Search

HNO2 + HMnO4 = H2O + HNO3 + Mn(NO3)2

Input interpretation

HNO_2 nitrous acid + HMnO4 ⟶ H_2O water + HNO_3 nitric acid + Mn(NO_3)_2 manganese(II) nitrate
HNO_2 nitrous acid + HMnO4 ⟶ H_2O water + HNO_3 nitric acid + Mn(NO_3)_2 manganese(II) nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_2 + HMnO4 ⟶ H_2O + HNO_3 + Mn(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_2 + c_2 HMnO4 ⟶ c_3 H_2O + c_4 HNO_3 + c_5 Mn(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Mn: H: | c_1 + c_2 = 2 c_3 + c_4 N: | c_1 = c_4 + 2 c_5 O: | 2 c_1 + 4 c_2 = c_3 + 3 c_4 + 6 c_5 Mn: | c_2 = 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 2 c_3 = 3 c_4 = 1 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 HNO_2 + 2 HMnO4 ⟶ 3 H_2O + HNO_3 + 2 Mn(NO_3)_2
Balance the chemical equation algebraically: HNO_2 + HMnO4 ⟶ H_2O + HNO_3 + Mn(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_2 + c_2 HMnO4 ⟶ c_3 H_2O + c_4 HNO_3 + c_5 Mn(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Mn: H: | c_1 + c_2 = 2 c_3 + c_4 N: | c_1 = c_4 + 2 c_5 O: | 2 c_1 + 4 c_2 = c_3 + 3 c_4 + 6 c_5 Mn: | c_2 = 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 2 c_3 = 3 c_4 = 1 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 HNO_2 + 2 HMnO4 ⟶ 3 H_2O + HNO_3 + 2 Mn(NO_3)_2

Structures

+ HMnO4 ⟶ + +
+ HMnO4 ⟶ + +

Names

nitrous acid + HMnO4 ⟶ water + nitric acid + manganese(II) nitrate
nitrous acid + HMnO4 ⟶ water + nitric acid + manganese(II) nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_2 + HMnO4 ⟶ H_2O + HNO_3 + Mn(NO_3)_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: 5 HNO_2 + 2 HMnO4 ⟶ 3 H_2O + HNO_3 + 2 Mn(NO_3)_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 HNO_2 | 5 | -5 HMnO4 | 2 | -2 H_2O | 3 | 3 HNO_3 | 1 | 1 Mn(NO_3)_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_2 | 5 | -5 | ([HNO2])^(-5) HMnO4 | 2 | -2 | ([HMnO4])^(-2) H_2O | 3 | 3 | ([H2O])^3 HNO_3 | 1 | 1 | [HNO3] Mn(NO_3)_2 | 2 | 2 | ([Mn(NO3)2])^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 = ([HNO2])^(-5) ([HMnO4])^(-2) ([H2O])^3 [HNO3] ([Mn(NO3)2])^2 = (([H2O])^3 [HNO3] ([Mn(NO3)2])^2)/(([HNO2])^5 ([HMnO4])^2)
Construct the equilibrium constant, K, expression for: HNO_2 + HMnO4 ⟶ H_2O + HNO_3 + Mn(NO_3)_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: 5 HNO_2 + 2 HMnO4 ⟶ 3 H_2O + HNO_3 + 2 Mn(NO_3)_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 HNO_2 | 5 | -5 HMnO4 | 2 | -2 H_2O | 3 | 3 HNO_3 | 1 | 1 Mn(NO_3)_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_2 | 5 | -5 | ([HNO2])^(-5) HMnO4 | 2 | -2 | ([HMnO4])^(-2) H_2O | 3 | 3 | ([H2O])^3 HNO_3 | 1 | 1 | [HNO3] Mn(NO_3)_2 | 2 | 2 | ([Mn(NO3)2])^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 = ([HNO2])^(-5) ([HMnO4])^(-2) ([H2O])^3 [HNO3] ([Mn(NO3)2])^2 = (([H2O])^3 [HNO3] ([Mn(NO3)2])^2)/(([HNO2])^5 ([HMnO4])^2)

Rate of reaction

Construct the rate of reaction expression for: HNO_2 + HMnO4 ⟶ H_2O + HNO_3 + Mn(NO_3)_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: 5 HNO_2 + 2 HMnO4 ⟶ 3 H_2O + HNO_3 + 2 Mn(NO_3)_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 HNO_2 | 5 | -5 HMnO4 | 2 | -2 H_2O | 3 | 3 HNO_3 | 1 | 1 Mn(NO_3)_2 | 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 HNO_2 | 5 | -5 | -1/5 (Δ[HNO2])/(Δt) HMnO4 | 2 | -2 | -1/2 (Δ[HMnO4])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) HNO_3 | 1 | 1 | (Δ[HNO3])/(Δt) Mn(NO_3)_2 | 2 | 2 | 1/2 (Δ[Mn(NO3)2])/(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 = -1/5 (Δ[HNO2])/(Δt) = -1/2 (Δ[HMnO4])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[HNO3])/(Δt) = 1/2 (Δ[Mn(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_2 + HMnO4 ⟶ H_2O + HNO_3 + Mn(NO_3)_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: 5 HNO_2 + 2 HMnO4 ⟶ 3 H_2O + HNO_3 + 2 Mn(NO_3)_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 HNO_2 | 5 | -5 HMnO4 | 2 | -2 H_2O | 3 | 3 HNO_3 | 1 | 1 Mn(NO_3)_2 | 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 HNO_2 | 5 | -5 | -1/5 (Δ[HNO2])/(Δt) HMnO4 | 2 | -2 | -1/2 (Δ[HMnO4])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) HNO_3 | 1 | 1 | (Δ[HNO3])/(Δt) Mn(NO_3)_2 | 2 | 2 | 1/2 (Δ[Mn(NO3)2])/(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 = -1/5 (Δ[HNO2])/(Δt) = -1/2 (Δ[HMnO4])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[HNO3])/(Δt) = 1/2 (Δ[Mn(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitrous acid | HMnO4 | water | nitric acid | manganese(II) nitrate formula | HNO_2 | HMnO4 | H_2O | HNO_3 | Mn(NO_3)_2 Hill formula | HNO_2 | HMnO4 | H_2O | HNO_3 | MnN_2O_6 name | nitrous acid | | water | nitric acid | manganese(II) nitrate IUPAC name | nitrous acid | | water | nitric acid | manganese(2+) dinitrate
| nitrous acid | HMnO4 | water | nitric acid | manganese(II) nitrate formula | HNO_2 | HMnO4 | H_2O | HNO_3 | Mn(NO_3)_2 Hill formula | HNO_2 | HMnO4 | H_2O | HNO_3 | MnN_2O_6 name | nitrous acid | | water | nitric acid | manganese(II) nitrate IUPAC name | nitrous acid | | water | nitric acid | manganese(2+) dinitrate

Substance properties

| nitrous acid | HMnO4 | water | nitric acid | manganese(II) nitrate molar mass | 47.013 g/mol | 119.94 g/mol | 18.015 g/mol | 63.012 g/mol | 178.95 g/mol phase | | | liquid (at STP) | liquid (at STP) | melting point | | | 0 °C | -41.6 °C | boiling point | | | 99.9839 °C | 83 °C | density | | | 1 g/cm^3 | 1.5129 g/cm^3 | 1.536 g/cm^3 solubility in water | | | | miscible | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | | | odorless | |
| nitrous acid | HMnO4 | water | nitric acid | manganese(II) nitrate molar mass | 47.013 g/mol | 119.94 g/mol | 18.015 g/mol | 63.012 g/mol | 178.95 g/mol phase | | | liquid (at STP) | liquid (at STP) | melting point | | | 0 °C | -41.6 °C | boiling point | | | 99.9839 °C | 83 °C | density | | | 1 g/cm^3 | 1.5129 g/cm^3 | 1.536 g/cm^3 solubility in water | | | | miscible | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | | | odorless | |

Units

Random Queries

H2SO4 + Al(OH)3 = H2O + Al2(SO4)3
IUPAC name of 2,4-diethylhepta-2,6-dienal
molar mass of tin(II) cation vs tin(IV) cation
HNO3 + NH4I = H2O + I2 + NO2 + NH4NO3
threshold frequency of lanthanum
SMILES identifier iron(II) selenide
molar mass of sulfide(1-) anion vs sulfur(III) cation
electron affinity of scandium
bond types of 1,1,2-trimethylcyclopropane
color of technetium vs xenon