Search

H2SO4 + H2S + K2MnO4 = H2O + K2SO4 + S + MnSO4

Input interpretation

H_2SO_4 sulfuric acid + H_2S hydrogen sulfide + K_2MnO_4 potassium manganate ⟶ H_2O water + K_2SO_4 potassium sulfate + S mixed sulfur + MnSO_4 manganese(II) sulfate
H_2SO_4 sulfuric acid + H_2S hydrogen sulfide + K_2MnO_4 potassium manganate ⟶ H_2O water + K_2SO_4 potassium sulfate + S mixed sulfur + MnSO_4 manganese(II) sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + H_2S + K_2MnO_4 ⟶ H_2O + K_2SO_4 + S + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2S + c_3 K_2MnO_4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 S + 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 and Mn: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 4 c_3 = c_4 + 4 c_5 + 4 c_7 S: | c_1 + c_2 = c_5 + c_6 + c_7 K: | 2 c_3 = 2 c_5 Mn: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = 3 c_1 - 4 c_3 = 1 c_4 = 4 c_1 - 4 c_5 = 1 c_6 = 4 c_1 - 6 c_7 = 1 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 = 2 c_3 = 1 c_4 = 4 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 H_2S + K_2MnO_4 ⟶ 4 H_2O + K_2SO_4 + 2 S + MnSO_4
Balance the chemical equation algebraically: H_2SO_4 + H_2S + K_2MnO_4 ⟶ H_2O + K_2SO_4 + S + MnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 H_2S + c_3 K_2MnO_4 ⟶ c_4 H_2O + c_5 K_2SO_4 + c_6 S + 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 and Mn: H: | 2 c_1 + 2 c_2 = 2 c_4 O: | 4 c_1 + 4 c_3 = c_4 + 4 c_5 + 4 c_7 S: | c_1 + c_2 = c_5 + c_6 + c_7 K: | 2 c_3 = 2 c_5 Mn: | 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_3 = 1 and solve the system of equations for the remaining coefficients: c_2 = 3 c_1 - 4 c_3 = 1 c_4 = 4 c_1 - 4 c_5 = 1 c_6 = 4 c_1 - 6 c_7 = 1 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 = 2 c_3 = 1 c_4 = 4 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + 2 H_2S + K_2MnO_4 ⟶ 4 H_2O + K_2SO_4 + 2 S + MnSO_4

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + hydrogen sulfide + potassium manganate ⟶ water + potassium sulfate + mixed sulfur + manganese(II) sulfate
sulfuric acid + hydrogen sulfide + potassium manganate ⟶ water + potassium sulfate + mixed sulfur + manganese(II) sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2S + K_2MnO_4 ⟶ H_2O + K_2SO_4 + S + 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: 2 H_2SO_4 + 2 H_2S + K_2MnO_4 ⟶ 4 H_2O + K_2SO_4 + 2 S + 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 | 2 | -2 H_2S | 2 | -2 K_2MnO_4 | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 S | 2 | 2 MnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) H_2S | 2 | -2 | ([H2S])^(-2) K_2MnO_4 | 1 | -1 | ([K2MnO4])^(-1) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 1 | 1 | [K2SO4] S | 2 | 2 | ([S])^2 MnSO_4 | 1 | 1 | [MnSO4] 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])^(-2) ([H2S])^(-2) ([K2MnO4])^(-1) ([H2O])^4 [K2SO4] ([S])^2 [MnSO4] = (([H2O])^4 [K2SO4] ([S])^2 [MnSO4])/(([H2SO4])^2 ([H2S])^2 [K2MnO4])
Construct the equilibrium constant, K, expression for: H_2SO_4 + H_2S + K_2MnO_4 ⟶ H_2O + K_2SO_4 + S + 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: 2 H_2SO_4 + 2 H_2S + K_2MnO_4 ⟶ 4 H_2O + K_2SO_4 + 2 S + 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 | 2 | -2 H_2S | 2 | -2 K_2MnO_4 | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 S | 2 | 2 MnSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) H_2S | 2 | -2 | ([H2S])^(-2) K_2MnO_4 | 1 | -1 | ([K2MnO4])^(-1) H_2O | 4 | 4 | ([H2O])^4 K_2SO_4 | 1 | 1 | [K2SO4] S | 2 | 2 | ([S])^2 MnSO_4 | 1 | 1 | [MnSO4] 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])^(-2) ([H2S])^(-2) ([K2MnO4])^(-1) ([H2O])^4 [K2SO4] ([S])^2 [MnSO4] = (([H2O])^4 [K2SO4] ([S])^2 [MnSO4])/(([H2SO4])^2 ([H2S])^2 [K2MnO4])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + H_2S + K_2MnO_4 ⟶ H_2O + K_2SO_4 + S + 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: 2 H_2SO_4 + 2 H_2S + K_2MnO_4 ⟶ 4 H_2O + K_2SO_4 + 2 S + 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 | 2 | -2 H_2S | 2 | -2 K_2MnO_4 | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 S | 2 | 2 MnSO_4 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) H_2S | 2 | -2 | -1/2 (Δ[H2S])/(Δt) K_2MnO_4 | 1 | -1 | -(Δ[K2MnO4])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) S | 2 | 2 | 1/2 (Δ[S])/(Δt) MnSO_4 | 1 | 1 | (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 = -1/2 (Δ[H2SO4])/(Δt) = -1/2 (Δ[H2S])/(Δt) = -(Δ[K2MnO4])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[S])/(Δt) = (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + H_2S + K_2MnO_4 ⟶ H_2O + K_2SO_4 + S + 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: 2 H_2SO_4 + 2 H_2S + K_2MnO_4 ⟶ 4 H_2O + K_2SO_4 + 2 S + 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 | 2 | -2 H_2S | 2 | -2 K_2MnO_4 | 1 | -1 H_2O | 4 | 4 K_2SO_4 | 1 | 1 S | 2 | 2 MnSO_4 | 1 | 1 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 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) H_2S | 2 | -2 | -1/2 (Δ[H2S])/(Δt) K_2MnO_4 | 1 | -1 | -(Δ[K2MnO4])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) S | 2 | 2 | 1/2 (Δ[S])/(Δt) MnSO_4 | 1 | 1 | (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 = -1/2 (Δ[H2SO4])/(Δt) = -1/2 (Δ[H2S])/(Δt) = -(Δ[K2MnO4])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[S])/(Δt) = (Δ[MnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen sulfide | potassium manganate | water | potassium sulfate | mixed sulfur | manganese(II) sulfate formula | H_2SO_4 | H_2S | K_2MnO_4 | H_2O | K_2SO_4 | S | MnSO_4 Hill formula | H_2O_4S | H_2S | K_2MnO_4 | H_2O | K_2O_4S | S | MnSO_4 name | sulfuric acid | hydrogen sulfide | potassium manganate | water | potassium sulfate | mixed sulfur | manganese(II) sulfate IUPAC name | sulfuric acid | hydrogen sulfide | dipotassium dioxido-dioxomanganese | water | dipotassium sulfate | sulfur | manganese(+2) cation sulfate
| sulfuric acid | hydrogen sulfide | potassium manganate | water | potassium sulfate | mixed sulfur | manganese(II) sulfate formula | H_2SO_4 | H_2S | K_2MnO_4 | H_2O | K_2SO_4 | S | MnSO_4 Hill formula | H_2O_4S | H_2S | K_2MnO_4 | H_2O | K_2O_4S | S | MnSO_4 name | sulfuric acid | hydrogen sulfide | potassium manganate | water | potassium sulfate | mixed sulfur | manganese(II) sulfate IUPAC name | sulfuric acid | hydrogen sulfide | dipotassium dioxido-dioxomanganese | water | dipotassium sulfate | sulfur | manganese(+2) cation sulfate

Random Queries

density of hydrogen sulfide vs trimethylamine
discovery year of sodium vs potassium
boiling point of oxygen vs nitrogen
formula string of selenium ions
molar mass of metatellurate anion vs hypobromite anion
ion class of rhodium(III) cation
IUPAC name of 2,2,2-trifluoroethanol vs 1,1,1,4,4,4-hexafluoro-2-butyne
formula string of monatomic anions
(melting point of cobalt trifluoride)/(freezing point of cobalt trifluoride)
unit cell volume of abelsonite vs dinite