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H2SO4 + CaBr2 = H2O + SO2 + Br2 + CaSO4

Input interpretation

H_2SO_4 sulfuric acid + CaBr_2 calcium bromide ⟶ H_2O water + SO_2 sulfur dioxide + Br_2 bromine + CaSO_4 calcium sulfate
H_2SO_4 sulfuric acid + CaBr_2 calcium bromide ⟶ H_2O water + SO_2 sulfur dioxide + Br_2 bromine + CaSO_4 calcium sulfate

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + CaBr_2 ⟶ H_2O + SO_2 + Br_2 + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CaBr_2 ⟶ c_3 H_2O + c_4 SO_2 + c_5 Br_2 + c_6 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Br and Ca: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 2 c_4 + 4 c_6 S: | c_1 = c_4 + c_6 Br: | 2 c_2 = 2 c_5 Ca: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + CaBr_2 ⟶ 2 H_2O + SO_2 + Br_2 + CaSO_4
Balance the chemical equation algebraically: H_2SO_4 + CaBr_2 ⟶ H_2O + SO_2 + Br_2 + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CaBr_2 ⟶ c_3 H_2O + c_4 SO_2 + c_5 Br_2 + c_6 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Br and Ca: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 2 c_4 + 4 c_6 S: | c_1 = c_4 + c_6 Br: | 2 c_2 = 2 c_5 Ca: | c_2 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 c_5 = 1 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2SO_4 + CaBr_2 ⟶ 2 H_2O + SO_2 + Br_2 + CaSO_4

Structures

+ ⟶ + + +
+ ⟶ + + +

Names

sulfuric acid + calcium bromide ⟶ water + sulfur dioxide + bromine + calcium sulfate
sulfuric acid + calcium bromide ⟶ water + sulfur dioxide + bromine + calcium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + CaBr_2 ⟶ H_2O + SO_2 + Br_2 + CaSO_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: 2 H_2SO_4 + CaBr_2 ⟶ 2 H_2O + SO_2 + Br_2 + CaSO_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 | 2 | -2 CaBr_2 | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Br_2 | 1 | 1 CaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) CaBr_2 | 1 | -1 | ([CaBr2])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] Br_2 | 1 | 1 | [Br2] CaSO_4 | 1 | 1 | [CaSO4] 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])^(-2) ([CaBr2])^(-1) ([H2O])^2 [SO2] [Br2] [CaSO4] = (([H2O])^2 [SO2] [Br2] [CaSO4])/(([H2SO4])^2 [CaBr2])
Construct the equilibrium constant, K, expression for: H_2SO_4 + CaBr_2 ⟶ H_2O + SO_2 + Br_2 + CaSO_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: 2 H_2SO_4 + CaBr_2 ⟶ 2 H_2O + SO_2 + Br_2 + CaSO_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 | 2 | -2 CaBr_2 | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Br_2 | 1 | 1 CaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 2 | -2 | ([H2SO4])^(-2) CaBr_2 | 1 | -1 | ([CaBr2])^(-1) H_2O | 2 | 2 | ([H2O])^2 SO_2 | 1 | 1 | [SO2] Br_2 | 1 | 1 | [Br2] CaSO_4 | 1 | 1 | [CaSO4] 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])^(-2) ([CaBr2])^(-1) ([H2O])^2 [SO2] [Br2] [CaSO4] = (([H2O])^2 [SO2] [Br2] [CaSO4])/(([H2SO4])^2 [CaBr2])

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + CaBr_2 ⟶ H_2O + SO_2 + Br_2 + CaSO_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: 2 H_2SO_4 + CaBr_2 ⟶ 2 H_2O + SO_2 + Br_2 + CaSO_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 | 2 | -2 CaBr_2 | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Br_2 | 1 | 1 CaSO_4 | 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 H_2SO_4 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) CaBr_2 | 1 | -1 | -(Δ[CaBr2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) Br_2 | 1 | 1 | (Δ[Br2])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[H2SO4])/(Δt) = -(Δ[CaBr2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[Br2])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + CaBr_2 ⟶ H_2O + SO_2 + Br_2 + CaSO_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: 2 H_2SO_4 + CaBr_2 ⟶ 2 H_2O + SO_2 + Br_2 + CaSO_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 | 2 | -2 CaBr_2 | 1 | -1 H_2O | 2 | 2 SO_2 | 1 | 1 Br_2 | 1 | 1 CaSO_4 | 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 H_2SO_4 | 2 | -2 | -1/2 (Δ[H2SO4])/(Δt) CaBr_2 | 1 | -1 | -(Δ[CaBr2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) SO_2 | 1 | 1 | (Δ[SO2])/(Δt) Br_2 | 1 | 1 | (Δ[Br2])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[H2SO4])/(Δt) = -(Δ[CaBr2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[SO2])/(Δt) = (Δ[Br2])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | calcium bromide | water | sulfur dioxide | bromine | calcium sulfate formula | H_2SO_4 | CaBr_2 | H_2O | SO_2 | Br_2 | CaSO_4 Hill formula | H_2O_4S | Br_2Ca | H_2O | O_2S | Br_2 | CaO_4S name | sulfuric acid | calcium bromide | water | sulfur dioxide | bromine | calcium sulfate IUPAC name | sulfuric acid | calcium dibromide | water | sulfur dioxide | molecular bromine | calcium sulfate
| sulfuric acid | calcium bromide | water | sulfur dioxide | bromine | calcium sulfate formula | H_2SO_4 | CaBr_2 | H_2O | SO_2 | Br_2 | CaSO_4 Hill formula | H_2O_4S | Br_2Ca | H_2O | O_2S | Br_2 | CaO_4S name | sulfuric acid | calcium bromide | water | sulfur dioxide | bromine | calcium sulfate IUPAC name | sulfuric acid | calcium dibromide | water | sulfur dioxide | molecular bromine | calcium sulfate

Substance properties

| sulfuric acid | calcium bromide | water | sulfur dioxide | bromine | calcium sulfate molar mass | 98.07 g/mol | 199.89 g/mol | 18.015 g/mol | 64.06 g/mol | 159.81 g/mol | 136.13 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | liquid (at STP) | melting point | 10.371 °C | 730 °C | 0 °C | -73 °C | -7.2 °C | boiling point | 279.6 °C | 810 °C | 99.9839 °C | -10 °C | 58.8 °C | density | 1.8305 g/cm^3 | 3.353 g/cm^3 | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 3.119 g/cm^3 | solubility in water | very soluble | soluble | | | insoluble | slightly soluble surface tension | 0.0735 N/m | | 0.0728 N/m | 0.02859 N/m | 0.0409 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | 9.44×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless | | | odorless
| sulfuric acid | calcium bromide | water | sulfur dioxide | bromine | calcium sulfate molar mass | 98.07 g/mol | 199.89 g/mol | 18.015 g/mol | 64.06 g/mol | 159.81 g/mol | 136.13 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | liquid (at STP) | melting point | 10.371 °C | 730 °C | 0 °C | -73 °C | -7.2 °C | boiling point | 279.6 °C | 810 °C | 99.9839 °C | -10 °C | 58.8 °C | density | 1.8305 g/cm^3 | 3.353 g/cm^3 | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | 3.119 g/cm^3 | solubility in water | very soluble | soluble | | | insoluble | slightly soluble surface tension | 0.0735 N/m | | 0.0728 N/m | 0.02859 N/m | 0.0409 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | 9.44×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless | | | odorless

Units

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