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HCl + NaNO3 + Au = HNO3 + NO + Na2O + HAuCl4

Input interpretation

HCl hydrogen chloride + NaNO_3 sodium nitrate + Au gold ⟶ HNO_3 nitric acid + NO nitric oxide + Na_2O sodium oxide + HAuCl_4·xH_2O gold(III) chloride hydrate
HCl hydrogen chloride + NaNO_3 sodium nitrate + Au gold ⟶ HNO_3 nitric acid + NO nitric oxide + Na_2O sodium oxide + HAuCl_4·xH_2O gold(III) chloride hydrate

Balanced equation

Balance the chemical equation algebraically: HCl + NaNO_3 + Au ⟶ HNO_3 + NO + Na_2O + HAuCl_4·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaNO_3 + c_3 Au ⟶ c_4 HNO_3 + c_5 NO + c_6 Na_2O + c_7 HAuCl_4·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, Na, O and Au: Cl: | c_1 = 4 c_7 H: | c_1 = c_4 + c_7 N: | c_2 = c_4 + c_5 Na: | c_2 = 2 c_6 O: | 3 c_2 = 3 c_4 + c_5 + c_6 Au: | c_3 = c_7 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 c_2 = 4 c_3 = 1 c_4 = 3 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + 4 NaNO_3 + Au ⟶ 3 HNO_3 + NO + 2 Na_2O + HAuCl_4·xH_2O
Balance the chemical equation algebraically: HCl + NaNO_3 + Au ⟶ HNO_3 + NO + Na_2O + HAuCl_4·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaNO_3 + c_3 Au ⟶ c_4 HNO_3 + c_5 NO + c_6 Na_2O + c_7 HAuCl_4·xH_2O Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, Na, O and Au: Cl: | c_1 = 4 c_7 H: | c_1 = c_4 + c_7 N: | c_2 = c_4 + c_5 Na: | c_2 = 2 c_6 O: | 3 c_2 = 3 c_4 + c_5 + c_6 Au: | c_3 = c_7 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 c_2 = 4 c_3 = 1 c_4 = 3 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + 4 NaNO_3 + Au ⟶ 3 HNO_3 + NO + 2 Na_2O + HAuCl_4·xH_2O

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

hydrogen chloride + sodium nitrate + gold ⟶ nitric acid + nitric oxide + sodium oxide + gold(III) chloride hydrate
hydrogen chloride + sodium nitrate + gold ⟶ nitric acid + nitric oxide + sodium oxide + gold(III) chloride hydrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + NaNO_3 + Au ⟶ HNO_3 + NO + Na_2O + HAuCl_4·xH_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: 4 HCl + 4 NaNO_3 + Au ⟶ 3 HNO_3 + NO + 2 Na_2O + HAuCl_4·xH_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 HCl | 4 | -4 NaNO_3 | 4 | -4 Au | 1 | -1 HNO_3 | 3 | 3 NO | 1 | 1 Na_2O | 2 | 2 HAuCl_4·xH_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) NaNO_3 | 4 | -4 | ([NaNO3])^(-4) Au | 1 | -1 | ([Au])^(-1) HNO_3 | 3 | 3 | ([HNO3])^3 NO | 1 | 1 | [NO] Na_2O | 2 | 2 | ([Na2O])^2 HAuCl_4·xH_2O | 1 | 1 | [HAuCl4·xH2O] 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 = ([HCl])^(-4) ([NaNO3])^(-4) ([Au])^(-1) ([HNO3])^3 [NO] ([Na2O])^2 [HAuCl4·xH2O] = (([HNO3])^3 [NO] ([Na2O])^2 [HAuCl4·xH2O])/(([HCl])^4 ([NaNO3])^4 [Au])
Construct the equilibrium constant, K, expression for: HCl + NaNO_3 + Au ⟶ HNO_3 + NO + Na_2O + HAuCl_4·xH_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: 4 HCl + 4 NaNO_3 + Au ⟶ 3 HNO_3 + NO + 2 Na_2O + HAuCl_4·xH_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 HCl | 4 | -4 NaNO_3 | 4 | -4 Au | 1 | -1 HNO_3 | 3 | 3 NO | 1 | 1 Na_2O | 2 | 2 HAuCl_4·xH_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) NaNO_3 | 4 | -4 | ([NaNO3])^(-4) Au | 1 | -1 | ([Au])^(-1) HNO_3 | 3 | 3 | ([HNO3])^3 NO | 1 | 1 | [NO] Na_2O | 2 | 2 | ([Na2O])^2 HAuCl_4·xH_2O | 1 | 1 | [HAuCl4·xH2O] 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 = ([HCl])^(-4) ([NaNO3])^(-4) ([Au])^(-1) ([HNO3])^3 [NO] ([Na2O])^2 [HAuCl4·xH2O] = (([HNO3])^3 [NO] ([Na2O])^2 [HAuCl4·xH2O])/(([HCl])^4 ([NaNO3])^4 [Au])

Rate of reaction

Construct the rate of reaction expression for: HCl + NaNO_3 + Au ⟶ HNO_3 + NO + Na_2O + HAuCl_4·xH_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: 4 HCl + 4 NaNO_3 + Au ⟶ 3 HNO_3 + NO + 2 Na_2O + HAuCl_4·xH_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 HCl | 4 | -4 NaNO_3 | 4 | -4 Au | 1 | -1 HNO_3 | 3 | 3 NO | 1 | 1 Na_2O | 2 | 2 HAuCl_4·xH_2O | 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 HCl | 4 | -4 | -1/4 (Δ[HCl])/(Δt) NaNO_3 | 4 | -4 | -1/4 (Δ[NaNO3])/(Δt) Au | 1 | -1 | -(Δ[Au])/(Δt) HNO_3 | 3 | 3 | 1/3 (Δ[HNO3])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) Na_2O | 2 | 2 | 1/2 (Δ[Na2O])/(Δt) HAuCl_4·xH_2O | 1 | 1 | (Δ[HAuCl4·xH2O])/(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[HCl])/(Δt) = -1/4 (Δ[NaNO3])/(Δt) = -(Δ[Au])/(Δt) = 1/3 (Δ[HNO3])/(Δt) = (Δ[NO])/(Δt) = 1/2 (Δ[Na2O])/(Δt) = (Δ[HAuCl4·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + NaNO_3 + Au ⟶ HNO_3 + NO + Na_2O + HAuCl_4·xH_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: 4 HCl + 4 NaNO_3 + Au ⟶ 3 HNO_3 + NO + 2 Na_2O + HAuCl_4·xH_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 HCl | 4 | -4 NaNO_3 | 4 | -4 Au | 1 | -1 HNO_3 | 3 | 3 NO | 1 | 1 Na_2O | 2 | 2 HAuCl_4·xH_2O | 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 HCl | 4 | -4 | -1/4 (Δ[HCl])/(Δt) NaNO_3 | 4 | -4 | -1/4 (Δ[NaNO3])/(Δt) Au | 1 | -1 | -(Δ[Au])/(Δt) HNO_3 | 3 | 3 | 1/3 (Δ[HNO3])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) Na_2O | 2 | 2 | 1/2 (Δ[Na2O])/(Δt) HAuCl_4·xH_2O | 1 | 1 | (Δ[HAuCl4·xH2O])/(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[HCl])/(Δt) = -1/4 (Δ[NaNO3])/(Δt) = -(Δ[Au])/(Δt) = 1/3 (Δ[HNO3])/(Δt) = (Δ[NO])/(Δt) = 1/2 (Δ[Na2O])/(Δt) = (Δ[HAuCl4·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | sodium nitrate | gold | nitric acid | nitric oxide | sodium oxide | gold(III) chloride hydrate formula | HCl | NaNO_3 | Au | HNO_3 | NO | Na_2O | HAuCl_4·xH_2O Hill formula | ClH | NNaO_3 | Au | HNO_3 | NO | Na_2O | AuCl_4H name | hydrogen chloride | sodium nitrate | gold | nitric acid | nitric oxide | sodium oxide | gold(III) chloride hydrate IUPAC name | hydrogen chloride | sodium nitrate | gold | nitric acid | nitric oxide | disodium oxygen(-2) anion | hydron; tetrachlorogold
| hydrogen chloride | sodium nitrate | gold | nitric acid | nitric oxide | sodium oxide | gold(III) chloride hydrate formula | HCl | NaNO_3 | Au | HNO_3 | NO | Na_2O | HAuCl_4·xH_2O Hill formula | ClH | NNaO_3 | Au | HNO_3 | NO | Na_2O | AuCl_4H name | hydrogen chloride | sodium nitrate | gold | nitric acid | nitric oxide | sodium oxide | gold(III) chloride hydrate IUPAC name | hydrogen chloride | sodium nitrate | gold | nitric acid | nitric oxide | disodium oxygen(-2) anion | hydron; tetrachlorogold

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