Input interpretation
H_2SO_4 (sulfuric acid) + KMnO_4 (potassium permanganate) + KNO_2 (potassium nitrite) ⟶ H_2O (water) + K_2SO_4 (potassium sulfate) + MnSO_4 (manganese(II) sulfate) + KNO_3 (potassium nitrate)
Balanced equation
Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 KNO_2 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 MnSO_4 + c_7 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K, Mn and N: H: | 2 c_1 = 2 c_4 O: | 4 c_1 + 4 c_2 + 2 c_3 = c_4 + 4 c_5 + 4 c_6 + 3 c_7 S: | c_1 = c_5 + c_6 K: | c_2 + c_3 = 2 c_5 + c_7 Mn: | c_2 = c_6 N: | c_3 = 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 5 c_4 = 3 c_5 = 1 c_6 = 2 c_7 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 2 KMnO_4 + 5 KNO_2 ⟶ 3 H_2O + K_2SO_4 + 2 MnSO_4 + 5 KNO_3
Structures
+ + ⟶ + + +
Names
sulfuric acid + potassium permanganate + potassium nitrite ⟶ water + potassium sulfate + manganese(II) sulfate + potassium nitrate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + KNO_3 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: 3 H_2SO_4 + 2 KMnO_4 + 5 KNO_2 ⟶ 3 H_2O + K_2SO_4 + 2 MnSO_4 + 5 KNO_3 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 | 3 | -3 KMnO_4 | 2 | -2 KNO_2 | 5 | -5 H_2O | 3 | 3 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 KNO_3 | 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 | 3 | -3 | ([H2SO4])^(-3) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) KNO_2 | 5 | -5 | ([KNO2])^(-5) H_2O | 3 | 3 | ([H2O])^3 K_2SO_4 | 1 | 1 | [K2SO4] MnSO_4 | 2 | 2 | ([MnSO4])^2 KNO_3 | 5 | 5 | ([KNO3])^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])^(-3) ([KMnO4])^(-2) ([KNO2])^(-5) ([H2O])^3 [K2SO4] ([MnSO4])^2 ([KNO3])^5 = (([H2O])^3 [K2SO4] ([MnSO4])^2 ([KNO3])^5)/(([H2SO4])^3 ([KMnO4])^2 ([KNO2])^5)](../image_source/84f8fcb68cc1a8140294b18b27cb4f50.png)
Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + KNO_3 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: 3 H_2SO_4 + 2 KMnO_4 + 5 KNO_2 ⟶ 3 H_2O + K_2SO_4 + 2 MnSO_4 + 5 KNO_3 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 | 3 | -3 KMnO_4 | 2 | -2 KNO_2 | 5 | -5 H_2O | 3 | 3 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 KNO_3 | 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 | 3 | -3 | ([H2SO4])^(-3) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) KNO_2 | 5 | -5 | ([KNO2])^(-5) H_2O | 3 | 3 | ([H2O])^3 K_2SO_4 | 1 | 1 | [K2SO4] MnSO_4 | 2 | 2 | ([MnSO4])^2 KNO_3 | 5 | 5 | ([KNO3])^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])^(-3) ([KMnO4])^(-2) ([KNO2])^(-5) ([H2O])^3 [K2SO4] ([MnSO4])^2 ([KNO3])^5 = (([H2O])^3 [K2SO4] ([MnSO4])^2 ([KNO3])^5)/(([H2SO4])^3 ([KMnO4])^2 ([KNO2])^5)
Rate of reaction
![Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + KNO_3 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: 3 H_2SO_4 + 2 KMnO_4 + 5 KNO_2 ⟶ 3 H_2O + K_2SO_4 + 2 MnSO_4 + 5 KNO_3 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 | 3 | -3 KMnO_4 | 2 | -2 KNO_2 | 5 | -5 H_2O | 3 | 3 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 KNO_3 | 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 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) KNO_2 | 5 | -5 | -1/5 (Δ[KNO2])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(Δt) KNO_3 | 5 | 5 | 1/5 (Δ[KNO3])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/5 (Δ[KNO2])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) = 1/5 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/73517508ebf0a7cf9b319d2b5d9f3c38.png)
Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + MnSO_4 + KNO_3 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: 3 H_2SO_4 + 2 KMnO_4 + 5 KNO_2 ⟶ 3 H_2O + K_2SO_4 + 2 MnSO_4 + 5 KNO_3 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 | 3 | -3 KMnO_4 | 2 | -2 KNO_2 | 5 | -5 H_2O | 3 | 3 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 KNO_3 | 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 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) KNO_2 | 5 | -5 | -1/5 (Δ[KNO2])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(Δt) KNO_3 | 5 | 5 | 1/5 (Δ[KNO3])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/5 (Δ[KNO2])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) = 1/5 (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| sulfuric acid | potassium permanganate | potassium nitrite | water | potassium sulfate | manganese(II) sulfate | potassium nitrate formula | H_2SO_4 | KMnO_4 | KNO_2 | H_2O | K_2SO_4 | MnSO_4 | KNO_3 Hill formula | H_2O_4S | KMnO_4 | KNO_2 | H_2O | K_2O_4S | MnSO_4 | KNO_3 name | sulfuric acid | potassium permanganate | potassium nitrite | water | potassium sulfate | manganese(II) sulfate | potassium nitrate IUPAC name | sulfuric acid | potassium permanganate | potassium nitrite | water | dipotassium sulfate | manganese(+2) cation sulfate | potassium nitrate