Search

KMnO4 + NaNO2 = NO2 + K2MnO4 + Na2MnO4

Input interpretation

KMnO_4 potassium permanganate + NaNO_2 sodium nitrite ⟶ NO_2 nitrogen dioxide + K_2MnO_4 potassium manganate + Na2MnO4
KMnO_4 potassium permanganate + NaNO_2 sodium nitrite ⟶ NO_2 nitrogen dioxide + K_2MnO_4 potassium manganate + Na2MnO4

Balanced equation

Balance the chemical equation algebraically: KMnO_4 + NaNO_2 ⟶ NO_2 + K_2MnO_4 + Na2MnO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 NaNO_2 ⟶ c_3 NO_2 + c_4 K_2MnO_4 + c_5 Na2MnO4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, N and Na: K: | c_1 = 2 c_4 Mn: | c_1 = c_4 + c_5 O: | 4 c_1 + 2 c_2 = 2 c_3 + 4 c_4 + 4 c_5 N: | c_2 = c_3 Na: | c_2 = 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 = 2 c_2 = 2 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KMnO_4 + 2 NaNO_2 ⟶ 2 NO_2 + K_2MnO_4 + Na2MnO4
Balance the chemical equation algebraically: KMnO_4 + NaNO_2 ⟶ NO_2 + K_2MnO_4 + Na2MnO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KMnO_4 + c_2 NaNO_2 ⟶ c_3 NO_2 + c_4 K_2MnO_4 + c_5 Na2MnO4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, N and Na: K: | c_1 = 2 c_4 Mn: | c_1 = c_4 + c_5 O: | 4 c_1 + 2 c_2 = 2 c_3 + 4 c_4 + 4 c_5 N: | c_2 = c_3 Na: | c_2 = 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 = 2 c_2 = 2 c_3 = 2 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KMnO_4 + 2 NaNO_2 ⟶ 2 NO_2 + K_2MnO_4 + Na2MnO4

Structures

+ ⟶ + + Na2MnO4
+ ⟶ + + Na2MnO4

Names

potassium permanganate + sodium nitrite ⟶ nitrogen dioxide + potassium manganate + Na2MnO4
potassium permanganate + sodium nitrite ⟶ nitrogen dioxide + potassium manganate + Na2MnO4

Equilibrium constant

Construct the equilibrium constant, K, expression for: KMnO_4 + NaNO_2 ⟶ NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 + 2 NaNO_2 ⟶ 2 NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 | 2 | -2 NaNO_2 | 2 | -2 NO_2 | 2 | 2 K_2MnO_4 | 1 | 1 Na2MnO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 2 | -2 | ([KMnO4])^(-2) NaNO_2 | 2 | -2 | ([NaNO2])^(-2) NO_2 | 2 | 2 | ([NO2])^2 K_2MnO_4 | 1 | 1 | [K2MnO4] Na2MnO4 | 1 | 1 | [Na2MnO4] 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 = ([KMnO4])^(-2) ([NaNO2])^(-2) ([NO2])^2 [K2MnO4] [Na2MnO4] = (([NO2])^2 [K2MnO4] [Na2MnO4])/(([KMnO4])^2 ([NaNO2])^2)
Construct the equilibrium constant, K, expression for: KMnO_4 + NaNO_2 ⟶ NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 + 2 NaNO_2 ⟶ 2 NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 | 2 | -2 NaNO_2 | 2 | -2 NO_2 | 2 | 2 K_2MnO_4 | 1 | 1 Na2MnO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KMnO_4 | 2 | -2 | ([KMnO4])^(-2) NaNO_2 | 2 | -2 | ([NaNO2])^(-2) NO_2 | 2 | 2 | ([NO2])^2 K_2MnO_4 | 1 | 1 | [K2MnO4] Na2MnO4 | 1 | 1 | [Na2MnO4] 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 = ([KMnO4])^(-2) ([NaNO2])^(-2) ([NO2])^2 [K2MnO4] [Na2MnO4] = (([NO2])^2 [K2MnO4] [Na2MnO4])/(([KMnO4])^2 ([NaNO2])^2)

Rate of reaction

Construct the rate of reaction expression for: KMnO_4 + NaNO_2 ⟶ NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 + 2 NaNO_2 ⟶ 2 NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 | 2 | -2 NaNO_2 | 2 | -2 NO_2 | 2 | 2 K_2MnO_4 | 1 | 1 Na2MnO4 | 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 KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) NaNO_2 | 2 | -2 | -1/2 (Δ[NaNO2])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) K_2MnO_4 | 1 | 1 | (Δ[K2MnO4])/(Δt) Na2MnO4 | 1 | 1 | (Δ[Na2MnO4])/(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[KMnO4])/(Δt) = -1/2 (Δ[NaNO2])/(Δt) = 1/2 (Δ[NO2])/(Δt) = (Δ[K2MnO4])/(Δt) = (Δ[Na2MnO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KMnO_4 + NaNO_2 ⟶ NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 + 2 NaNO_2 ⟶ 2 NO_2 + K_2MnO_4 + Na2MnO4 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 KMnO_4 | 2 | -2 NaNO_2 | 2 | -2 NO_2 | 2 | 2 K_2MnO_4 | 1 | 1 Na2MnO4 | 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 KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) NaNO_2 | 2 | -2 | -1/2 (Δ[NaNO2])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) K_2MnO_4 | 1 | 1 | (Δ[K2MnO4])/(Δt) Na2MnO4 | 1 | 1 | (Δ[Na2MnO4])/(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[KMnO4])/(Δt) = -1/2 (Δ[NaNO2])/(Δt) = 1/2 (Δ[NO2])/(Δt) = (Δ[K2MnO4])/(Δt) = (Δ[Na2MnO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium permanganate | sodium nitrite | nitrogen dioxide | potassium manganate | Na2MnO4 formula | KMnO_4 | NaNO_2 | NO_2 | K_2MnO_4 | Na2MnO4 Hill formula | KMnO_4 | NNaO_2 | NO_2 | K_2MnO_4 | MnNa2O4 name | potassium permanganate | sodium nitrite | nitrogen dioxide | potassium manganate | IUPAC name | potassium permanganate | sodium nitrite | Nitrogen dioxide | dipotassium dioxido-dioxomanganese |
| potassium permanganate | sodium nitrite | nitrogen dioxide | potassium manganate | Na2MnO4 formula | KMnO_4 | NaNO_2 | NO_2 | K_2MnO_4 | Na2MnO4 Hill formula | KMnO_4 | NNaO_2 | NO_2 | K_2MnO_4 | MnNa2O4 name | potassium permanganate | sodium nitrite | nitrogen dioxide | potassium manganate | IUPAC name | potassium permanganate | sodium nitrite | Nitrogen dioxide | dipotassium dioxido-dioxomanganese |

Substance properties

| potassium permanganate | sodium nitrite | nitrogen dioxide | potassium manganate | Na2MnO4 molar mass | 158.03 g/mol | 68.995 g/mol | 46.005 g/mol | 197.13 g/mol | 164.91 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | melting point | 240 °C | 271 °C | -11 °C | 190 °C | boiling point | | | 21 °C | | density | 1 g/cm^3 | 2.168 g/cm^3 | 0.00188 g/cm^3 (at 25 °C) | | solubility in water | | | reacts | decomposes | dynamic viscosity | | | 4.02×10^-4 Pa s (at 25 °C) | | odor | odorless | | | |
| potassium permanganate | sodium nitrite | nitrogen dioxide | potassium manganate | Na2MnO4 molar mass | 158.03 g/mol | 68.995 g/mol | 46.005 g/mol | 197.13 g/mol | 164.91 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | melting point | 240 °C | 271 °C | -11 °C | 190 °C | boiling point | | | 21 °C | | density | 1 g/cm^3 | 2.168 g/cm^3 | 0.00188 g/cm^3 (at 25 °C) | | solubility in water | | | reacts | decomposes | dynamic viscosity | | | 4.02×10^-4 Pa s (at 25 °C) | | odor | odorless | | | |

Units

Random Queries

melting point of potassium hexachloroosmate(IV)
Cl2 + NaOH + MnCl2 = H2O + NaCl + MnO2
Ca(OH)2 + (NH4)2SO4 = H2O + NH3 + CaSO4
name of rubidium bromide
formula of barium cation vs magnesium cation
ion class of palladium(III) cation vs mercury(II) cation
molar magnetic susceptibilities of reductants
molar mass of ammonium cerium(IV) sulfate hydrate
InChI identifier of lead tetrachloride
HNO3 + P = H2O + NO2 + HPO3