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HCl + (NH4)2S = H2S + NH4Cl

Input interpretation

HCl hydrogen chloride + (NH_4)_2S diammonium sulfide ⟶ H_2S hydrogen sulfide + NH_4Cl ammonium chloride
HCl hydrogen chloride + (NH_4)_2S diammonium sulfide ⟶ H_2S hydrogen sulfide + NH_4Cl ammonium chloride

Balanced equation

Balance the chemical equation algebraically: HCl + (NH_4)_2S ⟶ H_2S + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 (NH_4)_2S ⟶ c_3 H_2S + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and S: Cl: | c_1 = c_4 H: | c_1 + 8 c_2 = 2 c_3 + 4 c_4 N: | 2 c_2 = c_4 S: | 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 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + (NH_4)_2S ⟶ H_2S + 2 NH_4Cl
Balance the chemical equation algebraically: HCl + (NH_4)_2S ⟶ H_2S + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 (NH_4)_2S ⟶ c_3 H_2S + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and S: Cl: | c_1 = c_4 H: | c_1 + 8 c_2 = 2 c_3 + 4 c_4 N: | 2 c_2 = c_4 S: | 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 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + (NH_4)_2S ⟶ H_2S + 2 NH_4Cl

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen chloride + diammonium sulfide ⟶ hydrogen sulfide + ammonium chloride
hydrogen chloride + diammonium sulfide ⟶ hydrogen sulfide + ammonium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + (NH_4)_2S ⟶ H_2S + NH_4Cl 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: 2 HCl + (NH_4)_2S ⟶ H_2S + 2 NH_4Cl 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 | 2 | -2 (NH_4)_2S | 1 | -1 H_2S | 1 | 1 NH_4Cl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) (NH_4)_2S | 1 | -1 | ([(NH4)2S])^(-1) H_2S | 1 | 1 | [H2S] NH_4Cl | 2 | 2 | ([NH4Cl])^2 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])^(-2) ([(NH4)2S])^(-1) [H2S] ([NH4Cl])^2 = ([H2S] ([NH4Cl])^2)/(([HCl])^2 [(NH4)2S])
Construct the equilibrium constant, K, expression for: HCl + (NH_4)_2S ⟶ H_2S + NH_4Cl 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: 2 HCl + (NH_4)_2S ⟶ H_2S + 2 NH_4Cl 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 | 2 | -2 (NH_4)_2S | 1 | -1 H_2S | 1 | 1 NH_4Cl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) (NH_4)_2S | 1 | -1 | ([(NH4)2S])^(-1) H_2S | 1 | 1 | [H2S] NH_4Cl | 2 | 2 | ([NH4Cl])^2 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])^(-2) ([(NH4)2S])^(-1) [H2S] ([NH4Cl])^2 = ([H2S] ([NH4Cl])^2)/(([HCl])^2 [(NH4)2S])

Rate of reaction

Construct the rate of reaction expression for: HCl + (NH_4)_2S ⟶ H_2S + NH_4Cl 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: 2 HCl + (NH_4)_2S ⟶ H_2S + 2 NH_4Cl 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 | 2 | -2 (NH_4)_2S | 1 | -1 H_2S | 1 | 1 NH_4Cl | 2 | 2 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) (NH_4)_2S | 1 | -1 | -(Δ[(NH4)2S])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) NH_4Cl | 2 | 2 | 1/2 (Δ[NH4Cl])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[(NH4)2S])/(Δt) = (Δ[H2S])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + (NH_4)_2S ⟶ H_2S + NH_4Cl 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: 2 HCl + (NH_4)_2S ⟶ H_2S + 2 NH_4Cl 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 | 2 | -2 (NH_4)_2S | 1 | -1 H_2S | 1 | 1 NH_4Cl | 2 | 2 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 | 2 | -2 | -1/2 (Δ[HCl])/(Δt) (NH_4)_2S | 1 | -1 | -(Δ[(NH4)2S])/(Δt) H_2S | 1 | 1 | (Δ[H2S])/(Δt) NH_4Cl | 2 | 2 | 1/2 (Δ[NH4Cl])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[(NH4)2S])/(Δt) = (Δ[H2S])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | diammonium sulfide | hydrogen sulfide | ammonium chloride formula | HCl | (NH_4)_2S | H_2S | NH_4Cl Hill formula | ClH | H_8N_2S | H_2S | ClH_4N name | hydrogen chloride | diammonium sulfide | hydrogen sulfide | ammonium chloride
| hydrogen chloride | diammonium sulfide | hydrogen sulfide | ammonium chloride formula | HCl | (NH_4)_2S | H_2S | NH_4Cl Hill formula | ClH | H_8N_2S | H_2S | ClH_4N name | hydrogen chloride | diammonium sulfide | hydrogen sulfide | ammonium chloride

Substance properties

| hydrogen chloride | diammonium sulfide | hydrogen sulfide | ammonium chloride molar mass | 36.46 g/mol | 68.14 g/mol | 34.08 g/mol | 53.49 g/mol phase | gas (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | -18 °C | -85 °C | 340 °C boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | 0.997 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 1.5256 g/cm^3 solubility in water | miscible | very soluble | | soluble dynamic viscosity | | | 1.239×10^-5 Pa s (at 25 °C) |
| hydrogen chloride | diammonium sulfide | hydrogen sulfide | ammonium chloride molar mass | 36.46 g/mol | 68.14 g/mol | 34.08 g/mol | 53.49 g/mol phase | gas (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | -18 °C | -85 °C | 340 °C boiling point | -85 °C | | -60 °C | density | 0.00149 g/cm^3 (at 25 °C) | 0.997 g/cm^3 | 0.001393 g/cm^3 (at 25 °C) | 1.5256 g/cm^3 solubility in water | miscible | very soluble | | soluble dynamic viscosity | | | 1.239×10^-5 Pa s (at 25 °C) |

Units

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