnO4])^(-4) MnSO_4 | 4 | -4 | ([MnSO4])^(-4) H_2SO_4 | 2 | 2 | ([H2SO4])^2 O_2 | 1 | 1 | [O2] K_2SO_4 | 2 | 2 | ([K2SO4])^2 MnO_2 | 8 | 8 | ([MnO2])^8 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 = ([H2O])^(-2) ([KMnO4])^(-4) ([MnSO4])^(-4) ([H2SO4])^2 [O2] ([K2SO4])^2 ([MnO2])^8 = (([H2SO4])^2 [O2] ([K2SO4])^2 ([MnO2])^8)/(([H2O])^2 ([KMnO4])^4 ([MnSO4])^4)

Rate of reaction

Construct the rate of reaction expression for: H_2O + KMnO_4 + MnSO_4 ⟶ H_2SO_4 + O_2 + K_2SO_4 + MnO_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: 2 H_2O + 4 KMnO_4 + 4 MnSO_4 ⟶ 2 H_2SO_4 + O_2 + 2 K_2SO_4 + 8 MnO_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_2O | 2 | -2 KMnO_4 | 4 | -4 MnSO_4 | 4 | -4 H_2SO_4 | 2 | 2 O_2 | 1 | 1 K_2SO_4 | 2 | 2 MnO_2 | 8 | 8 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) KMnO_4 | 4 | -4 | -1/4 (Δ[KMnO4])/(Δt) MnSO_4 | 4 | -4 | -1/4 (Δ[MnSO4])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) K_2SO_4 | 2 | 2 | 1/2 (Δ[K2SO4])/(Δt) MnO_2 | 8 | 8 | 1/8 (Δ[MnO2])/(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 = -1/2 (Δ[H2O])/(Δt) = -1/4 (Δ[KMnO4])/(Δt) = -1/4 (Δ[MnSO4])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[K2SO4])/(Δt) = 1/8 (Δ[MnO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + KMnO_4 + MnSO_4 ⟶ H_2SO_4 + O_2 + K_2SO_4 + MnO_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: 2 H_2O + 4 KMnO_4 + 4 MnSO_4 ⟶ 2 H_2SO_4 + O_2 + 2 K_2SO_4 + 8 MnO_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_2O | 2 | -2 KMnO_4 | 4 | -4 MnSO_4 | 4 | -4 H_2SO_4 | 2 | 2 O_2 | 1 | 1 K_2SO_4 | 2 | 2 MnO_2 | 8 | 8 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) KMnO_4 | 4 | -4 | -1/4 (Δ[KMnO4])/(Δt) MnSO_4 | 4 | -4 | -1/4 (Δ[MnSO4])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) K_2SO_4 | 2 | 2 | 1/2 (Δ[K2SO4])/(Δt) MnO_2 | 8 | 8 | 1/8 (Δ[MnO2])/(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 = -1/2 (Δ[H2O])/(Δt) = -1/4 (Δ[KMnO4])/(Δt) = -1/4 (Δ[MnSO4])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[K2SO4])/(Δt) = 1/8 (Δ[MnO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | potassium permanganate | manganese(II) sulfate | sulfuric acid | oxygen | potassium sulfate | manganese dioxide formula | H_2O | KMnO_4 | MnSO_4 | H_2SO_4 | O_2 | K_2SO_4 | MnO_2 Hill formula | H_2O | KMnO_4 | MnSO_4 | H_2O_4S | O_2 | K_2O_4S | MnO_2 name | water | potassium permanganate | manganese(II) sulfate | sulfuric acid | oxygen | potassium sulfate | manganese dioxide IUPAC name | water | potassium permanganate | manganese(+2) cation sulfate | sulfuric acid | molecular oxygen | dipotassium sulfate | dioxomanganese
| water | potassium permanganate | manganese(II) sulfate | sulfuric acid | oxygen | potassium sulfate | manganese dioxide formula | H_2O | KMnO_4 | MnSO_4 | H_2SO_4 | O_2 | K_2SO_4 | MnO_2 Hill formula | H_2O | KMnO_4 | MnSO_4 | H_2O_4S | O_2 | K_2O_4S | MnO_2 name | water | potassium permanganate | manganese(II) sulfate | sulfuric acid | oxygen | potassium sulfate | manganese dioxide IUPAC name | water | potassium permanganate | manganese(+2) cation sulfate | sulfuric acid | molecular oxygen | dipotassium sulfate | dioxomanganese

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