Input interpretation
![HCl hydrogen chloride + KHCO_3 potassium bicarbonate ⟶ H_2O water + CO_2 carbon dioxide + KCl potassium chloride](../image_source/2f6826705ea1fef894282fa338b60d38.png)
HCl hydrogen chloride + KHCO_3 potassium bicarbonate ⟶ H_2O water + CO_2 carbon dioxide + KCl potassium chloride
Balanced equation
![Balance the chemical equation algebraically: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KHCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, C, K and O: Cl: | c_1 = c_5 H: | c_1 + c_2 = 2 c_3 C: | c_2 = c_4 K: | c_2 = c_5 O: | 3 c_2 = c_3 + 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 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: | | HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl](../image_source/6ce562132fe1d1c1b20cf7083be71e66.png)
Balance the chemical equation algebraically: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KHCO_3 ⟶ c_3 H_2O + c_4 CO_2 + c_5 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, C, K and O: Cl: | c_1 = c_5 H: | c_1 + c_2 = 2 c_3 C: | c_2 = c_4 K: | c_2 = c_5 O: | 3 c_2 = c_3 + 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 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: | | HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl
Structures
![+ ⟶ + +](../image_source/46b6d36d2d85d8d7da8a930f6a63d4a9.png)
+ ⟶ + +
Names
![hydrogen chloride + potassium bicarbonate ⟶ water + carbon dioxide + potassium chloride](../image_source/2f3e8ca79dcbe84ce79bc08059d33845.png)
hydrogen chloride + potassium bicarbonate ⟶ water + carbon dioxide + potassium chloride
Reaction thermodynamics
Enthalpy
![| hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride molecular enthalpy | -92.3 kJ/mol | -963.2 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol | -436.5 kJ/mol total enthalpy | -92.3 kJ/mol | -963.2 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol | -436.5 kJ/mol | H_initial = -1056 kJ/mol | | H_final = -1116 kJ/mol | | ΔH_rxn^0 | -1116 kJ/mol - -1056 kJ/mol = -60.33 kJ/mol (exothermic) | | | |](../image_source/d5ae31330d5e27c87749572f6ddf19cd.png)
| hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride molecular enthalpy | -92.3 kJ/mol | -963.2 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol | -436.5 kJ/mol total enthalpy | -92.3 kJ/mol | -963.2 kJ/mol | -285.8 kJ/mol | -393.5 kJ/mol | -436.5 kJ/mol | H_initial = -1056 kJ/mol | | H_final = -1116 kJ/mol | | ΔH_rxn^0 | -1116 kJ/mol - -1056 kJ/mol = -60.33 kJ/mol (exothermic) | | | |
Gibbs free energy
![| hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride molecular free energy | -95.3 kJ/mol | -863.5 kJ/mol | -237.1 kJ/mol | -394.4 kJ/mol | -408.5 kJ/mol total free energy | -95.3 kJ/mol | -863.5 kJ/mol | -237.1 kJ/mol | -394.4 kJ/mol | -408.5 kJ/mol | G_initial = -958.8 kJ/mol | | G_final = -1040 kJ/mol | | ΔG_rxn^0 | -1040 kJ/mol - -958.8 kJ/mol = -81.2 kJ/mol (exergonic) | | | |](../image_source/4a9ec69f79167eaab0e56164eeb6b758.png)
| hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride molecular free energy | -95.3 kJ/mol | -863.5 kJ/mol | -237.1 kJ/mol | -394.4 kJ/mol | -408.5 kJ/mol total free energy | -95.3 kJ/mol | -863.5 kJ/mol | -237.1 kJ/mol | -394.4 kJ/mol | -408.5 kJ/mol | G_initial = -958.8 kJ/mol | | G_final = -1040 kJ/mol | | ΔG_rxn^0 | -1040 kJ/mol - -958.8 kJ/mol = -81.2 kJ/mol (exergonic) | | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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 | 1 | -1 KHCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 KCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 1 | -1 | ([HCl])^(-1) KHCO_3 | 1 | -1 | ([KHCO3])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] KCl | 1 | 1 | [KCl] 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])^(-1) ([KHCO3])^(-1) [H2O] [CO2] [KCl] = ([H2O] [CO2] [KCl])/([HCl] [KHCO3])](../image_source/2e939897e952ee2297224f736a8bd12f.png)
Construct the equilibrium constant, K, expression for: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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 | 1 | -1 KHCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 KCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 1 | -1 | ([HCl])^(-1) KHCO_3 | 1 | -1 | ([KHCO3])^(-1) H_2O | 1 | 1 | [H2O] CO_2 | 1 | 1 | [CO2] KCl | 1 | 1 | [KCl] 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])^(-1) ([KHCO3])^(-1) [H2O] [CO2] [KCl] = ([H2O] [CO2] [KCl])/([HCl] [KHCO3])
Rate of reaction
![Construct the rate of reaction expression for: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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 | 1 | -1 KHCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 KCl | 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 | 1 | -1 | -(Δ[HCl])/(Δt) KHCO_3 | 1 | -1 | -(Δ[KHCO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(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 = -(Δ[HCl])/(Δt) = -(Δ[KHCO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/bb5c97ea91ec8954b3de64050506b47b.png)
Construct the rate of reaction expression for: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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: HCl + KHCO_3 ⟶ H_2O + CO_2 + KCl 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 | 1 | -1 KHCO_3 | 1 | -1 H_2O | 1 | 1 CO_2 | 1 | 1 KCl | 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 | 1 | -1 | -(Δ[HCl])/(Δt) KHCO_3 | 1 | -1 | -(Δ[KHCO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CO_2 | 1 | 1 | (Δ[CO2])/(Δt) KCl | 1 | 1 | (Δ[KCl])/(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 = -(Δ[HCl])/(Δt) = -(Δ[KHCO3])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CO2])/(Δt) = (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride formula | HCl | KHCO_3 | H_2O | CO_2 | KCl Hill formula | ClH | CHKO_3 | H_2O | CO_2 | ClK name | hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride IUPAC name | hydrogen chloride | potassium hydrogen carbonate | water | carbon dioxide | potassium chloride](../image_source/4392fbeda08824ceaa01a75cfa458c3c.png)
| hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride formula | HCl | KHCO_3 | H_2O | CO_2 | KCl Hill formula | ClH | CHKO_3 | H_2O | CO_2 | ClK name | hydrogen chloride | potassium bicarbonate | water | carbon dioxide | potassium chloride IUPAC name | hydrogen chloride | potassium hydrogen carbonate | water | carbon dioxide | potassium chloride