Search

H2O + KMnO4 + VOSO4 = H2SO4 + K2SO4 + MnSO4 + V2O5

Input interpretation

H_2O water + KMnO_4 potassium permanganate + VOSO_4·2H_2O vanadyl sulfate ⟶ H_2SO_4 sulfuric acid + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + V_2O_5 vanadium pentoxide
H_2O water + KMnO_4 potassium permanganate + VOSO_4·2H_2O vanadyl sulfate ⟶ H_2SO_4 sulfuric acid + K_2SO_4 potassium sulfate + MnSO_4 manganese(II) sulfate + V_2O_5 vanadium pentoxide

Balanced equation

Balance the chemical equation algebraically: H_2O + KMnO_4 + VOSO_4·2H_2O ⟶ H_2SO_4 + K_2SO_4 + MnSO_4 + V_2O_5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 VOSO_4·2H_2O ⟶ c_4 H_2SO_4 + c_5 K_2SO_4 + c_6 MnSO_4 + c_7 V_2O_5 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn, S and V: H: | 2 c_1 = 2 c_4 O: | c_1 + 4 c_2 + 5 c_3 = 4 c_4 + 4 c_5 + 4 c_6 + 5 c_7 K: | c_2 = 2 c_5 Mn: | c_2 = c_6 S: | c_3 = c_4 + c_5 + c_6 V: | c_3 = 2 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 = 7 c_2 = 2 c_3 = 10 c_4 = 7 c_5 = 1 c_6 = 2 c_7 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 H_2O + 2 KMnO_4 + 10 VOSO_4·2H_2O ⟶ 7 H_2SO_4 + K_2SO_4 + 2 MnSO_4 + 5 V_2O_5
Balance the chemical equation algebraically: H_2O + KMnO_4 + VOSO_4·2H_2O ⟶ H_2SO_4 + K_2SO_4 + MnSO_4 + V_2O_5 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 VOSO_4·2H_2O ⟶ c_4 H_2SO_4 + c_5 K_2SO_4 + c_6 MnSO_4 + c_7 V_2O_5 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn, S and V: H: | 2 c_1 = 2 c_4 O: | c_1 + 4 c_2 + 5 c_3 = 4 c_4 + 4 c_5 + 4 c_6 + 5 c_7 K: | c_2 = 2 c_5 Mn: | c_2 = c_6 S: | c_3 = c_4 + c_5 + c_6 V: | c_3 = 2 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 = 7 c_2 = 2 c_3 = 10 c_4 = 7 c_5 = 1 c_6 = 2 c_7 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 7 H_2O + 2 KMnO_4 + 10 VOSO_4·2H_2O ⟶ 7 H_2SO_4 + K_2SO_4 + 2 MnSO_4 + 5 V_2O_5

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

water + potassium permanganate + vanadyl sulfate ⟶ sulfuric acid + potassium sulfate + manganese(II) sulfate + vanadium pentoxide
water + potassium permanganate + vanadyl sulfate ⟶ sulfuric acid + potassium sulfate + manganese(II) sulfate + vanadium pentoxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + VOSO_4·2H_2O ⟶ H_2SO_4 + K_2SO_4 + MnSO_4 + V_2O_5 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: 7 H_2O + 2 KMnO_4 + 10 VOSO_4·2H_2O ⟶ 7 H_2SO_4 + K_2SO_4 + 2 MnSO_4 + 5 V_2O_5 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 | 7 | -7 KMnO_4 | 2 | -2 VOSO_4·2H_2O | 10 | -10 H_2SO_4 | 7 | 7 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 V_2O_5 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 7 | -7 | ([H2O])^(-7) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) VOSO_4·2H_2O | 10 | -10 | ([VOSO4·2H2O])^(-10) H_2SO_4 | 7 | 7 | ([H2SO4])^7 K_2SO_4 | 1 | 1 | [K2SO4] MnSO_4 | 2 | 2 | ([MnSO4])^2 V_2O_5 | 5 | 5 | ([V2O5])^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 = ([H2O])^(-7) ([KMnO4])^(-2) ([VOSO4·2H2O])^(-10) ([H2SO4])^7 [K2SO4] ([MnSO4])^2 ([V2O5])^5 = (([H2SO4])^7 [K2SO4] ([MnSO4])^2 ([V2O5])^5)/(([H2O])^7 ([KMnO4])^2 ([VOSO4·2H2O])^10)
Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + VOSO_4·2H_2O ⟶ H_2SO_4 + K_2SO_4 + MnSO_4 + V_2O_5 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: 7 H_2O + 2 KMnO_4 + 10 VOSO_4·2H_2O ⟶ 7 H_2SO_4 + K_2SO_4 + 2 MnSO_4 + 5 V_2O_5 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 | 7 | -7 KMnO_4 | 2 | -2 VOSO_4·2H_2O | 10 | -10 H_2SO_4 | 7 | 7 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 V_2O_5 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 7 | -7 | ([H2O])^(-7) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) VOSO_4·2H_2O | 10 | -10 | ([VOSO4·2H2O])^(-10) H_2SO_4 | 7 | 7 | ([H2SO4])^7 K_2SO_4 | 1 | 1 | [K2SO4] MnSO_4 | 2 | 2 | ([MnSO4])^2 V_2O_5 | 5 | 5 | ([V2O5])^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 = ([H2O])^(-7) ([KMnO4])^(-2) ([VOSO4·2H2O])^(-10) ([H2SO4])^7 [K2SO4] ([MnSO4])^2 ([V2O5])^5 = (([H2SO4])^7 [K2SO4] ([MnSO4])^2 ([V2O5])^5)/(([H2O])^7 ([KMnO4])^2 ([VOSO4·2H2O])^10)

Rate of reaction

Construct the rate of reaction expression for: H_2O + KMnO_4 + VOSO_4·2H_2O ⟶ H_2SO_4 + K_2SO_4 + MnSO_4 + V_2O_5 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: 7 H_2O + 2 KMnO_4 + 10 VOSO_4·2H_2O ⟶ 7 H_2SO_4 + K_2SO_4 + 2 MnSO_4 + 5 V_2O_5 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 | 7 | -7 KMnO_4 | 2 | -2 VOSO_4·2H_2O | 10 | -10 H_2SO_4 | 7 | 7 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 V_2O_5 | 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_2O | 7 | -7 | -1/7 (Δ[H2O])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) VOSO_4·2H_2O | 10 | -10 | -1/10 (Δ[VOSO4·2H2O])/(Δt) H_2SO_4 | 7 | 7 | 1/7 (Δ[H2SO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(Δt) V_2O_5 | 5 | 5 | 1/5 (Δ[V2O5])/(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 = -1/7 (Δ[H2O])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/10 (Δ[VOSO4·2H2O])/(Δt) = 1/7 (Δ[H2SO4])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) = 1/5 (Δ[V2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + KMnO_4 + VOSO_4·2H_2O ⟶ H_2SO_4 + K_2SO_4 + MnSO_4 + V_2O_5 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: 7 H_2O + 2 KMnO_4 + 10 VOSO_4·2H_2O ⟶ 7 H_2SO_4 + K_2SO_4 + 2 MnSO_4 + 5 V_2O_5 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 | 7 | -7 KMnO_4 | 2 | -2 VOSO_4·2H_2O | 10 | -10 H_2SO_4 | 7 | 7 K_2SO_4 | 1 | 1 MnSO_4 | 2 | 2 V_2O_5 | 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_2O | 7 | -7 | -1/7 (Δ[H2O])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) VOSO_4·2H_2O | 10 | -10 | -1/10 (Δ[VOSO4·2H2O])/(Δt) H_2SO_4 | 7 | 7 | 1/7 (Δ[H2SO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) MnSO_4 | 2 | 2 | 1/2 (Δ[MnSO4])/(Δt) V_2O_5 | 5 | 5 | 1/5 (Δ[V2O5])/(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 = -1/7 (Δ[H2O])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/10 (Δ[VOSO4·2H2O])/(Δt) = 1/7 (Δ[H2SO4])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[MnSO4])/(Δt) = 1/5 (Δ[V2O5])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | potassium permanganate | vanadyl sulfate | sulfuric acid | potassium sulfate | manganese(II) sulfate | vanadium pentoxide formula | H_2O | KMnO_4 | VOSO_4·2H_2O | H_2SO_4 | K_2SO_4 | MnSO_4 | V_2O_5 Hill formula | H_2O | KMnO_4 | O_5SV | H_2O_4S | K_2O_4S | MnSO_4 | O_5V_2 name | water | potassium permanganate | vanadyl sulfate | sulfuric acid | potassium sulfate | manganese(II) sulfate | vanadium pentoxide IUPAC name | water | potassium permanganate | oxovanadium sulfate | sulfuric acid | dipotassium sulfate | manganese(+2) cation sulfate |
| water | potassium permanganate | vanadyl sulfate | sulfuric acid | potassium sulfate | manganese(II) sulfate | vanadium pentoxide formula | H_2O | KMnO_4 | VOSO_4·2H_2O | H_2SO_4 | K_2SO_4 | MnSO_4 | V_2O_5 Hill formula | H_2O | KMnO_4 | O_5SV | H_2O_4S | K_2O_4S | MnSO_4 | O_5V_2 name | water | potassium permanganate | vanadyl sulfate | sulfuric acid | potassium sulfate | manganese(II) sulfate | vanadium pentoxide IUPAC name | water | potassium permanganate | oxovanadium sulfate | sulfuric acid | dipotassium sulfate | manganese(+2) cation sulfate |

Random Queries

mass fractions of lanthanum fluoride
isomeric SMILES identifier of rubidium fluoride
CAS number of mercuric chloride vs zinc arsenite
net ionic charge of bromine V
formula tetrabutylammonium tribromide
liquid densities of platinum metals
Fe + AgNO3 = Ag + FeNO3
edge types of 2-fluoro-3-(trifluoromethyl)benzyl alcohol vs 4-bromo-2-fluoro-1-nitrobenzene
IUPAC name of zinc chlorate vs sodium perchlorate
common sources of ion of group 4 ions