Search

SnCl2 + H2[Hg(Cl)4] = HCl + SnCl4 + Hg2Cl2

Input interpretation

SnCl_2 stannous chloride + H2Hg(Cl)4 ⟶ HCl hydrogen chloride + SnCl_4 stannic chloride + Hg_2Cl_2 mercury(I) chloride
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
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 ⟶ + +
+ H2Hg(Cl)4 ⟶ + +

Names

stannous chloride + H2Hg(Cl)4 ⟶ hydrogen chloride + stannic chloride + mercury(I) chloride
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)
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)
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
| 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 | | | |
| 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

Random Queries

find features image rokühnite
atomic radius of chlorine vs neon
molar mass of oxygen difluoride vs 1-buten-3-yne
chemical types of potassium butyltrifluoroborate vs bis(dibutylchlorotin(IV))oxide
atomic diameter of rubidium
CAS number of sodium bromate vs cobalt
Hill formula of hydrogen chloride vs picric acid
density of cobalt trifluoride vs 3,5-bis(trifluoromethyl)benzenamine
AgNO3 + Cl
formula of dichlorodifluorosilane vs zinc barate