Input interpretation
SnCl_2 stannous chloride + HAuCl_4·xH_2O gold(III) chloride hydrate ⟶ HCl hydrogen chloride + Au gold + SnCl_4 stannic chloride
Balanced equation
Balance the chemical equation algebraically: SnCl_2 + HAuCl_4·xH_2O ⟶ HCl + Au + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnCl_2 + c_2 HAuCl_4·xH_2O ⟶ c_3 HCl + c_4 Au + c_5 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Sn, Au and H: Cl: | 2 c_1 + 4 c_2 = c_3 + 4 c_5 Sn: | c_1 = c_5 Au: | c_2 = c_4 H: | 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 = 3/2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 2 c_3 = 2 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 SnCl_2 + 2 HAuCl_4·xH_2O ⟶ 2 HCl + 2 Au + 3 SnCl_4
Structures
+ ⟶ + +
Names
stannous chloride + gold(III) chloride hydrate ⟶ hydrogen chloride + gold + stannic chloride
Equilibrium constant
![Construct the equilibrium constant, K, expression for: SnCl_2 + HAuCl_4·xH_2O ⟶ HCl + Au + SnCl_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: 3 SnCl_2 + 2 HAuCl_4·xH_2O ⟶ 2 HCl + 2 Au + 3 SnCl_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 SnCl_2 | 3 | -3 HAuCl_4·xH_2O | 2 | -2 HCl | 2 | 2 Au | 2 | 2 SnCl_4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnCl_2 | 3 | -3 | ([SnCl2])^(-3) HAuCl_4·xH_2O | 2 | -2 | ([HAuCl4·xH2O])^(-2) HCl | 2 | 2 | ([HCl])^2 Au | 2 | 2 | ([Au])^2 SnCl_4 | 3 | 3 | ([SnCl4])^3 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 = ([SnCl2])^(-3) ([HAuCl4·xH2O])^(-2) ([HCl])^2 ([Au])^2 ([SnCl4])^3 = (([HCl])^2 ([Au])^2 ([SnCl4])^3)/(([SnCl2])^3 ([HAuCl4·xH2O])^2)](../image_source/50426c65065e7697f962ef803bf4cfea.png)
Construct the equilibrium constant, K, expression for: SnCl_2 + HAuCl_4·xH_2O ⟶ HCl + Au + SnCl_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: 3 SnCl_2 + 2 HAuCl_4·xH_2O ⟶ 2 HCl + 2 Au + 3 SnCl_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 SnCl_2 | 3 | -3 HAuCl_4·xH_2O | 2 | -2 HCl | 2 | 2 Au | 2 | 2 SnCl_4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnCl_2 | 3 | -3 | ([SnCl2])^(-3) HAuCl_4·xH_2O | 2 | -2 | ([HAuCl4·xH2O])^(-2) HCl | 2 | 2 | ([HCl])^2 Au | 2 | 2 | ([Au])^2 SnCl_4 | 3 | 3 | ([SnCl4])^3 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 = ([SnCl2])^(-3) ([HAuCl4·xH2O])^(-2) ([HCl])^2 ([Au])^2 ([SnCl4])^3 = (([HCl])^2 ([Au])^2 ([SnCl4])^3)/(([SnCl2])^3 ([HAuCl4·xH2O])^2)
Rate of reaction
![Construct the rate of reaction expression for: SnCl_2 + HAuCl_4·xH_2O ⟶ HCl + Au + SnCl_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: 3 SnCl_2 + 2 HAuCl_4·xH_2O ⟶ 2 HCl + 2 Au + 3 SnCl_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 SnCl_2 | 3 | -3 HAuCl_4·xH_2O | 2 | -2 HCl | 2 | 2 Au | 2 | 2 SnCl_4 | 3 | 3 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 SnCl_2 | 3 | -3 | -1/3 (Δ[SnCl2])/(Δt) HAuCl_4·xH_2O | 2 | -2 | -1/2 (Δ[HAuCl4·xH2O])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) Au | 2 | 2 | 1/2 (Δ[Au])/(Δt) SnCl_4 | 3 | 3 | 1/3 (Δ[SnCl4])/(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 = -1/3 (Δ[SnCl2])/(Δt) = -1/2 (Δ[HAuCl4·xH2O])/(Δt) = 1/2 (Δ[HCl])/(Δt) = 1/2 (Δ[Au])/(Δt) = 1/3 (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/22ee2f6643c329c32534667a4560f389.png)
Construct the rate of reaction expression for: SnCl_2 + HAuCl_4·xH_2O ⟶ HCl + Au + SnCl_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: 3 SnCl_2 + 2 HAuCl_4·xH_2O ⟶ 2 HCl + 2 Au + 3 SnCl_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 SnCl_2 | 3 | -3 HAuCl_4·xH_2O | 2 | -2 HCl | 2 | 2 Au | 2 | 2 SnCl_4 | 3 | 3 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 SnCl_2 | 3 | -3 | -1/3 (Δ[SnCl2])/(Δt) HAuCl_4·xH_2O | 2 | -2 | -1/2 (Δ[HAuCl4·xH2O])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) Au | 2 | 2 | 1/2 (Δ[Au])/(Δt) SnCl_4 | 3 | 3 | 1/3 (Δ[SnCl4])/(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 = -1/3 (Δ[SnCl2])/(Δt) = -1/2 (Δ[HAuCl4·xH2O])/(Δt) = 1/2 (Δ[HCl])/(Δt) = 1/2 (Δ[Au])/(Δt) = 1/3 (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| stannous chloride | gold(III) chloride hydrate | hydrogen chloride | gold | stannic chloride formula | SnCl_2 | HAuCl_4·xH_2O | HCl | Au | SnCl_4 Hill formula | Cl_2Sn | AuCl_4H | ClH | Au | Cl_4Sn name | stannous chloride | gold(III) chloride hydrate | hydrogen chloride | gold | stannic chloride IUPAC name | dichlorotin | hydron; tetrachlorogold | hydrogen chloride | gold | tetrachlorostannane
Substance properties
| stannous chloride | gold(III) chloride hydrate | hydrogen chloride | gold | stannic chloride molar mass | 189.6 g/mol | 339.8 g/mol | 36.46 g/mol | 196.966569 g/mol | 260.5 g/mol phase | solid (at STP) | | gas (at STP) | solid (at STP) | liquid (at STP) melting point | 246 °C | | -114.17 °C | 1063 °C | -33 °C boiling point | 652 °C | | -85 °C | 2856 °C | 114 °C density | 3.354 g/cm^3 | 3.9 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 19.3 g/cm^3 | 2.226 g/cm^3 solubility in water | | | miscible | insoluble | soluble dynamic viscosity | 7 Pa s (at 25 °C) | | | | 5.8×10^-4 Pa s (at 60 °C) odor | odorless | | | |
Units
