Search

H2O + HNO3 + As2S5 = S + NO + H3AsO4

Input interpretation

H_2O water + HNO_3 nitric acid + As_2S_5 arsenic(V) sulfide ⟶ S mixed sulfur + NO nitric oxide + H_3AsO_4 arsenic acid, solid
H_2O water + HNO_3 nitric acid + As_2S_5 arsenic(V) sulfide ⟶ S mixed sulfur + NO nitric oxide + H_3AsO_4 arsenic acid, solid

Balanced equation

Balance the chemical equation algebraically: H_2O + HNO_3 + As_2S_5 ⟶ S + NO + H_3AsO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 As_2S_5 ⟶ c_4 S + c_5 NO + c_6 H_3AsO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N, As and S: H: | 2 c_1 + c_2 = 3 c_6 O: | c_1 + 3 c_2 = c_5 + 4 c_6 N: | c_2 = c_5 As: | 2 c_3 = c_6 S: | 5 c_3 = 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 = 4/3 c_2 = 10/3 c_3 = 1 c_4 = 5 c_5 = 10/3 c_6 = 2 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 4 c_2 = 10 c_3 = 3 c_4 = 15 c_5 = 10 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 10 HNO_3 + 3 As_2S_5 ⟶ 15 S + 10 NO + 6 H_3AsO_4
Balance the chemical equation algebraically: H_2O + HNO_3 + As_2S_5 ⟶ S + NO + H_3AsO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 HNO_3 + c_3 As_2S_5 ⟶ c_4 S + c_5 NO + c_6 H_3AsO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, N, As and S: H: | 2 c_1 + c_2 = 3 c_6 O: | c_1 + 3 c_2 = c_5 + 4 c_6 N: | c_2 = c_5 As: | 2 c_3 = c_6 S: | 5 c_3 = 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 = 4/3 c_2 = 10/3 c_3 = 1 c_4 = 5 c_5 = 10/3 c_6 = 2 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 4 c_2 = 10 c_3 = 3 c_4 = 15 c_5 = 10 c_6 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 10 HNO_3 + 3 As_2S_5 ⟶ 15 S + 10 NO + 6 H_3AsO_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

water + nitric acid + arsenic(V) sulfide ⟶ mixed sulfur + nitric oxide + arsenic acid, solid
water + nitric acid + arsenic(V) sulfide ⟶ mixed sulfur + nitric oxide + arsenic acid, solid

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + As_2S_5 ⟶ S + NO + H_3AsO_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: 4 H_2O + 10 HNO_3 + 3 As_2S_5 ⟶ 15 S + 10 NO + 6 H_3AsO_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 H_2O | 4 | -4 HNO_3 | 10 | -10 As_2S_5 | 3 | -3 S | 15 | 15 NO | 10 | 10 H_3AsO_4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) HNO_3 | 10 | -10 | ([HNO3])^(-10) As_2S_5 | 3 | -3 | ([As2S5])^(-3) S | 15 | 15 | ([S])^15 NO | 10 | 10 | ([NO])^10 H_3AsO_4 | 6 | 6 | ([H3AsO4])^6 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 = ([H2O])^(-4) ([HNO3])^(-10) ([As2S5])^(-3) ([S])^15 ([NO])^10 ([H3AsO4])^6 = (([S])^15 ([NO])^10 ([H3AsO4])^6)/(([H2O])^4 ([HNO3])^10 ([As2S5])^3)
Construct the equilibrium constant, K, expression for: H_2O + HNO_3 + As_2S_5 ⟶ S + NO + H_3AsO_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: 4 H_2O + 10 HNO_3 + 3 As_2S_5 ⟶ 15 S + 10 NO + 6 H_3AsO_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 H_2O | 4 | -4 HNO_3 | 10 | -10 As_2S_5 | 3 | -3 S | 15 | 15 NO | 10 | 10 H_3AsO_4 | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) HNO_3 | 10 | -10 | ([HNO3])^(-10) As_2S_5 | 3 | -3 | ([As2S5])^(-3) S | 15 | 15 | ([S])^15 NO | 10 | 10 | ([NO])^10 H_3AsO_4 | 6 | 6 | ([H3AsO4])^6 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 = ([H2O])^(-4) ([HNO3])^(-10) ([As2S5])^(-3) ([S])^15 ([NO])^10 ([H3AsO4])^6 = (([S])^15 ([NO])^10 ([H3AsO4])^6)/(([H2O])^4 ([HNO3])^10 ([As2S5])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2O + HNO_3 + As_2S_5 ⟶ S + NO + H_3AsO_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: 4 H_2O + 10 HNO_3 + 3 As_2S_5 ⟶ 15 S + 10 NO + 6 H_3AsO_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 H_2O | 4 | -4 HNO_3 | 10 | -10 As_2S_5 | 3 | -3 S | 15 | 15 NO | 10 | 10 H_3AsO_4 | 6 | 6 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_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) As_2S_5 | 3 | -3 | -1/3 (Δ[As2S5])/(Δt) S | 15 | 15 | 1/15 (Δ[S])/(Δt) NO | 10 | 10 | 1/10 (Δ[NO])/(Δt) H_3AsO_4 | 6 | 6 | 1/6 (Δ[H3AsO4])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/10 (Δ[HNO3])/(Δt) = -1/3 (Δ[As2S5])/(Δt) = 1/15 (Δ[S])/(Δt) = 1/10 (Δ[NO])/(Δt) = 1/6 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + HNO_3 + As_2S_5 ⟶ S + NO + H_3AsO_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: 4 H_2O + 10 HNO_3 + 3 As_2S_5 ⟶ 15 S + 10 NO + 6 H_3AsO_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 H_2O | 4 | -4 HNO_3 | 10 | -10 As_2S_5 | 3 | -3 S | 15 | 15 NO | 10 | 10 H_3AsO_4 | 6 | 6 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_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) As_2S_5 | 3 | -3 | -1/3 (Δ[As2S5])/(Δt) S | 15 | 15 | 1/15 (Δ[S])/(Δt) NO | 10 | 10 | 1/10 (Δ[NO])/(Δt) H_3AsO_4 | 6 | 6 | 1/6 (Δ[H3AsO4])/(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 = -1/4 (Δ[H2O])/(Δt) = -1/10 (Δ[HNO3])/(Δt) = -1/3 (Δ[As2S5])/(Δt) = 1/15 (Δ[S])/(Δt) = 1/10 (Δ[NO])/(Δt) = 1/6 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | nitric acid | arsenic(V) sulfide | mixed sulfur | nitric oxide | arsenic acid, solid formula | H_2O | HNO_3 | As_2S_5 | S | NO | H_3AsO_4 Hill formula | H_2O | HNO_3 | As_2S_5 | S | NO | AsH_3O_4 name | water | nitric acid | arsenic(V) sulfide | mixed sulfur | nitric oxide | arsenic acid, solid IUPAC name | water | nitric acid | | sulfur | nitric oxide | arsoric acid
| water | nitric acid | arsenic(V) sulfide | mixed sulfur | nitric oxide | arsenic acid, solid formula | H_2O | HNO_3 | As_2S_5 | S | NO | H_3AsO_4 Hill formula | H_2O | HNO_3 | As_2S_5 | S | NO | AsH_3O_4 name | water | nitric acid | arsenic(V) sulfide | mixed sulfur | nitric oxide | arsenic acid, solid IUPAC name | water | nitric acid | | sulfur | nitric oxide | arsoric acid

Random Queries

chemical types of selenium tetrafluoride
Hill formula of sodium hydride vs cesium iodide
longest aliphatic chain length of 2,2,3,3-tetrafluoropropyl acrylate
group of tantalum vs molybdenum
formula of hafnium vs yttrium(III)nitrate tetrahydrate
structure diagram of hydrogen carbonate anion vs copper(II) cation
alternate names of calcium chloride dihydrate
molar mass of perrhenic acid vs rhodium dioxide
name of IR-895
alternate names of sodium erythorbate