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S + KNO3 = SO2 + NO + K2O

Input interpretation

S mixed sulfur + KNO_3 potassium nitrate ⟶ SO_2 sulfur dioxide + NO nitric oxide + K_2O potassium oxide
S mixed sulfur + KNO_3 potassium nitrate ⟶ SO_2 sulfur dioxide + NO nitric oxide + K_2O potassium oxide

Balanced equation

Balance the chemical equation algebraically: S + KNO_3 ⟶ SO_2 + NO + K_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 S + c_2 KNO_3 ⟶ c_3 SO_2 + c_4 NO + c_5 K_2O Set the number of atoms in the reactants equal to the number of atoms in the products for S, K, N and O: S: | c_1 = c_3 K: | c_2 = 2 c_5 N: | c_2 = c_4 O: | 3 c_2 = 2 c_3 + c_4 + 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 2 c_3 = 3/2 c_4 = 2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 4 c_3 = 3 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 S + 4 KNO_3 ⟶ 3 SO_2 + 4 NO + 2 K_2O
Balance the chemical equation algebraically: S + KNO_3 ⟶ SO_2 + NO + K_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 S + c_2 KNO_3 ⟶ c_3 SO_2 + c_4 NO + c_5 K_2O Set the number of atoms in the reactants equal to the number of atoms in the products for S, K, N and O: S: | c_1 = c_3 K: | c_2 = 2 c_5 N: | c_2 = c_4 O: | 3 c_2 = 2 c_3 + c_4 + 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 2 c_3 = 3/2 c_4 = 2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 4 c_3 = 3 c_4 = 4 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 S + 4 KNO_3 ⟶ 3 SO_2 + 4 NO + 2 K_2O

Structures

+ ⟶ + +
+ ⟶ + +

Names

mixed sulfur + potassium nitrate ⟶ sulfur dioxide + nitric oxide + potassium oxide
mixed sulfur + potassium nitrate ⟶ sulfur dioxide + nitric oxide + potassium oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: S + KNO_3 ⟶ SO_2 + NO + K_2O 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: 3 S + 4 KNO_3 ⟶ 3 SO_2 + 4 NO + 2 K_2O 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 S | 3 | -3 KNO_3 | 4 | -4 SO_2 | 3 | 3 NO | 4 | 4 K_2O | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression S | 3 | -3 | ([S])^(-3) KNO_3 | 4 | -4 | ([KNO3])^(-4) SO_2 | 3 | 3 | ([SO2])^3 NO | 4 | 4 | ([NO])^4 K_2O | 2 | 2 | ([K2O])^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 = ([S])^(-3) ([KNO3])^(-4) ([SO2])^3 ([NO])^4 ([K2O])^2 = (([SO2])^3 ([NO])^4 ([K2O])^2)/(([S])^3 ([KNO3])^4)
Construct the equilibrium constant, K, expression for: S + KNO_3 ⟶ SO_2 + NO + K_2O 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: 3 S + 4 KNO_3 ⟶ 3 SO_2 + 4 NO + 2 K_2O 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 S | 3 | -3 KNO_3 | 4 | -4 SO_2 | 3 | 3 NO | 4 | 4 K_2O | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression S | 3 | -3 | ([S])^(-3) KNO_3 | 4 | -4 | ([KNO3])^(-4) SO_2 | 3 | 3 | ([SO2])^3 NO | 4 | 4 | ([NO])^4 K_2O | 2 | 2 | ([K2O])^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 = ([S])^(-3) ([KNO3])^(-4) ([SO2])^3 ([NO])^4 ([K2O])^2 = (([SO2])^3 ([NO])^4 ([K2O])^2)/(([S])^3 ([KNO3])^4)

Rate of reaction

Construct the rate of reaction expression for: S + KNO_3 ⟶ SO_2 + NO + K_2O 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: 3 S + 4 KNO_3 ⟶ 3 SO_2 + 4 NO + 2 K_2O 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 S | 3 | -3 KNO_3 | 4 | -4 SO_2 | 3 | 3 NO | 4 | 4 K_2O | 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 S | 3 | -3 | -1/3 (Δ[S])/(Δt) KNO_3 | 4 | -4 | -1/4 (Δ[KNO3])/(Δt) SO_2 | 3 | 3 | 1/3 (Δ[SO2])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(Δt) K_2O | 2 | 2 | 1/2 (Δ[K2O])/(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 = -1/3 (Δ[S])/(Δt) = -1/4 (Δ[KNO3])/(Δt) = 1/3 (Δ[SO2])/(Δt) = 1/4 (Δ[NO])/(Δt) = 1/2 (Δ[K2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: S + KNO_3 ⟶ SO_2 + NO + K_2O 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: 3 S + 4 KNO_3 ⟶ 3 SO_2 + 4 NO + 2 K_2O 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 S | 3 | -3 KNO_3 | 4 | -4 SO_2 | 3 | 3 NO | 4 | 4 K_2O | 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 S | 3 | -3 | -1/3 (Δ[S])/(Δt) KNO_3 | 4 | -4 | -1/4 (Δ[KNO3])/(Δt) SO_2 | 3 | 3 | 1/3 (Δ[SO2])/(Δt) NO | 4 | 4 | 1/4 (Δ[NO])/(Δt) K_2O | 2 | 2 | 1/2 (Δ[K2O])/(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 = -1/3 (Δ[S])/(Δt) = -1/4 (Δ[KNO3])/(Δt) = 1/3 (Δ[SO2])/(Δt) = 1/4 (Δ[NO])/(Δt) = 1/2 (Δ[K2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| mixed sulfur | potassium nitrate | sulfur dioxide | nitric oxide | potassium oxide formula | S | KNO_3 | SO_2 | NO | K_2O Hill formula | S | KNO_3 | O_2S | NO | K_2O name | mixed sulfur | potassium nitrate | sulfur dioxide | nitric oxide | potassium oxide IUPAC name | sulfur | potassium nitrate | sulfur dioxide | nitric oxide | dipotassium oxygen(2-)
| mixed sulfur | potassium nitrate | sulfur dioxide | nitric oxide | potassium oxide formula | S | KNO_3 | SO_2 | NO | K_2O Hill formula | S | KNO_3 | O_2S | NO | K_2O name | mixed sulfur | potassium nitrate | sulfur dioxide | nitric oxide | potassium oxide IUPAC name | sulfur | potassium nitrate | sulfur dioxide | nitric oxide | dipotassium oxygen(2-)

Substance properties

| mixed sulfur | potassium nitrate | sulfur dioxide | nitric oxide | potassium oxide molar mass | 32.06 g/mol | 101.1 g/mol | 64.06 g/mol | 30.006 g/mol | 94.196 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | gas (at STP) | melting point | 112.8 °C | 334 °C | -73 °C | -163.6 °C | boiling point | 444.7 °C | | -10 °C | -151.7 °C | density | 2.07 g/cm^3 | | 0.002619 g/cm^3 (at 25 °C) | 0.001226 g/cm^3 (at 25 °C) | solubility in water | | soluble | | | surface tension | | | 0.02859 N/m | | dynamic viscosity | | | 1.282×10^-5 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | | odorless | | |
| mixed sulfur | potassium nitrate | sulfur dioxide | nitric oxide | potassium oxide molar mass | 32.06 g/mol | 101.1 g/mol | 64.06 g/mol | 30.006 g/mol | 94.196 g/mol phase | solid (at STP) | solid (at STP) | gas (at STP) | gas (at STP) | melting point | 112.8 °C | 334 °C | -73 °C | -163.6 °C | boiling point | 444.7 °C | | -10 °C | -151.7 °C | density | 2.07 g/cm^3 | | 0.002619 g/cm^3 (at 25 °C) | 0.001226 g/cm^3 (at 25 °C) | solubility in water | | soluble | | | surface tension | | | 0.02859 N/m | | dynamic viscosity | | | 1.282×10^-5 Pa s (at 25 °C) | 1.911×10^-5 Pa s (at 25 °C) | odor | | odorless | | |

Units

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