Input interpretation
![SnCl_2 stannous chloride + H2Hg(Cl)4 ⟶ HCl hydrogen chloride + SnCl_4 stannic chloride + Hg_2Cl_2 mercury(I) chloride](../image_source/9b8848bd206e50831a5d94076107f387.png)
SnCl_2 stannous chloride + H2Hg(Cl)4 ⟶ HCl hydrogen chloride + SnCl_4 stannic chloride + Hg_2Cl_2 mercury(I) chloride
Balanced equation
![Balance the chemical equation algebraically: SnCl_2 + H2Hg(Cl)4 ⟶ HCl + SnCl_4 + Hg_2Cl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnCl_2 + c_2 H2Hg(Cl)4 ⟶ c_3 HCl + c_4 SnCl_4 + c_5 Hg_2Cl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Sn, H and Hg: Cl: | 2 c_1 + 4 c_2 = c_3 + 4 c_4 + 2 c_5 Sn: | c_1 = c_4 H: | 2 c_2 = c_3 Hg: | c_2 = 2 c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SnCl_2 + 2 H2Hg(Cl)4 ⟶ 4 HCl + SnCl_4 + Hg_2Cl_2](../image_source/c3b2e1e5dfb336eea584fb265ee4acb1.png)
Balance the chemical equation algebraically: SnCl_2 + H2Hg(Cl)4 ⟶ HCl + SnCl_4 + Hg_2Cl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 SnCl_2 + c_2 H2Hg(Cl)4 ⟶ c_3 HCl + c_4 SnCl_4 + c_5 Hg_2Cl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Sn, H and Hg: Cl: | 2 c_1 + 4 c_2 = c_3 + 4 c_4 + 2 c_5 Sn: | c_1 = c_4 H: | 2 c_2 = c_3 Hg: | c_2 = 2 c_5 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 4 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | SnCl_2 + 2 H2Hg(Cl)4 ⟶ 4 HCl + SnCl_4 + Hg_2Cl_2
Structures
![+ H2Hg(Cl)4 ⟶ + +](../image_source/2ba25931371b98e8601f9e2bd67880b4.png)
+ H2Hg(Cl)4 ⟶ + +
Names
![stannous chloride + H2Hg(Cl)4 ⟶ hydrogen chloride + stannic chloride + mercury(I) chloride](../image_source/82e3829d820aedd82932f07f62d19fd4.png)
stannous chloride + H2Hg(Cl)4 ⟶ hydrogen chloride + stannic chloride + mercury(I) chloride
Equilibrium constant
![Construct the equilibrium constant, K, expression for: SnCl_2 + H2Hg(Cl)4 ⟶ HCl + SnCl_4 + Hg_2Cl_2 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: SnCl_2 + 2 H2Hg(Cl)4 ⟶ 4 HCl + SnCl_4 + Hg_2Cl_2 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 | 1 | -1 H2Hg(Cl)4 | 2 | -2 HCl | 4 | 4 SnCl_4 | 1 | 1 Hg_2Cl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnCl_2 | 1 | -1 | ([SnCl2])^(-1) H2Hg(Cl)4 | 2 | -2 | ([H2Hg(Cl)4])^(-2) HCl | 4 | 4 | ([HCl])^4 SnCl_4 | 1 | 1 | [SnCl4] Hg_2Cl_2 | 1 | 1 | [Hg2Cl2] 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])^(-1) ([H2Hg(Cl)4])^(-2) ([HCl])^4 [SnCl4] [Hg2Cl2] = (([HCl])^4 [SnCl4] [Hg2Cl2])/([SnCl2] ([H2Hg(Cl)4])^2)](../image_source/2d00d35a30c8dedddcd3e8341ee0a0ec.png)
Construct the equilibrium constant, K, expression for: SnCl_2 + H2Hg(Cl)4 ⟶ HCl + SnCl_4 + Hg_2Cl_2 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: SnCl_2 + 2 H2Hg(Cl)4 ⟶ 4 HCl + SnCl_4 + Hg_2Cl_2 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 | 1 | -1 H2Hg(Cl)4 | 2 | -2 HCl | 4 | 4 SnCl_4 | 1 | 1 Hg_2Cl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression SnCl_2 | 1 | -1 | ([SnCl2])^(-1) H2Hg(Cl)4 | 2 | -2 | ([H2Hg(Cl)4])^(-2) HCl | 4 | 4 | ([HCl])^4 SnCl_4 | 1 | 1 | [SnCl4] Hg_2Cl_2 | 1 | 1 | [Hg2Cl2] 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])^(-1) ([H2Hg(Cl)4])^(-2) ([HCl])^4 [SnCl4] [Hg2Cl2] = (([HCl])^4 [SnCl4] [Hg2Cl2])/([SnCl2] ([H2Hg(Cl)4])^2)
Rate of reaction
![Construct the rate of reaction expression for: SnCl_2 + H2Hg(Cl)4 ⟶ HCl + SnCl_4 + Hg_2Cl_2 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: SnCl_2 + 2 H2Hg(Cl)4 ⟶ 4 HCl + SnCl_4 + Hg_2Cl_2 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 | 1 | -1 H2Hg(Cl)4 | 2 | -2 HCl | 4 | 4 SnCl_4 | 1 | 1 Hg_2Cl_2 | 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 SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) H2Hg(Cl)4 | 2 | -2 | -1/2 (Δ[H2Hg(Cl)4])/(Δt) HCl | 4 | 4 | 1/4 (Δ[HCl])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(Δt) Hg_2Cl_2 | 1 | 1 | (Δ[Hg2Cl2])/(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 = -(Δ[SnCl2])/(Δt) = -1/2 (Δ[H2Hg(Cl)4])/(Δt) = 1/4 (Δ[HCl])/(Δt) = (Δ[SnCl4])/(Δt) = (Δ[Hg2Cl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/35b74f92a18ece1e9c441fd64f9dd97e.png)
Construct the rate of reaction expression for: SnCl_2 + H2Hg(Cl)4 ⟶ HCl + SnCl_4 + Hg_2Cl_2 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: SnCl_2 + 2 H2Hg(Cl)4 ⟶ 4 HCl + SnCl_4 + Hg_2Cl_2 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 | 1 | -1 H2Hg(Cl)4 | 2 | -2 HCl | 4 | 4 SnCl_4 | 1 | 1 Hg_2Cl_2 | 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 SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) H2Hg(Cl)4 | 2 | -2 | -1/2 (Δ[H2Hg(Cl)4])/(Δt) HCl | 4 | 4 | 1/4 (Δ[HCl])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(Δt) Hg_2Cl_2 | 1 | 1 | (Δ[Hg2Cl2])/(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 = -(Δ[SnCl2])/(Δt) = -1/2 (Δ[H2Hg(Cl)4])/(Δt) = 1/4 (Δ[HCl])/(Δt) = (Δ[SnCl4])/(Δt) = (Δ[Hg2Cl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| stannous chloride | H2Hg(Cl)4 | hydrogen chloride | stannic chloride | mercury(I) chloride formula | SnCl_2 | H2Hg(Cl)4 | HCl | SnCl_4 | Hg_2Cl_2 Hill formula | Cl_2Sn | H2Cl4Hg | ClH | Cl_4Sn | Cl_2Hg_2 name | stannous chloride | | hydrogen chloride | stannic chloride | mercury(I) chloride IUPAC name | dichlorotin | | hydrogen chloride | tetrachlorostannane | chloromercury](../image_source/0648a0987c8bb4fdc143886a157265de.png)
| stannous chloride | H2Hg(Cl)4 | hydrogen chloride | stannic chloride | mercury(I) chloride formula | SnCl_2 | H2Hg(Cl)4 | HCl | SnCl_4 | Hg_2Cl_2 Hill formula | Cl_2Sn | H2Cl4Hg | ClH | Cl_4Sn | Cl_2Hg_2 name | stannous chloride | | hydrogen chloride | stannic chloride | mercury(I) chloride IUPAC name | dichlorotin | | hydrogen chloride | tetrachlorostannane | chloromercury
Substance properties
![| stannous chloride | H2Hg(Cl)4 | hydrogen chloride | stannic chloride | mercury(I) chloride molar mass | 189.6 g/mol | 344.4 g/mol | 36.46 g/mol | 260.5 g/mol | 472.08 g/mol phase | solid (at STP) | | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 246 °C | | -114.17 °C | -33 °C | 525 °C boiling point | 652 °C | | -85 °C | 114 °C | 383 °C density | 3.354 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 2.226 g/cm^3 | 7.16 g/cm^3 solubility in water | | | miscible | soluble | insoluble dynamic viscosity | 7 Pa s (at 25 °C) | | | 5.8×10^-4 Pa s (at 60 °C) | odor | odorless | | | |](../image_source/31816a5ce6320709acb9ef6ae0a5b92d.png)
| stannous chloride | H2Hg(Cl)4 | hydrogen chloride | stannic chloride | mercury(I) chloride molar mass | 189.6 g/mol | 344.4 g/mol | 36.46 g/mol | 260.5 g/mol | 472.08 g/mol phase | solid (at STP) | | gas (at STP) | liquid (at STP) | solid (at STP) melting point | 246 °C | | -114.17 °C | -33 °C | 525 °C boiling point | 652 °C | | -85 °C | 114 °C | 383 °C density | 3.354 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 2.226 g/cm^3 | 7.16 g/cm^3 solubility in water | | | miscible | soluble | insoluble dynamic viscosity | 7 Pa s (at 25 °C) | | | 5.8×10^-4 Pa s (at 60 °C) | odor | odorless | | | |
Units