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H2O2 + Ca(ClO2)2 = H2O + O2 + CaCl2

Input interpretation

H_2O_2 hydrogen peroxide + Ca(ClO_2)_2 calcium chlorite ⟶ H_2O water + O_2 oxygen + CaCl_2 calcium chloride
H_2O_2 hydrogen peroxide + Ca(ClO_2)_2 calcium chlorite ⟶ H_2O water + O_2 oxygen + CaCl_2 calcium chloride

Balanced equation

Balance the chemical equation algebraically: H_2O_2 + Ca(ClO_2)_2 ⟶ H_2O + O_2 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 Ca(ClO_2)_2 ⟶ c_3 H_2O + c_4 O_2 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ca and Cl: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + 4 c_2 = c_3 + 2 c_4 Ca: | c_2 = c_5 Cl: | 2 c_2 = 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_2 = 1 c_3 = c_1 c_4 = c_1/2 + 2 c_5 = 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O_2 + Ca(ClO_2)_2 ⟶ 2 H_2O + 3 O_2 + CaCl_2
Balance the chemical equation algebraically: H_2O_2 + Ca(ClO_2)_2 ⟶ H_2O + O_2 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 Ca(ClO_2)_2 ⟶ c_3 H_2O + c_4 O_2 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ca and Cl: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + 4 c_2 = c_3 + 2 c_4 Ca: | c_2 = c_5 Cl: | 2 c_2 = 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_2 = 1 c_3 = c_1 c_4 = c_1/2 + 2 c_5 = 1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O_2 + Ca(ClO_2)_2 ⟶ 2 H_2O + 3 O_2 + CaCl_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

hydrogen peroxide + calcium chlorite ⟶ water + oxygen + calcium chloride
hydrogen peroxide + calcium chlorite ⟶ water + oxygen + calcium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O_2 + Ca(ClO_2)_2 ⟶ H_2O + O_2 + CaCl_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 H_2O_2 + Ca(ClO_2)_2 ⟶ 2 H_2O + 3 O_2 + CaCl_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 H_2O_2 | 2 | -2 Ca(ClO_2)_2 | 1 | -1 H_2O | 2 | 2 O_2 | 3 | 3 CaCl_2 | 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_2 | 2 | -2 | ([H2O2])^(-2) Ca(ClO_2)_2 | 1 | -1 | ([Ca(ClO2)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 O_2 | 3 | 3 | ([O2])^3 CaCl_2 | 1 | 1 | [CaCl2] 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 = ([H2O2])^(-2) ([Ca(ClO2)2])^(-1) ([H2O])^2 ([O2])^3 [CaCl2] = (([H2O])^2 ([O2])^3 [CaCl2])/(([H2O2])^2 [Ca(ClO2)2])
Construct the equilibrium constant, K, expression for: H_2O_2 + Ca(ClO_2)_2 ⟶ H_2O + O_2 + CaCl_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 H_2O_2 + Ca(ClO_2)_2 ⟶ 2 H_2O + 3 O_2 + CaCl_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 H_2O_2 | 2 | -2 Ca(ClO_2)_2 | 1 | -1 H_2O | 2 | 2 O_2 | 3 | 3 CaCl_2 | 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_2 | 2 | -2 | ([H2O2])^(-2) Ca(ClO_2)_2 | 1 | -1 | ([Ca(ClO2)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 O_2 | 3 | 3 | ([O2])^3 CaCl_2 | 1 | 1 | [CaCl2] 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 = ([H2O2])^(-2) ([Ca(ClO2)2])^(-1) ([H2O])^2 ([O2])^3 [CaCl2] = (([H2O])^2 ([O2])^3 [CaCl2])/(([H2O2])^2 [Ca(ClO2)2])

Rate of reaction

Construct the rate of reaction expression for: H_2O_2 + Ca(ClO_2)_2 ⟶ H_2O + O_2 + CaCl_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 H_2O_2 + Ca(ClO_2)_2 ⟶ 2 H_2O + 3 O_2 + CaCl_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 H_2O_2 | 2 | -2 Ca(ClO_2)_2 | 1 | -1 H_2O | 2 | 2 O_2 | 3 | 3 CaCl_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 H_2O_2 | 2 | -2 | -1/2 (Δ[H2O2])/(Δt) Ca(ClO_2)_2 | 1 | -1 | -(Δ[Ca(ClO2)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) CaCl_2 | 1 | 1 | (Δ[CaCl2])/(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[H2O2])/(Δt) = -(Δ[Ca(ClO2)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O_2 + Ca(ClO_2)_2 ⟶ H_2O + O_2 + CaCl_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 H_2O_2 + Ca(ClO_2)_2 ⟶ 2 H_2O + 3 O_2 + CaCl_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 H_2O_2 | 2 | -2 Ca(ClO_2)_2 | 1 | -1 H_2O | 2 | 2 O_2 | 3 | 3 CaCl_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 H_2O_2 | 2 | -2 | -1/2 (Δ[H2O2])/(Δt) Ca(ClO_2)_2 | 1 | -1 | -(Δ[Ca(ClO2)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) O_2 | 3 | 3 | 1/3 (Δ[O2])/(Δt) CaCl_2 | 1 | 1 | (Δ[CaCl2])/(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[H2O2])/(Δt) = -(Δ[Ca(ClO2)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[O2])/(Δt) = (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen peroxide | calcium chlorite | water | oxygen | calcium chloride formula | H_2O_2 | Ca(ClO_2)_2 | H_2O | O_2 | CaCl_2 Hill formula | H_2O_2 | CaCl_2O_4 | H_2O | O_2 | CaCl_2 name | hydrogen peroxide | calcium chlorite | water | oxygen | calcium chloride IUPAC name | hydrogen peroxide | calcium dichlorite | water | molecular oxygen | calcium dichloride
| hydrogen peroxide | calcium chlorite | water | oxygen | calcium chloride formula | H_2O_2 | Ca(ClO_2)_2 | H_2O | O_2 | CaCl_2 Hill formula | H_2O_2 | CaCl_2O_4 | H_2O | O_2 | CaCl_2 name | hydrogen peroxide | calcium chlorite | water | oxygen | calcium chloride IUPAC name | hydrogen peroxide | calcium dichlorite | water | molecular oxygen | calcium dichloride

Substance properties

| hydrogen peroxide | calcium chlorite | water | oxygen | calcium chloride molar mass | 34.014 g/mol | 175 g/mol | 18.015 g/mol | 31.998 g/mol | 111 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -0.43 °C | | 0 °C | -218 °C | 772 °C boiling point | 150.2 °C | | 99.9839 °C | -183 °C | density | 1.44 g/cm^3 | 2.71 g/cm^3 | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 2.15 g/cm^3 solubility in water | miscible | | | | soluble surface tension | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |
| hydrogen peroxide | calcium chlorite | water | oxygen | calcium chloride molar mass | 34.014 g/mol | 175 g/mol | 18.015 g/mol | 31.998 g/mol | 111 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -0.43 °C | | 0 °C | -218 °C | 772 °C boiling point | 150.2 °C | | 99.9839 °C | -183 °C | density | 1.44 g/cm^3 | 2.71 g/cm^3 | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 2.15 g/cm^3 solubility in water | miscible | | | | soluble surface tension | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |

Units

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