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H2O + S + Br2 = H2SO4 + HBr

Input interpretation

H_2O water + S mixed sulfur + Br_2 bromine ⟶ H_2SO_4 sulfuric acid + HBr hydrogen bromide
H_2O water + S mixed sulfur + Br_2 bromine ⟶ H_2SO_4 sulfuric acid + HBr hydrogen bromide

Balanced equation

Balance the chemical equation algebraically: H_2O + S + Br_2 ⟶ H_2SO_4 + HBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 S + c_3 Br_2 ⟶ c_4 H_2SO_4 + c_5 HBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Br: H: | 2 c_1 = 2 c_4 + c_5 O: | c_1 = 4 c_4 S: | c_2 = c_4 Br: | 2 c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 3 c_4 = 1 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + S + 3 Br_2 ⟶ H_2SO_4 + 6 HBr
Balance the chemical equation algebraically: H_2O + S + Br_2 ⟶ H_2SO_4 + HBr Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 S + c_3 Br_2 ⟶ c_4 H_2SO_4 + c_5 HBr Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Br: H: | 2 c_1 = 2 c_4 + c_5 O: | c_1 = 4 c_4 S: | c_2 = c_4 Br: | 2 c_3 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 3 c_4 = 1 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + S + 3 Br_2 ⟶ H_2SO_4 + 6 HBr

Structures

+ + ⟶ +
+ + ⟶ +

Names

water + mixed sulfur + bromine ⟶ sulfuric acid + hydrogen bromide
water + mixed sulfur + bromine ⟶ sulfuric acid + hydrogen bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + S + Br_2 ⟶ H_2SO_4 + HBr 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: 4 H_2O + S + 3 Br_2 ⟶ H_2SO_4 + 6 HBr 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_2O | 4 | -4 S | 1 | -1 Br_2 | 3 | -3 H_2SO_4 | 1 | 1 HBr | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) S | 1 | -1 | ([S])^(-1) Br_2 | 3 | -3 | ([Br2])^(-3) H_2SO_4 | 1 | 1 | [H2SO4] HBr | 6 | 6 | ([HBr])^6 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 = ([H2O])^(-4) ([S])^(-1) ([Br2])^(-3) [H2SO4] ([HBr])^6 = ([H2SO4] ([HBr])^6)/(([H2O])^4 [S] ([Br2])^3)
Construct the equilibrium constant, K, expression for: H_2O + S + Br_2 ⟶ H_2SO_4 + HBr 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: 4 H_2O + S + 3 Br_2 ⟶ H_2SO_4 + 6 HBr 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_2O | 4 | -4 S | 1 | -1 Br_2 | 3 | -3 H_2SO_4 | 1 | 1 HBr | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) S | 1 | -1 | ([S])^(-1) Br_2 | 3 | -3 | ([Br2])^(-3) H_2SO_4 | 1 | 1 | [H2SO4] HBr | 6 | 6 | ([HBr])^6 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 = ([H2O])^(-4) ([S])^(-1) ([Br2])^(-3) [H2SO4] ([HBr])^6 = ([H2SO4] ([HBr])^6)/(([H2O])^4 [S] ([Br2])^3)

Rate of reaction

Construct the rate of reaction expression for: H_2O + S + Br_2 ⟶ H_2SO_4 + HBr 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: 4 H_2O + S + 3 Br_2 ⟶ H_2SO_4 + 6 HBr 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_2O | 4 | -4 S | 1 | -1 Br_2 | 3 | -3 H_2SO_4 | 1 | 1 HBr | 6 | 6 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_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) S | 1 | -1 | -(Δ[S])/(Δt) Br_2 | 3 | -3 | -1/3 (Δ[Br2])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) HBr | 6 | 6 | 1/6 (Δ[HBr])/(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 = -1/4 (Δ[H2O])/(Δt) = -(Δ[S])/(Δt) = -1/3 (Δ[Br2])/(Δt) = (Δ[H2SO4])/(Δt) = 1/6 (Δ[HBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + S + Br_2 ⟶ H_2SO_4 + HBr 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: 4 H_2O + S + 3 Br_2 ⟶ H_2SO_4 + 6 HBr 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_2O | 4 | -4 S | 1 | -1 Br_2 | 3 | -3 H_2SO_4 | 1 | 1 HBr | 6 | 6 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_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) S | 1 | -1 | -(Δ[S])/(Δt) Br_2 | 3 | -3 | -1/3 (Δ[Br2])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) HBr | 6 | 6 | 1/6 (Δ[HBr])/(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 = -1/4 (Δ[H2O])/(Δt) = -(Δ[S])/(Δt) = -1/3 (Δ[Br2])/(Δt) = (Δ[H2SO4])/(Δt) = 1/6 (Δ[HBr])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | mixed sulfur | bromine | sulfuric acid | hydrogen bromide formula | H_2O | S | Br_2 | H_2SO_4 | HBr Hill formula | H_2O | S | Br_2 | H_2O_4S | BrH name | water | mixed sulfur | bromine | sulfuric acid | hydrogen bromide IUPAC name | water | sulfur | molecular bromine | sulfuric acid | hydrogen bromide
| water | mixed sulfur | bromine | sulfuric acid | hydrogen bromide formula | H_2O | S | Br_2 | H_2SO_4 | HBr Hill formula | H_2O | S | Br_2 | H_2O_4S | BrH name | water | mixed sulfur | bromine | sulfuric acid | hydrogen bromide IUPAC name | water | sulfur | molecular bromine | sulfuric acid | hydrogen bromide

Substance properties

| water | mixed sulfur | bromine | sulfuric acid | hydrogen bromide molar mass | 18.015 g/mol | 32.06 g/mol | 159.81 g/mol | 98.07 g/mol | 80.912 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) melting point | 0 °C | 112.8 °C | -7.2 °C | 10.371 °C | -86.8 °C boiling point | 99.9839 °C | 444.7 °C | 58.8 °C | 279.6 °C | -66.38 °C density | 1 g/cm^3 | 2.07 g/cm^3 | 3.119 g/cm^3 | 1.8305 g/cm^3 | 0.003307 g/cm^3 (at 25 °C) solubility in water | | | insoluble | very soluble | miscible surface tension | 0.0728 N/m | | 0.0409 N/m | 0.0735 N/m | 0.0271 N/m dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 9.44×10^-4 Pa s (at 25 °C) | 0.021 Pa s (at 25 °C) | 8.4×10^-4 Pa s (at -75 °C) odor | odorless | | | odorless |
| water | mixed sulfur | bromine | sulfuric acid | hydrogen bromide molar mass | 18.015 g/mol | 32.06 g/mol | 159.81 g/mol | 98.07 g/mol | 80.912 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | gas (at STP) melting point | 0 °C | 112.8 °C | -7.2 °C | 10.371 °C | -86.8 °C boiling point | 99.9839 °C | 444.7 °C | 58.8 °C | 279.6 °C | -66.38 °C density | 1 g/cm^3 | 2.07 g/cm^3 | 3.119 g/cm^3 | 1.8305 g/cm^3 | 0.003307 g/cm^3 (at 25 °C) solubility in water | | | insoluble | very soluble | miscible surface tension | 0.0728 N/m | | 0.0409 N/m | 0.0735 N/m | 0.0271 N/m dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 9.44×10^-4 Pa s (at 25 °C) | 0.021 Pa s (at 25 °C) | 8.4×10^-4 Pa s (at -75 °C) odor | odorless | | | odorless |

Units

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