Search

H2SO4 + HCl + SnCl2 = H2O + H2S + SnCl4

Input interpretation

H_2SO_4 sulfuric acid + HCl hydrogen chloride + SnCl_2 stannous chloride ⟶ H_2O water + H_2S hydrogen sulfide + SnCl_4 stannic chloride
H_2SO_4 sulfuric acid + HCl hydrogen chloride + SnCl_2 stannous chloride ⟶ H_2O water + H_2S hydrogen sulfide + SnCl_4 stannic chloride

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + HCl + SnCl_2 ⟶ H_2O + H_2S + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HCl + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 H_2S + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cl and Sn: H: | 2 c_1 + c_2 = 2 c_4 + 2 c_5 O: | 4 c_1 = c_4 S: | c_1 = c_5 Cl: | c_2 + 2 c_3 = 4 c_6 Sn: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 8 c_3 = 4 c_4 = 4 c_5 = 1 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 8 HCl + 4 SnCl_2 ⟶ 4 H_2O + H_2S + 4 SnCl_4
Balance the chemical equation algebraically: H_2SO_4 + HCl + SnCl_2 ⟶ H_2O + H_2S + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 HCl + c_3 SnCl_2 ⟶ c_4 H_2O + c_5 H_2S + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Cl and Sn: H: | 2 c_1 + c_2 = 2 c_4 + 2 c_5 O: | 4 c_1 = c_4 S: | c_1 = c_5 Cl: | c_2 + 2 c_3 = 4 c_6 Sn: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 8 c_3 = 4 c_4 = 4 c_5 = 1 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + 8 HCl + 4 SnCl_2 ⟶ 4 H_2O + H_2S + 4 SnCl_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

sulfuric acid + hydrogen chloride + stannous chloride ⟶ water + hydrogen sulfide + stannic chloride
sulfuric acid + hydrogen chloride + stannous chloride ⟶ water + hydrogen sulfide + stannic chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + HCl + SnCl_2 ⟶ H_2O + H_2S + 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: H_2SO_4 + 8 HCl + 4 SnCl_2 ⟶ 4 H_2O + H_2S + 4 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 H_2SO_4 | 1 | -1 HCl | 8 | -8 SnCl_2 | 4 | -4 H_2O | 4 | 4 H_2S | 1 | 1 SnCl_4 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) HCl | 8 | -8 | ([HCl])^(-8) SnCl_2 | 4 | -4 | ([SnCl2])^(-4) H_2O | 4 | 4 | ([H2O])^4 H_2S | 1 | 1 | [H2S] SnCl_4 | 4 | 4 | ([SnCl4])^4 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 = ([H2SO4])^(-1) ([HCl])^(-8) ([SnCl2])^(-4) ([H2O])^4 [H2S] ([SnCl4])^4 = (([H2O])^4 [H2S] ([SnCl4])^4)/([H2SO4] ([HCl])^8 ([SnCl2])^4)
Construct the equilibrium constant, K, expression for: H_2SO_4 + HCl + SnCl_2 ⟶ H_2O + H_2S + 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: H_2SO_4 + 8 HCl + 4 SnCl_2 ⟶ 4 H_2O + H_2S + 4 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 H_2SO_4 | 1 | -1 HCl | 8 | -8 SnCl_2 | 4 | -4 H_2O | 4 | 4 H_2S | 1 | 1 SnCl_4 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) HCl | 8 | -8 | ([HCl])^(-8) SnCl_2 | 4 | -4 | ([SnCl2])^(-4) H_2O | 4 | 4 | ([H2O])^4 H_2S | 1 | 1 | [H2S] SnCl_4 | 4 | 4 | ([SnCl4])^4 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 = ([H2SO4])^(-1) ([HCl])^(-8) ([SnCl2])^(-4) ([H2O])^4 [H2S] ([SnCl4])^4 = (([H2O])^4 [H2S] ([SnCl4])^4)/([H2SO4] ([HCl])^8 ([SnCl2])^4)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + HCl + SnCl_2 ⟶ H_2O + H_2S + 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: H_2SO_4 + 8 HCl + 4 SnCl_2 ⟶ 4 H_2O + H_2S + 4 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 H_2SO_4 | 1 | -1 HCl | 8 | -8 SnCl_2 | 4 | -4 H_2O | 4 | 4 H_2S | 1 | 1 SnCl_4 | 4 | 4 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) HCl | 8 | -8 | -1/8 (Δ[HCl])/(Δt) SnCl_2 | 4 | -4 | -1/4 (Δ[SnCl2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) SnCl_4 | 4 | 4 | 1/4 (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 = -(Δ[H2SO4])/(Δt) = -1/8 (Δ[HCl])/(Δt) = -1/4 (Δ[SnCl2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[H2S])/(Δt) = 1/4 (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + HCl + SnCl_2 ⟶ H_2O + H_2S + 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: H_2SO_4 + 8 HCl + 4 SnCl_2 ⟶ 4 H_2O + H_2S + 4 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 H_2SO_4 | 1 | -1 HCl | 8 | -8 SnCl_2 | 4 | -4 H_2O | 4 | 4 H_2S | 1 | 1 SnCl_4 | 4 | 4 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) HCl | 8 | -8 | -1/8 (Δ[HCl])/(Δt) SnCl_2 | 4 | -4 | -1/4 (Δ[SnCl2])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) SnCl_4 | 4 | 4 | 1/4 (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 = -(Δ[H2SO4])/(Δt) = -1/8 (Δ[HCl])/(Δt) = -1/4 (Δ[SnCl2])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[H2S])/(Δt) = 1/4 (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | hydrogen chloride | stannous chloride | water | hydrogen sulfide | stannic chloride formula | H_2SO_4 | HCl | SnCl_2 | H_2O | H_2S | SnCl_4 Hill formula | H_2O_4S | ClH | Cl_2Sn | H_2O | H_2S | Cl_4Sn name | sulfuric acid | hydrogen chloride | stannous chloride | water | hydrogen sulfide | stannic chloride IUPAC name | sulfuric acid | hydrogen chloride | dichlorotin | water | hydrogen sulfide | tetrachlorostannane
| sulfuric acid | hydrogen chloride | stannous chloride | water | hydrogen sulfide | stannic chloride formula | H_2SO_4 | HCl | SnCl_2 | H_2O | H_2S | SnCl_4 Hill formula | H_2O_4S | ClH | Cl_2Sn | H_2O | H_2S | Cl_4Sn name | sulfuric acid | hydrogen chloride | stannous chloride | water | hydrogen sulfide | stannic chloride IUPAC name | sulfuric acid | hydrogen chloride | dichlorotin | water | hydrogen sulfide | tetrachlorostannane

Random Queries

DOT numbers of potassium nitrite vs sodium amide
melting point of ethylene glycol vs N-pentane
ions of copper(I) cyanide-13C,15N
magnesium nitrate
melting point of diborane vs 1-chloro-1-fluoroethylene
alternate names of palladium(III) cation
width of Al-36
specific gravities of Brønsted-Lowry bases
density of xenon pentafluoride hexafluororuthenate
chemical types of zinc formate dihydrate vs lithium bromide hydrate