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HBr + Zn(OH)2 = H2O + ZnBr2

Input interpretation

HBr hydrogen bromide + Zn(OH)_2 zinc hydroxide ⟶ H_2O water + ZnBr_2 zinc bromide
HBr hydrogen bromide + Zn(OH)_2 zinc hydroxide ⟶ H_2O water + ZnBr_2 zinc bromide

Balanced equation

Balance the chemical equation algebraically: HBr + Zn(OH)_2 ⟶ H_2O + ZnBr_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HBr + c_2 Zn(OH)_2 ⟶ c_3 H_2O + c_4 ZnBr_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Br, H, O and Zn: Br: | c_1 = 2 c_4 H: | c_1 + 2 c_2 = 2 c_3 O: | 2 c_2 = c_3 Zn: | c_2 = c_4 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HBr + Zn(OH)_2 ⟶ 2 H_2O + ZnBr_2
Balance the chemical equation algebraically: HBr + Zn(OH)_2 ⟶ H_2O + ZnBr_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HBr + c_2 Zn(OH)_2 ⟶ c_3 H_2O + c_4 ZnBr_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Br, H, O and Zn: Br: | c_1 = 2 c_4 H: | c_1 + 2 c_2 = 2 c_3 O: | 2 c_2 = c_3 Zn: | c_2 = c_4 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HBr + Zn(OH)_2 ⟶ 2 H_2O + ZnBr_2

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen bromide + zinc hydroxide ⟶ water + zinc bromide
hydrogen bromide + zinc hydroxide ⟶ water + zinc bromide

Equilibrium constant

Construct the equilibrium constant, K, expression for: HBr + Zn(OH)_2 ⟶ H_2O + ZnBr_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: 2 HBr + Zn(OH)_2 ⟶ 2 H_2O + ZnBr_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 HBr | 2 | -2 Zn(OH)_2 | 1 | -1 H_2O | 2 | 2 ZnBr_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HBr | 2 | -2 | ([HBr])^(-2) Zn(OH)_2 | 1 | -1 | ([Zn(OH)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 ZnBr_2 | 1 | 1 | [ZnBr2] 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 = ([HBr])^(-2) ([Zn(OH)2])^(-1) ([H2O])^2 [ZnBr2] = (([H2O])^2 [ZnBr2])/(([HBr])^2 [Zn(OH)2])
Construct the equilibrium constant, K, expression for: HBr + Zn(OH)_2 ⟶ H_2O + ZnBr_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: 2 HBr + Zn(OH)_2 ⟶ 2 H_2O + ZnBr_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 HBr | 2 | -2 Zn(OH)_2 | 1 | -1 H_2O | 2 | 2 ZnBr_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HBr | 2 | -2 | ([HBr])^(-2) Zn(OH)_2 | 1 | -1 | ([Zn(OH)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 ZnBr_2 | 1 | 1 | [ZnBr2] 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 = ([HBr])^(-2) ([Zn(OH)2])^(-1) ([H2O])^2 [ZnBr2] = (([H2O])^2 [ZnBr2])/(([HBr])^2 [Zn(OH)2])

Rate of reaction

Construct the rate of reaction expression for: HBr + Zn(OH)_2 ⟶ H_2O + ZnBr_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: 2 HBr + Zn(OH)_2 ⟶ 2 H_2O + ZnBr_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 HBr | 2 | -2 Zn(OH)_2 | 1 | -1 H_2O | 2 | 2 ZnBr_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 HBr | 2 | -2 | -1/2 (Δ[HBr])/(Δt) Zn(OH)_2 | 1 | -1 | -(Δ[Zn(OH)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) ZnBr_2 | 1 | 1 | (Δ[ZnBr2])/(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[HBr])/(Δt) = -(Δ[Zn(OH)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[ZnBr2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HBr + Zn(OH)_2 ⟶ H_2O + ZnBr_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: 2 HBr + Zn(OH)_2 ⟶ 2 H_2O + ZnBr_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 HBr | 2 | -2 Zn(OH)_2 | 1 | -1 H_2O | 2 | 2 ZnBr_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 HBr | 2 | -2 | -1/2 (Δ[HBr])/(Δt) Zn(OH)_2 | 1 | -1 | -(Δ[Zn(OH)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) ZnBr_2 | 1 | 1 | (Δ[ZnBr2])/(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[HBr])/(Δt) = -(Δ[Zn(OH)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[ZnBr2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen bromide | zinc hydroxide | water | zinc bromide formula | HBr | Zn(OH)_2 | H_2O | ZnBr_2 Hill formula | BrH | H_2O_2Zn | H_2O | Br_2Zn name | hydrogen bromide | zinc hydroxide | water | zinc bromide IUPAC name | hydrogen bromide | zinc dihydroxide | water | dibromozinc
| hydrogen bromide | zinc hydroxide | water | zinc bromide formula | HBr | Zn(OH)_2 | H_2O | ZnBr_2 Hill formula | BrH | H_2O_2Zn | H_2O | Br_2Zn name | hydrogen bromide | zinc hydroxide | water | zinc bromide IUPAC name | hydrogen bromide | zinc dihydroxide | water | dibromozinc

Substance properties

| hydrogen bromide | zinc hydroxide | water | zinc bromide molar mass | 80.912 g/mol | 99.39 g/mol | 18.015 g/mol | 225.2 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | -86.8 °C | | 0 °C | 394 °C boiling point | -66.38 °C | | 99.9839 °C | 675 °C density | 0.003307 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 4.22 g/cm^3 solubility in water | miscible | | | surface tension | 0.0271 N/m | | 0.0728 N/m | dynamic viscosity | 8.4×10^-4 Pa s (at -75 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |
| hydrogen bromide | zinc hydroxide | water | zinc bromide molar mass | 80.912 g/mol | 99.39 g/mol | 18.015 g/mol | 225.2 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | -86.8 °C | | 0 °C | 394 °C boiling point | -66.38 °C | | 99.9839 °C | 675 °C density | 0.003307 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 4.22 g/cm^3 solubility in water | miscible | | | surface tension | 0.0271 N/m | | 0.0728 N/m | dynamic viscosity | 8.4×10^-4 Pa s (at -75 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |

Units

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