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H2O + CO2 + MnO2 + KI = I2 + KHCO3 + MnCO3

Input interpretation

H_2O water + CO_2 carbon dioxide + MnO_2 manganese dioxide + KI potassium iodide ⟶ I_2 iodine + KHCO_3 potassium bicarbonate + MnCO_3 manganese carbonate
H_2O water + CO_2 carbon dioxide + MnO_2 manganese dioxide + KI potassium iodide ⟶ I_2 iodine + KHCO_3 potassium bicarbonate + MnCO_3 manganese carbonate

Balanced equation

Balance the chemical equation algebraically: H_2O + CO_2 + MnO_2 + KI ⟶ I_2 + KHCO_3 + MnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 CO_2 + c_3 MnO_2 + c_4 KI ⟶ c_5 I_2 + c_6 KHCO_3 + c_7 MnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, C, Mn, I and K: H: | 2 c_1 = c_6 O: | c_1 + 2 c_2 + 2 c_3 = 3 c_6 + 3 c_7 C: | c_2 = c_6 + c_7 Mn: | c_3 = c_7 I: | c_4 = 2 c_5 K: | c_4 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + 3 CO_2 + MnO_2 + 2 KI ⟶ I_2 + 2 KHCO_3 + MnCO_3
Balance the chemical equation algebraically: H_2O + CO_2 + MnO_2 + KI ⟶ I_2 + KHCO_3 + MnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 CO_2 + c_3 MnO_2 + c_4 KI ⟶ c_5 I_2 + c_6 KHCO_3 + c_7 MnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, C, Mn, I and K: H: | 2 c_1 = c_6 O: | c_1 + 2 c_2 + 2 c_3 = 3 c_6 + 3 c_7 C: | c_2 = c_6 + c_7 Mn: | c_3 = c_7 I: | c_4 = 2 c_5 K: | c_4 = 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 1 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O + 3 CO_2 + MnO_2 + 2 KI ⟶ I_2 + 2 KHCO_3 + MnCO_3

Structures

+ + + ⟶ + +
+ + + ⟶ + +

Names

water + carbon dioxide + manganese dioxide + potassium iodide ⟶ iodine + potassium bicarbonate + manganese carbonate
water + carbon dioxide + manganese dioxide + potassium iodide ⟶ iodine + potassium bicarbonate + manganese carbonate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + CO_2 + MnO_2 + KI ⟶ I_2 + KHCO_3 + MnCO_3 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: H_2O + 3 CO_2 + MnO_2 + 2 KI ⟶ I_2 + 2 KHCO_3 + MnCO_3 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 | 1 | -1 CO_2 | 3 | -3 MnO_2 | 1 | -1 KI | 2 | -2 I_2 | 1 | 1 KHCO_3 | 2 | 2 MnCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) CO_2 | 3 | -3 | ([CO2])^(-3) MnO_2 | 1 | -1 | ([MnO2])^(-1) KI | 2 | -2 | ([KI])^(-2) I_2 | 1 | 1 | [I2] KHCO_3 | 2 | 2 | ([KHCO3])^2 MnCO_3 | 1 | 1 | [MnCO3] 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])^(-1) ([CO2])^(-3) ([MnO2])^(-1) ([KI])^(-2) [I2] ([KHCO3])^2 [MnCO3] = ([I2] ([KHCO3])^2 [MnCO3])/([H2O] ([CO2])^3 [MnO2] ([KI])^2)
Construct the equilibrium constant, K, expression for: H_2O + CO_2 + MnO_2 + KI ⟶ I_2 + KHCO_3 + MnCO_3 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: H_2O + 3 CO_2 + MnO_2 + 2 KI ⟶ I_2 + 2 KHCO_3 + MnCO_3 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 | 1 | -1 CO_2 | 3 | -3 MnO_2 | 1 | -1 KI | 2 | -2 I_2 | 1 | 1 KHCO_3 | 2 | 2 MnCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 1 | -1 | ([H2O])^(-1) CO_2 | 3 | -3 | ([CO2])^(-3) MnO_2 | 1 | -1 | ([MnO2])^(-1) KI | 2 | -2 | ([KI])^(-2) I_2 | 1 | 1 | [I2] KHCO_3 | 2 | 2 | ([KHCO3])^2 MnCO_3 | 1 | 1 | [MnCO3] 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])^(-1) ([CO2])^(-3) ([MnO2])^(-1) ([KI])^(-2) [I2] ([KHCO3])^2 [MnCO3] = ([I2] ([KHCO3])^2 [MnCO3])/([H2O] ([CO2])^3 [MnO2] ([KI])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2O + CO_2 + MnO_2 + KI ⟶ I_2 + KHCO_3 + MnCO_3 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: H_2O + 3 CO_2 + MnO_2 + 2 KI ⟶ I_2 + 2 KHCO_3 + MnCO_3 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 | 1 | -1 CO_2 | 3 | -3 MnO_2 | 1 | -1 KI | 2 | -2 I_2 | 1 | 1 KHCO_3 | 2 | 2 MnCO_3 | 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_2O | 1 | -1 | -(Δ[H2O])/(Δt) CO_2 | 3 | -3 | -1/3 (Δ[CO2])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) KHCO_3 | 2 | 2 | 1/2 (Δ[KHCO3])/(Δt) MnCO_3 | 1 | 1 | (Δ[MnCO3])/(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[H2O])/(Δt) = -1/3 (Δ[CO2])/(Δt) = -(Δ[MnO2])/(Δt) = -1/2 (Δ[KI])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[KHCO3])/(Δt) = (Δ[MnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + CO_2 + MnO_2 + KI ⟶ I_2 + KHCO_3 + MnCO_3 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: H_2O + 3 CO_2 + MnO_2 + 2 KI ⟶ I_2 + 2 KHCO_3 + MnCO_3 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 | 1 | -1 CO_2 | 3 | -3 MnO_2 | 1 | -1 KI | 2 | -2 I_2 | 1 | 1 KHCO_3 | 2 | 2 MnCO_3 | 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_2O | 1 | -1 | -(Δ[H2O])/(Δt) CO_2 | 3 | -3 | -1/3 (Δ[CO2])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) KI | 2 | -2 | -1/2 (Δ[KI])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) KHCO_3 | 2 | 2 | 1/2 (Δ[KHCO3])/(Δt) MnCO_3 | 1 | 1 | (Δ[MnCO3])/(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[H2O])/(Δt) = -1/3 (Δ[CO2])/(Δt) = -(Δ[MnO2])/(Δt) = -1/2 (Δ[KI])/(Δt) = (Δ[I2])/(Δt) = 1/2 (Δ[KHCO3])/(Δt) = (Δ[MnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | carbon dioxide | manganese dioxide | potassium iodide | iodine | potassium bicarbonate | manganese carbonate formula | H_2O | CO_2 | MnO_2 | KI | I_2 | KHCO_3 | MnCO_3 Hill formula | H_2O | CO_2 | MnO_2 | IK | I_2 | CHKO_3 | CMnO_3 name | water | carbon dioxide | manganese dioxide | potassium iodide | iodine | potassium bicarbonate | manganese carbonate IUPAC name | water | carbon dioxide | dioxomanganese | potassium iodide | molecular iodine | potassium hydrogen carbonate | manganous carbonate
| water | carbon dioxide | manganese dioxide | potassium iodide | iodine | potassium bicarbonate | manganese carbonate formula | H_2O | CO_2 | MnO_2 | KI | I_2 | KHCO_3 | MnCO_3 Hill formula | H_2O | CO_2 | MnO_2 | IK | I_2 | CHKO_3 | CMnO_3 name | water | carbon dioxide | manganese dioxide | potassium iodide | iodine | potassium bicarbonate | manganese carbonate IUPAC name | water | carbon dioxide | dioxomanganese | potassium iodide | molecular iodine | potassium hydrogen carbonate | manganous carbonate

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