Search

HCl + HNO3 + Au = H2O + NO + HAuCl4

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + Au gold ⟶ H_2O water + NO nitric oxide + HAuCl_4·xH_2O gold(III) chloride hydrate
HCl hydrogen chloride + HNO_3 nitric acid + Au gold ⟶ H_2O water + NO nitric oxide + HAuCl_4·xH_2O gold(III) chloride hydrate

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + Au ⟶ H_2O + NO + HAuCl_4·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 Au ⟶ c_4 H_2O + c_5 NO + c_6 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, O and Au: Cl: | c_1 = 4 c_6 H: | c_1 + c_2 = 2 c_4 + c_6 N: | c_2 = c_5 O: | 3 c_2 = c_4 + c_5 Au: | c_3 = c_6 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 = 4 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + HNO_3 + Au ⟶ 2 H_2O + NO + HAuCl_4·xH_2O
Balance the chemical equation algebraically: HCl + HNO_3 + Au ⟶ H_2O + NO + HAuCl_4·xH_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 Au ⟶ c_4 H_2O + c_5 NO + c_6 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, O and Au: Cl: | c_1 = 4 c_6 H: | c_1 + c_2 = 2 c_4 + c_6 N: | c_2 = c_5 O: | 3 c_2 = c_4 + c_5 Au: | c_3 = c_6 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 = 4 c_2 = 1 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + HNO_3 + Au ⟶ 2 H_2O + NO + HAuCl_4·xH_2O

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + Au ⟶ H_2O + NO + 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 + HNO_3 + Au ⟶ 2 H_2O + NO + 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 HNO_3 | 1 | -1 Au | 1 | -1 H_2O | 2 | 2 NO | 1 | 1 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) HNO_3 | 1 | -1 | ([HNO3])^(-1) Au | 1 | -1 | ([Au])^(-1) H_2O | 2 | 2 | ([H2O])^2 NO | 1 | 1 | [NO] 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) ([HNO3])^(-1) ([Au])^(-1) ([H2O])^2 [NO] [HAuCl4·xH2O] = (([H2O])^2 [NO] [HAuCl4·xH2O])/(([HCl])^4 [HNO3] [Au])
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + Au ⟶ H_2O + NO + 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 + HNO_3 + Au ⟶ 2 H_2O + NO + 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 HNO_3 | 1 | -1 Au | 1 | -1 H_2O | 2 | 2 NO | 1 | 1 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) HNO_3 | 1 | -1 | ([HNO3])^(-1) Au | 1 | -1 | ([Au])^(-1) H_2O | 2 | 2 | ([H2O])^2 NO | 1 | 1 | [NO] 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) ([HNO3])^(-1) ([Au])^(-1) ([H2O])^2 [NO] [HAuCl4·xH2O] = (([H2O])^2 [NO] [HAuCl4·xH2O])/(([HCl])^4 [HNO3] [Au])

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + Au ⟶ H_2O + NO + 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 + HNO_3 + Au ⟶ 2 H_2O + NO + 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 HNO_3 | 1 | -1 Au | 1 | -1 H_2O | 2 | 2 NO | 1 | 1 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) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) Au | 1 | -1 | -(Δ[Au])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(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) = -(Δ[HNO3])/(Δt) = -(Δ[Au])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = (Δ[HAuCl4·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + Au ⟶ H_2O + NO + 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 + HNO_3 + Au ⟶ 2 H_2O + NO + 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 HNO_3 | 1 | -1 Au | 1 | -1 H_2O | 2 | 2 NO | 1 | 1 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) HNO_3 | 1 | -1 | -(Δ[HNO3])/(Δt) Au | 1 | -1 | -(Δ[Au])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(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) = -(Δ[HNO3])/(Δt) = -(Δ[Au])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = (Δ[HAuCl4·xH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | gold | water | nitric oxide | gold(III) chloride hydrate formula | HCl | HNO_3 | Au | H_2O | NO | HAuCl_4·xH_2O Hill formula | ClH | HNO_3 | Au | H_2O | NO | AuCl_4H name | hydrogen chloride | nitric acid | gold | water | nitric oxide | gold(III) chloride hydrate IUPAC name | hydrogen chloride | nitric acid | gold | water | nitric oxide | hydron; tetrachlorogold
| hydrogen chloride | nitric acid | gold | water | nitric oxide | gold(III) chloride hydrate formula | HCl | HNO_3 | Au | H_2O | NO | HAuCl_4·xH_2O Hill formula | ClH | HNO_3 | Au | H_2O | NO | AuCl_4H name | hydrogen chloride | nitric acid | gold | water | nitric oxide | gold(III) chloride hydrate IUPAC name | hydrogen chloride | nitric acid | gold | water | nitric oxide | hydron; tetrachlorogold

Random Queries

Zn + PbNO3 = Pb + ZnNO3
Mohs hardness of poor metals
IUPAC name of nitroprusside
alternate names of beryllium cation vs magnesium cation
molar mass of diamminesilver(I) cation vs lead(IV) cation
titanium(IV) cation vs vanadium(V) cation
chemical types of 1-vinylnaphthalene vs diphenylfulvene
freezing point of germanium telluride
alternate names of hemiaminal functional group
hydrocodone-N-methyl-d 3solution