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S + KNO3 = K2SO4 + SO2 + N2

Input interpretation

S mixed sulfur + KNO_3 potassium nitrate ⟶ K_2SO_4 potassium sulfate + SO_2 sulfur dioxide + N_2 nitrogen
S mixed sulfur + KNO_3 potassium nitrate ⟶ K_2SO_4 potassium sulfate + SO_2 sulfur dioxide + N_2 nitrogen

Balanced equation

Balance the chemical equation algebraically: S + KNO_3 ⟶ K_2SO_4 + SO_2 + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 S + c_2 KNO_3 ⟶ c_3 K_2SO_4 + c_4 SO_2 + c_5 N_2 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 + c_4 K: | c_2 = 2 c_3 N: | c_2 = 2 c_5 O: | 3 c_2 = 4 c_3 + 2 c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 S + 2 KNO_3 ⟶ K_2SO_4 + SO_2 + N_2
Balance the chemical equation algebraically: S + KNO_3 ⟶ K_2SO_4 + SO_2 + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 S + c_2 KNO_3 ⟶ c_3 K_2SO_4 + c_4 SO_2 + c_5 N_2 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 + c_4 K: | c_2 = 2 c_3 N: | c_2 = 2 c_5 O: | 3 c_2 = 4 c_3 + 2 c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 S + 2 KNO_3 ⟶ K_2SO_4 + SO_2 + N_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

mixed sulfur + potassium nitrate ⟶ potassium sulfate + sulfur dioxide + nitrogen
mixed sulfur + potassium nitrate ⟶ potassium sulfate + sulfur dioxide + nitrogen

Equilibrium constant

Construct the equilibrium constant, K, expression for: S + KNO_3 ⟶ K_2SO_4 + SO_2 + N_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: 2 S + 2 KNO_3 ⟶ K_2SO_4 + SO_2 + N_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 S | 2 | -2 KNO_3 | 2 | -2 K_2SO_4 | 1 | 1 SO_2 | 1 | 1 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression S | 2 | -2 | ([S])^(-2) KNO_3 | 2 | -2 | ([KNO3])^(-2) K_2SO_4 | 1 | 1 | [K2SO4] SO_2 | 1 | 1 | [SO2] N_2 | 1 | 1 | [N2] 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])^(-2) ([KNO3])^(-2) [K2SO4] [SO2] [N2] = ([K2SO4] [SO2] [N2])/(([S])^2 ([KNO3])^2)
Construct the equilibrium constant, K, expression for: S + KNO_3 ⟶ K_2SO_4 + SO_2 + N_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: 2 S + 2 KNO_3 ⟶ K_2SO_4 + SO_2 + N_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 S | 2 | -2 KNO_3 | 2 | -2 K_2SO_4 | 1 | 1 SO_2 | 1 | 1 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression S | 2 | -2 | ([S])^(-2) KNO_3 | 2 | -2 | ([KNO3])^(-2) K_2SO_4 | 1 | 1 | [K2SO4] SO_2 | 1 | 1 | [SO2] N_2 | 1 | 1 | [N2] 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])^(-2) ([KNO3])^(-2) [K2SO4] [SO2] [N2] = ([K2SO4] [SO2] [N2])/(([S])^2 ([KNO3])^2)

Rate of reaction

Construct the rate of reaction expression for: S + KNO_3 ⟶ K_2SO_4 + SO_2 + N_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: 2 S + 2 KNO_3 ⟶ K_2SO_4 + SO_2 + N_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 S | 2 | -2 KNO_3 | 2 | -2 K_2SO_4 | 1 | 1 SO_2 | 1 | 1 N_2 | 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 S | 2 | -2 | -1/2 (Δ[S])/(Δt) KNO_3 | 2 | -2 | -1/2 (Δ[KNO3])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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[S])/(Δt) = -1/2 (Δ[KNO3])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[SO2])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: S + KNO_3 ⟶ K_2SO_4 + SO_2 + N_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: 2 S + 2 KNO_3 ⟶ K_2SO_4 + SO_2 + N_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 S | 2 | -2 KNO_3 | 2 | -2 K_2SO_4 | 1 | 1 SO_2 | 1 | 1 N_2 | 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 S | 2 | -2 | -1/2 (Δ[S])/(Δt) KNO_3 | 2 | -2 | -1/2 (Δ[KNO3])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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[S])/(Δt) = -1/2 (Δ[KNO3])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[SO2])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| mixed sulfur | potassium nitrate | potassium sulfate | sulfur dioxide | nitrogen formula | S | KNO_3 | K_2SO_4 | SO_2 | N_2 Hill formula | S | KNO_3 | K_2O_4S | O_2S | N_2 name | mixed sulfur | potassium nitrate | potassium sulfate | sulfur dioxide | nitrogen IUPAC name | sulfur | potassium nitrate | dipotassium sulfate | sulfur dioxide | molecular nitrogen
| mixed sulfur | potassium nitrate | potassium sulfate | sulfur dioxide | nitrogen formula | S | KNO_3 | K_2SO_4 | SO_2 | N_2 Hill formula | S | KNO_3 | K_2O_4S | O_2S | N_2 name | mixed sulfur | potassium nitrate | potassium sulfate | sulfur dioxide | nitrogen IUPAC name | sulfur | potassium nitrate | dipotassium sulfate | sulfur dioxide | molecular nitrogen

Substance properties

| mixed sulfur | potassium nitrate | potassium sulfate | sulfur dioxide | nitrogen molar mass | 32.06 g/mol | 101.1 g/mol | 174.25 g/mol | 64.06 g/mol | 28.014 g/mol phase | solid (at STP) | solid (at STP) | | gas (at STP) | gas (at STP) melting point | 112.8 °C | 334 °C | | -73 °C | -210 °C boiling point | 444.7 °C | | | -10 °C | -195.79 °C density | 2.07 g/cm^3 | | | 0.002619 g/cm^3 (at 25 °C) | 0.001251 g/cm^3 (at 0 °C) solubility in water | | soluble | soluble | | insoluble surface tension | | | | 0.02859 N/m | 0.0066 N/m dynamic viscosity | | | | 1.282×10^-5 Pa s (at 25 °C) | 1.78×10^-5 Pa s (at 25 °C) odor | | odorless | | | odorless
| mixed sulfur | potassium nitrate | potassium sulfate | sulfur dioxide | nitrogen molar mass | 32.06 g/mol | 101.1 g/mol | 174.25 g/mol | 64.06 g/mol | 28.014 g/mol phase | solid (at STP) | solid (at STP) | | gas (at STP) | gas (at STP) melting point | 112.8 °C | 334 °C | | -73 °C | -210 °C boiling point | 444.7 °C | | | -10 °C | -195.79 °C density | 2.07 g/cm^3 | | | 0.002619 g/cm^3 (at 25 °C) | 0.001251 g/cm^3 (at 0 °C) solubility in water | | soluble | soluble | | insoluble surface tension | | | | 0.02859 N/m | 0.0066 N/m dynamic viscosity | | | | 1.282×10^-5 Pa s (at 25 °C) | 1.78×10^-5 Pa s (at 25 °C) odor | | odorless | | | odorless

Units

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