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H2SO4 + KNO2 = H2O + K2SO4 + NO + KNO3

Input interpretation

H_2SO_4 sulfuric acid + KNO_2 potassium nitrite ⟶ H_2O water + K_2SO_4 potassium sulfate + NO nitric oxide + KNO_3 potassium nitrate
H_2SO_4 sulfuric acid + KNO_2 potassium nitrite ⟶ H_2O water + K_2SO_4 potassium sulfate + NO nitric oxide + KNO_3 potassium nitrate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + NO + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KNO_2 ⟶ c_3 H_2O + c_4 K_2SO_4 + c_5 NO + c_6 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K and N: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 + c_5 + 3 c_6 S: | c_1 = c_4 K: | c_2 = 2 c_4 + c_6 N: | c_2 = c_5 + c_6 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 1 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 3 KNO_2 ⟶ H_2O + K_2SO_4 + 2 NO + KNO_3
Balance the chemical equation algebraically: H_2SO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + NO + KNO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KNO_2 ⟶ c_3 H_2O + c_4 K_2SO_4 + c_5 NO + c_6 KNO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, K and N: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 + c_5 + 3 c_6 S: | c_1 = c_4 K: | c_2 = 2 c_4 + c_6 N: | c_2 = c_5 + c_6 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 1 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 3 KNO_2 ⟶ H_2O + K_2SO_4 + 2 NO + KNO_3

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

sulfuric acid + potassium nitrite ⟶ water + potassium sulfate + nitric oxide + potassium nitrate
sulfuric acid + potassium nitrite ⟶ water + potassium sulfate + nitric oxide + potassium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + NO + KNO_3 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: H_2SO_4 + 3 KNO_2 ⟶ H_2O + K_2SO_4 + 2 NO + KNO_3 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 | 1 | -1 KNO_2 | 3 | -3 H_2O | 1 | 1 K_2SO_4 | 1 | 1 NO | 2 | 2 KNO_3 | 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 | 1 | -1 | ([H2SO4])^(-1) KNO_2 | 3 | -3 | ([KNO2])^(-3) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] NO | 2 | 2 | ([NO])^2 KNO_3 | 1 | 1 | [KNO3] 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])^(-1) ([KNO2])^(-3) [H2O] [K2SO4] ([NO])^2 [KNO3] = ([H2O] [K2SO4] ([NO])^2 [KNO3])/([H2SO4] ([KNO2])^3)
Construct the equilibrium constant, K, expression for: H_2SO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + NO + KNO_3 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: H_2SO_4 + 3 KNO_2 ⟶ H_2O + K_2SO_4 + 2 NO + KNO_3 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 | 1 | -1 KNO_2 | 3 | -3 H_2O | 1 | 1 K_2SO_4 | 1 | 1 NO | 2 | 2 KNO_3 | 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 | 1 | -1 | ([H2SO4])^(-1) KNO_2 | 3 | -3 | ([KNO2])^(-3) H_2O | 1 | 1 | [H2O] K_2SO_4 | 1 | 1 | [K2SO4] NO | 2 | 2 | ([NO])^2 KNO_3 | 1 | 1 | [KNO3] 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])^(-1) ([KNO2])^(-3) [H2O] [K2SO4] ([NO])^2 [KNO3] = ([H2O] [K2SO4] ([NO])^2 [KNO3])/([H2SO4] ([KNO2])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + NO + KNO_3 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: H_2SO_4 + 3 KNO_2 ⟶ H_2O + K_2SO_4 + 2 NO + KNO_3 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 | 1 | -1 KNO_2 | 3 | -3 H_2O | 1 | 1 K_2SO_4 | 1 | 1 NO | 2 | 2 KNO_3 | 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) KNO_2 | 3 | -3 | -1/3 (Δ[KNO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) KNO_3 | 1 | 1 | (Δ[KNO3])/(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 = -(Δ[H2SO4])/(Δt) = -1/3 (Δ[KNO2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + KNO_2 ⟶ H_2O + K_2SO_4 + NO + KNO_3 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: H_2SO_4 + 3 KNO_2 ⟶ H_2O + K_2SO_4 + 2 NO + KNO_3 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 | 1 | -1 KNO_2 | 3 | -3 H_2O | 1 | 1 K_2SO_4 | 1 | 1 NO | 2 | 2 KNO_3 | 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 | 1 | -1 | -(Δ[H2SO4])/(Δt) KNO_2 | 3 | -3 | -1/3 (Δ[KNO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) KNO_3 | 1 | 1 | (Δ[KNO3])/(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 = -(Δ[H2SO4])/(Δt) = -1/3 (Δ[KNO2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[KNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | potassium nitrite | water | potassium sulfate | nitric oxide | potassium nitrate formula | H_2SO_4 | KNO_2 | H_2O | K_2SO_4 | NO | KNO_3 Hill formula | H_2O_4S | KNO_2 | H_2O | K_2O_4S | NO | KNO_3 name | sulfuric acid | potassium nitrite | water | potassium sulfate | nitric oxide | potassium nitrate IUPAC name | sulfuric acid | potassium nitrite | water | dipotassium sulfate | nitric oxide | potassium nitrate
| sulfuric acid | potassium nitrite | water | potassium sulfate | nitric oxide | potassium nitrate formula | H_2SO_4 | KNO_2 | H_2O | K_2SO_4 | NO | KNO_3 Hill formula | H_2O_4S | KNO_2 | H_2O | K_2O_4S | NO | KNO_3 name | sulfuric acid | potassium nitrite | water | potassium sulfate | nitric oxide | potassium nitrate IUPAC name | sulfuric acid | potassium nitrite | water | dipotassium sulfate | nitric oxide | potassium nitrate

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