Input interpretation
![HCl hydrogen chloride + ZnCO_3 zinc carbonate ⟶ H_2O water + CO_2 carbon dioxide + ZnCl_2 zinc chloride](../image_source/06cda590254d401eca02cb83a6f1b1e6.png)
HCl hydrogen chloride + ZnCO_3 zinc carbonate ⟶ H_2O water + CO_2 carbon dioxide + ZnCl_2 zinc chloride
Balanced equation
![Balance the chemical equation algebraically: HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 ZnCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 ZnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, C, O and Zn: Cl: | c_1 = 2 c_5 H: | c_1 = 2 c_3 C: | c_2 = c_4 O: | 3 c_2 = c_3 + 2 c_4 Zn: | c_2 = 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 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_2](../image_source/fb6d6944cb736a2aeac1c7b56b776b3e.png)
Balance the chemical equation algebraically: HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 ZnCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 ZnCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, C, O and Zn: Cl: | c_1 = 2 c_5 H: | c_1 = 2 c_3 C: | c_2 = c_4 O: | 3 c_2 = c_3 + 2 c_4 Zn: | c_2 = 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 = 2 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_2
Structures
![+ ⟶ + +](../image_source/e5ef11ea9561b9738162c2621bbe4b61.png)
+ ⟶ + +
Names
![hydrogen chloride + zinc carbonate ⟶ water + carbon dioxide + zinc chloride](../image_source/9fce69e716186c0aec17b77b7b14882f.png)
hydrogen chloride + zinc carbonate ⟶ water + carbon dioxide + zinc chloride
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl | 2 | -2 ZnCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 ZnCl_2 | 1 | 1 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) ZnCO_3 | 1 | -1 | ([ZnCO3])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] ZnCl_2 | 1 | 1 | [ZnCl2] 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) ([ZnCO3])^(-1) [H2O] [CO2] [ZnCl2] = ([H2O] [CO2] [ZnCl2])/(([HCl])^2 [ZnCO3])](../image_source/775c2036803b559dfa6455beadb5301c.png)
Construct the equilibrium constant, K, expression for: HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl | 2 | -2 ZnCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 ZnCl_2 | 1 | 1 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) ZnCO_3 | 1 | -1 | ([ZnCO3])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] ZnCl_2 | 1 | 1 | [ZnCl2] 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) ([ZnCO3])^(-1) [H2O] [CO2] [ZnCl2] = ([H2O] [CO2] [ZnCl2])/(([HCl])^2 [ZnCO3])
Rate of reaction
![Construct the rate of reaction expression for: HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl | 2 | -2 ZnCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 ZnCl_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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) ZnCO_3 | 1 | -1 | -(Δ[ZnCO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) ZnCl_2 | 1 | 1 | (Δ[ZnCl2])/(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[ZnCO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[ZnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/32fcfaf5e9b8bd64e72ce3e072be0fbd.png)
Construct the rate of reaction expression for: HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl + ZnCO_3 ⟶ H_2O + CO_2 + ZnCl_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 HCl | 2 | -2 ZnCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 ZnCl_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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) ZnCO_3 | 1 | -1 | -(Δ[ZnCO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) ZnCl_2 | 1 | 1 | (Δ[ZnCl2])/(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[ZnCO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[ZnCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc chloride formula | HCl | ZnCO_3 | H_2O | CO_2 | ZnCl_2 Hill formula | ClH | CO_3Zn | H_2O | CO_2 | Cl_2Zn name | hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc chloride IUPAC name | hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc dichloride](../image_source/2c84414311b1f0c604fb30f37fabc53f.png)
| hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc chloride formula | HCl | ZnCO_3 | H_2O | CO_2 | ZnCl_2 Hill formula | ClH | CO_3Zn | H_2O | CO_2 | Cl_2Zn name | hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc chloride IUPAC name | hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc dichloride
Substance properties
![| hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc chloride molar mass | 36.46 g/mol | 125.4 g/mol | 18.015 g/mol | 44.009 g/mol | 136.3 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -56.56 °C (at triple point) | 293 °C boiling point | -85 °C | | 99.9839 °C | -78.5 °C (at sublimation point) | density | 0.00149 g/cm^3 (at 25 °C) | 4.3476 g/cm^3 | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | solubility in water | miscible | insoluble | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless | odorless](../image_source/268427f7386e5def2b035a6f45fd8ade.png)
| hydrogen chloride | zinc carbonate | water | carbon dioxide | zinc chloride molar mass | 36.46 g/mol | 125.4 g/mol | 18.015 g/mol | 44.009 g/mol | 136.3 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | -56.56 °C (at triple point) | 293 °C boiling point | -85 °C | | 99.9839 °C | -78.5 °C (at sublimation point) | density | 0.00149 g/cm^3 (at 25 °C) | 4.3476 g/cm^3 | 1 g/cm^3 | 0.00184212 g/cm^3 (at 20 °C) | solubility in water | miscible | insoluble | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 1.491×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless | odorless
Units