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KNO3 + Cr2S3 = K2SO4 + NO + K2CrO4

Input interpretation

KNO_3 potassium nitrate + Cr_2S_3 chromium(III) sulfide ⟶ K_2SO_4 potassium sulfate + NO nitric oxide + K_2CrO_4 potassium chromate
KNO_3 potassium nitrate + Cr_2S_3 chromium(III) sulfide ⟶ K_2SO_4 potassium sulfate + NO nitric oxide + K_2CrO_4 potassium chromate

Balanced equation

Balance the chemical equation algebraically: KNO_3 + Cr_2S_3 ⟶ K_2SO_4 + NO + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KNO_3 + c_2 Cr_2S_3 ⟶ c_3 K_2SO_4 + c_4 NO + c_5 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, N, O, Cr and S: K: | c_1 = 2 c_3 + 2 c_5 N: | c_1 = c_4 O: | 3 c_1 = 4 c_3 + c_4 + 4 c_5 Cr: | 2 c_2 = c_5 S: | 3 c_2 = c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 1 c_3 = 3 c_4 = 10 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 KNO_3 + Cr_2S_3 ⟶ 3 K_2SO_4 + 10 NO + 2 K_2CrO_4
Balance the chemical equation algebraically: KNO_3 + Cr_2S_3 ⟶ K_2SO_4 + NO + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KNO_3 + c_2 Cr_2S_3 ⟶ c_3 K_2SO_4 + c_4 NO + c_5 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, N, O, Cr and S: K: | c_1 = 2 c_3 + 2 c_5 N: | c_1 = c_4 O: | 3 c_1 = 4 c_3 + c_4 + 4 c_5 Cr: | 2 c_2 = c_5 S: | 3 c_2 = c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 1 c_3 = 3 c_4 = 10 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 KNO_3 + Cr_2S_3 ⟶ 3 K_2SO_4 + 10 NO + 2 K_2CrO_4

Structures

+ ⟶ + +
+ ⟶ + +

Names

potassium nitrate + chromium(III) sulfide ⟶ potassium sulfate + nitric oxide + potassium chromate
potassium nitrate + chromium(III) sulfide ⟶ potassium sulfate + nitric oxide + potassium chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KNO_3 + Cr_2S_3 ⟶ K_2SO_4 + NO + K_2CrO_4 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: 10 KNO_3 + Cr_2S_3 ⟶ 3 K_2SO_4 + 10 NO + 2 K_2CrO_4 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 KNO_3 | 10 | -10 Cr_2S_3 | 1 | -1 K_2SO_4 | 3 | 3 NO | 10 | 10 K_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KNO_3 | 10 | -10 | ([KNO3])^(-10) Cr_2S_3 | 1 | -1 | ([Cr2S3])^(-1) K_2SO_4 | 3 | 3 | ([K2SO4])^3 NO | 10 | 10 | ([NO])^10 K_2CrO_4 | 2 | 2 | ([K2CrO4])^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 = ([KNO3])^(-10) ([Cr2S3])^(-1) ([K2SO4])^3 ([NO])^10 ([K2CrO4])^2 = (([K2SO4])^3 ([NO])^10 ([K2CrO4])^2)/(([KNO3])^10 [Cr2S3])
Construct the equilibrium constant, K, expression for: KNO_3 + Cr_2S_3 ⟶ K_2SO_4 + NO + K_2CrO_4 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: 10 KNO_3 + Cr_2S_3 ⟶ 3 K_2SO_4 + 10 NO + 2 K_2CrO_4 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 KNO_3 | 10 | -10 Cr_2S_3 | 1 | -1 K_2SO_4 | 3 | 3 NO | 10 | 10 K_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KNO_3 | 10 | -10 | ([KNO3])^(-10) Cr_2S_3 | 1 | -1 | ([Cr2S3])^(-1) K_2SO_4 | 3 | 3 | ([K2SO4])^3 NO | 10 | 10 | ([NO])^10 K_2CrO_4 | 2 | 2 | ([K2CrO4])^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 = ([KNO3])^(-10) ([Cr2S3])^(-1) ([K2SO4])^3 ([NO])^10 ([K2CrO4])^2 = (([K2SO4])^3 ([NO])^10 ([K2CrO4])^2)/(([KNO3])^10 [Cr2S3])

Rate of reaction

Construct the rate of reaction expression for: KNO_3 + Cr_2S_3 ⟶ K_2SO_4 + NO + K_2CrO_4 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: 10 KNO_3 + Cr_2S_3 ⟶ 3 K_2SO_4 + 10 NO + 2 K_2CrO_4 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 KNO_3 | 10 | -10 Cr_2S_3 | 1 | -1 K_2SO_4 | 3 | 3 NO | 10 | 10 K_2CrO_4 | 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 KNO_3 | 10 | -10 | -1/10 (Δ[KNO3])/(Δt) Cr_2S_3 | 1 | -1 | -(Δ[Cr2S3])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) NO | 10 | 10 | 1/10 (Δ[NO])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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 = -1/10 (Δ[KNO3])/(Δt) = -(Δ[Cr2S3])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/10 (Δ[NO])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KNO_3 + Cr_2S_3 ⟶ K_2SO_4 + NO + K_2CrO_4 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: 10 KNO_3 + Cr_2S_3 ⟶ 3 K_2SO_4 + 10 NO + 2 K_2CrO_4 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 KNO_3 | 10 | -10 Cr_2S_3 | 1 | -1 K_2SO_4 | 3 | 3 NO | 10 | 10 K_2CrO_4 | 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 KNO_3 | 10 | -10 | -1/10 (Δ[KNO3])/(Δt) Cr_2S_3 | 1 | -1 | -(Δ[Cr2S3])/(Δt) K_2SO_4 | 3 | 3 | 1/3 (Δ[K2SO4])/(Δt) NO | 10 | 10 | 1/10 (Δ[NO])/(Δt) K_2CrO_4 | 2 | 2 | 1/2 (Δ[K2CrO4])/(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 = -1/10 (Δ[KNO3])/(Δt) = -(Δ[Cr2S3])/(Δt) = 1/3 (Δ[K2SO4])/(Δt) = 1/10 (Δ[NO])/(Δt) = 1/2 (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium nitrate | chromium(III) sulfide | potassium sulfate | nitric oxide | potassium chromate formula | KNO_3 | Cr_2S_3 | K_2SO_4 | NO | K_2CrO_4 Hill formula | KNO_3 | Cr_2S_3 | K_2O_4S | NO | CrK_2O_4 name | potassium nitrate | chromium(III) sulfide | potassium sulfate | nitric oxide | potassium chromate IUPAC name | potassium nitrate | chromium(+3) cation trisulfide | dipotassium sulfate | nitric oxide | dipotassium dioxido-dioxochromium
| potassium nitrate | chromium(III) sulfide | potassium sulfate | nitric oxide | potassium chromate formula | KNO_3 | Cr_2S_3 | K_2SO_4 | NO | K_2CrO_4 Hill formula | KNO_3 | Cr_2S_3 | K_2O_4S | NO | CrK_2O_4 name | potassium nitrate | chromium(III) sulfide | potassium sulfate | nitric oxide | potassium chromate IUPAC name | potassium nitrate | chromium(+3) cation trisulfide | dipotassium sulfate | nitric oxide | dipotassium dioxido-dioxochromium

Substance properties

| potassium nitrate | chromium(III) sulfide | potassium sulfate | nitric oxide | potassium chromate molar mass | 101.1 g/mol | 200.2 g/mol | 174.25 g/mol | 30.006 g/mol | 194.19 g/mol phase | solid (at STP) | | | gas (at STP) | solid (at STP) melting point | 334 °C | | | -163.6 °C | 971 °C boiling point | | | | -151.7 °C | density | | 3.77 g/cm^3 | | 0.001226 g/cm^3 (at 25 °C) | 2.73 g/cm^3 solubility in water | soluble | | soluble | | soluble dynamic viscosity | | | | 1.911×10^-5 Pa s (at 25 °C) | odor | odorless | | | | odorless
| potassium nitrate | chromium(III) sulfide | potassium sulfate | nitric oxide | potassium chromate molar mass | 101.1 g/mol | 200.2 g/mol | 174.25 g/mol | 30.006 g/mol | 194.19 g/mol phase | solid (at STP) | | | gas (at STP) | solid (at STP) melting point | 334 °C | | | -163.6 °C | 971 °C boiling point | | | | -151.7 °C | density | | 3.77 g/cm^3 | | 0.001226 g/cm^3 (at 25 °C) | 2.73 g/cm^3 solubility in water | soluble | | soluble | | soluble dynamic viscosity | | | | 1.911×10^-5 Pa s (at 25 °C) | odor | odorless | | | | odorless

Units

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