Input interpretation
H_2SO_4 sulfuric acid + KMnO_4 potassium permanganate + HCOOH formic acid ⟶ H_2O water + CO_2 carbon dioxide + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate
Balanced equation
Balance the chemical equation algebraically: H_2SO_4 + KMnO_4 + HCOOH ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KMnO_4 + c_3 HCOOH ⟶ c_4 H_2O + c_5 CO_2 + c_6 K_2SO_4 + c_7 MnSO_4 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 + 2 c_3 = 2 c_4 O: | 4 c_1 + 4 c_2 + 2 c_3 = c_4 + 2 c_5 + 4 c_6 + 4 c_7 S: | c_1 = c_6 + c_7 K: | c_2 = 2 c_6 Mn: | c_2 = c_7 C: | c_3 = c_5 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_6 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 2 c_3 = 5 c_4 = 8 c_5 = 5 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + 2 KMnO_4 + 5 HCOOH ⟶ 8 H_2O + 5 CO_2 + K_2SO_4 + 2 MnSO_4
Structures
+ + ⟶ + + +
Names
sulfuric acid + potassium permanganate + formic acid ⟶ water + carbon dioxide + potassium sulfate + manganese(II) sulfate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + HCOOH ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_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: 3 H_2SO_4 + 2 KMnO_4 + 5 HCOOH ⟶ 8 H_2O + 5 CO_2 + K_2SO_4 + 2 MnSO_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 | 3 | -3 KMnO_4 | 2 | -2 HCOOH | 5 | -5 H_2O | 8 | 8 CO_2 | 5 | 5 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 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) HCOOH | 5 | -5 | ([HCOOH])^(-5) H_2O | 8 | 8 | ([H2O])^8 CO_2 | 5 | 5 | ([CO2])^5 K_2SO_4 | 1 | 1 | [K2SO4] MnSO_4 | 2 | 2 | ([MnSO4])^2 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) ([HCOOH])^(-5) ([H2O])^8 ([CO2])^5 [K2SO4] ([MnSO4])^2 = (([H2O])^8 ([CO2])^5 [K2SO4] ([MnSO4])^2)/(([H2SO4])^3 ([KMnO4])^2 ([HCOOH])^5)](../image_source/522bc51c9798c40520904a5ed293cca1.png)
Construct the equilibrium constant, K, expression for: H_2SO_4 + KMnO_4 + HCOOH ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_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: 3 H_2SO_4 + 2 KMnO_4 + 5 HCOOH ⟶ 8 H_2O + 5 CO_2 + K_2SO_4 + 2 MnSO_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 | 3 | -3 KMnO_4 | 2 | -2 HCOOH | 5 | -5 H_2O | 8 | 8 CO_2 | 5 | 5 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 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) HCOOH | 5 | -5 | ([HCOOH])^(-5) H_2O | 8 | 8 | ([H2O])^8 CO_2 | 5 | 5 | ([CO2])^5 K_2SO_4 | 1 | 1 | [K2SO4] MnSO_4 | 2 | 2 | ([MnSO4])^2 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) ([HCOOH])^(-5) ([H2O])^8 ([CO2])^5 [K2SO4] ([MnSO4])^2 = (([H2O])^8 ([CO2])^5 [K2SO4] ([MnSO4])^2)/(([H2SO4])^3 ([KMnO4])^2 ([HCOOH])^5)
Rate of reaction
![Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + HCOOH ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_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: 3 H_2SO_4 + 2 KMnO_4 + 5 HCOOH ⟶ 8 H_2O + 5 CO_2 + K_2SO_4 + 2 MnSO_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 | 3 | -3 KMnO_4 | 2 | -2 HCOOH | 5 | -5 H_2O | 8 | 8 CO_2 | 5 | 5 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 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) HCOOH | 5 | -5 | -1/5 (Δ[HCOOH])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) CO_2 | 5 | 5 | 1/5 (Δ[CO2])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(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[HCOOH])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/5 (Δ[CO2])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/fd2f858a5cfb2a3567fda8793ebdd7b3.png)
Construct the rate of reaction expression for: H_2SO_4 + KMnO_4 + HCOOH ⟶ H_2O + CO_2 + K_2SO_4 + MnSO_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: 3 H_2SO_4 + 2 KMnO_4 + 5 HCOOH ⟶ 8 H_2O + 5 CO_2 + K_2SO_4 + 2 MnSO_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 | 3 | -3 KMnO_4 | 2 | -2 HCOOH | 5 | -5 H_2O | 8 | 8 CO_2 | 5 | 5 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 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) HCOOH | 5 | -5 | -1/5 (Δ[HCOOH])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) CO_2 | 5 | 5 | 1/5 (Δ[CO2])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(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[HCOOH])/(Δt) = 1/8 (Δ[H2O])/(Δt) = 1/5 (Δ[CO2])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| sulfuric acid | potassium permanganate | formic acid | water | carbon dioxide | potassium sulfate | manganese(II) sulfate formula | H_2SO_4 | KMnO_4 | HCOOH | H_2O | CO_2 | K_2SO_4 | MnSO_4 Hill formula | H_2O_4S | KMnO_4 | CH_2O_2 | H_2O | CO_2 | K_2O_4S | MnSO_4 name | sulfuric acid | potassium permanganate | formic acid | water | carbon dioxide | potassium sulfate | manganese(II) sulfate IUPAC name | sulfuric acid | potassium permanganate | formic acid | water | carbon dioxide | dipotassium sulfate | manganese(+2) cation sulfate