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NaOH + H2O2 + Co(NO3)2 = H2O + Na(NO3) + CoO2

Input interpretation

NaOH sodium hydroxide + H_2O_2 hydrogen peroxide + CoN_2O_6 cobaltous nitrate ⟶ H_2O water + NaNO_3 sodium nitrate + CoO2
NaOH sodium hydroxide + H_2O_2 hydrogen peroxide + CoN_2O_6 cobaltous nitrate ⟶ H_2O water + NaNO_3 sodium nitrate + CoO2

Balanced equation

Balance the chemical equation algebraically: NaOH + H_2O_2 + CoN_2O_6 ⟶ H_2O + NaNO_3 + CoO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_2O_2 + c_3 CoN_2O_6 ⟶ c_4 H_2O + c_5 NaNO_3 + c_6 CoO2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Co and N: H: | c_1 + 2 c_2 = 2 c_4 Na: | c_1 = c_5 O: | c_1 + 2 c_2 + 6 c_3 = c_4 + 3 c_5 + 2 c_6 Co: | c_3 = c_6 N: | 2 c_3 = 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 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + H_2O_2 + CoN_2O_6 ⟶ 2 H_2O + 2 NaNO_3 + CoO2
Balance the chemical equation algebraically: NaOH + H_2O_2 + CoN_2O_6 ⟶ H_2O + NaNO_3 + CoO2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_2O_2 + c_3 CoN_2O_6 ⟶ c_4 H_2O + c_5 NaNO_3 + c_6 CoO2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Co and N: H: | c_1 + 2 c_2 = 2 c_4 Na: | c_1 = c_5 O: | c_1 + 2 c_2 + 6 c_3 = c_4 + 3 c_5 + 2 c_6 Co: | c_3 = c_6 N: | 2 c_3 = 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 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + H_2O_2 + CoN_2O_6 ⟶ 2 H_2O + 2 NaNO_3 + CoO2

Structures

+ + ⟶ + + CoO2
+ + ⟶ + + CoO2

Names

sodium hydroxide + hydrogen peroxide + cobaltous nitrate ⟶ water + sodium nitrate + CoO2
sodium hydroxide + hydrogen peroxide + cobaltous nitrate ⟶ water + sodium nitrate + CoO2

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + H_2O_2 + CoN_2O_6 ⟶ H_2O + NaNO_3 + CoO2 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 NaOH + H_2O_2 + CoN_2O_6 ⟶ 2 H_2O + 2 NaNO_3 + CoO2 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 CoN_2O_6 | 1 | -1 H_2O | 2 | 2 NaNO_3 | 2 | 2 CoO2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) CoN_2O_6 | 1 | -1 | ([CoN2O6])^(-1) H_2O | 2 | 2 | ([H2O])^2 NaNO_3 | 2 | 2 | ([NaNO3])^2 CoO2 | 1 | 1 | [CoO2] 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 = ([NaOH])^(-2) ([H2O2])^(-1) ([CoN2O6])^(-1) ([H2O])^2 ([NaNO3])^2 [CoO2] = (([H2O])^2 ([NaNO3])^2 [CoO2])/(([NaOH])^2 [H2O2] [CoN2O6])
Construct the equilibrium constant, K, expression for: NaOH + H_2O_2 + CoN_2O_6 ⟶ H_2O + NaNO_3 + CoO2 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 NaOH + H_2O_2 + CoN_2O_6 ⟶ 2 H_2O + 2 NaNO_3 + CoO2 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 CoN_2O_6 | 1 | -1 H_2O | 2 | 2 NaNO_3 | 2 | 2 CoO2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) CoN_2O_6 | 1 | -1 | ([CoN2O6])^(-1) H_2O | 2 | 2 | ([H2O])^2 NaNO_3 | 2 | 2 | ([NaNO3])^2 CoO2 | 1 | 1 | [CoO2] 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 = ([NaOH])^(-2) ([H2O2])^(-1) ([CoN2O6])^(-1) ([H2O])^2 ([NaNO3])^2 [CoO2] = (([H2O])^2 ([NaNO3])^2 [CoO2])/(([NaOH])^2 [H2O2] [CoN2O6])

Rate of reaction

Construct the rate of reaction expression for: NaOH + H_2O_2 + CoN_2O_6 ⟶ H_2O + NaNO_3 + CoO2 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 NaOH + H_2O_2 + CoN_2O_6 ⟶ 2 H_2O + 2 NaNO_3 + CoO2 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 CoN_2O_6 | 1 | -1 H_2O | 2 | 2 NaNO_3 | 2 | 2 CoO2 | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) CoN_2O_6 | 1 | -1 | -(Δ[CoN2O6])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) CoO2 | 1 | 1 | (Δ[CoO2])/(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[NaOH])/(Δt) = -(Δ[H2O2])/(Δt) = -(Δ[CoN2O6])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = (Δ[CoO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + H_2O_2 + CoN_2O_6 ⟶ H_2O + NaNO_3 + CoO2 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 NaOH + H_2O_2 + CoN_2O_6 ⟶ 2 H_2O + 2 NaNO_3 + CoO2 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 CoN_2O_6 | 1 | -1 H_2O | 2 | 2 NaNO_3 | 2 | 2 CoO2 | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) CoN_2O_6 | 1 | -1 | -(Δ[CoN2O6])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) CoO2 | 1 | 1 | (Δ[CoO2])/(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[NaOH])/(Δt) = -(Δ[H2O2])/(Δt) = -(Δ[CoN2O6])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = (Δ[CoO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | hydrogen peroxide | cobaltous nitrate | water | sodium nitrate | CoO2 formula | NaOH | H_2O_2 | CoN_2O_6 | H_2O | NaNO_3 | CoO2 Hill formula | HNaO | H_2O_2 | CoN_2O_6 | H_2O | NNaO_3 | CoO2 name | sodium hydroxide | hydrogen peroxide | cobaltous nitrate | water | sodium nitrate | IUPAC name | sodium hydroxide | hydrogen peroxide | cobalt(+2) cation dinitrate | water | sodium nitrate |
| sodium hydroxide | hydrogen peroxide | cobaltous nitrate | water | sodium nitrate | CoO2 formula | NaOH | H_2O_2 | CoN_2O_6 | H_2O | NaNO_3 | CoO2 Hill formula | HNaO | H_2O_2 | CoN_2O_6 | H_2O | NNaO_3 | CoO2 name | sodium hydroxide | hydrogen peroxide | cobaltous nitrate | water | sodium nitrate | IUPAC name | sodium hydroxide | hydrogen peroxide | cobalt(+2) cation dinitrate | water | sodium nitrate |

Substance properties

| sodium hydroxide | hydrogen peroxide | cobaltous nitrate | water | sodium nitrate | CoO2 molar mass | 39.997 g/mol | 34.014 g/mol | 182.94 g/mol | 18.015 g/mol | 84.994 g/mol | 90.931 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 323 °C | -0.43 °C | 55 °C | 0 °C | 306 °C | boiling point | 1390 °C | 150.2 °C | | 99.9839 °C | | density | 2.13 g/cm^3 | 1.44 g/cm^3 | 2.49 g/cm^3 | 1 g/cm^3 | 2.26 g/cm^3 | solubility in water | soluble | miscible | soluble | | soluble | surface tension | 0.07435 N/m | 0.0804 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 0.003 Pa s (at 250 °C) | odor | | | | odorless | |
| sodium hydroxide | hydrogen peroxide | cobaltous nitrate | water | sodium nitrate | CoO2 molar mass | 39.997 g/mol | 34.014 g/mol | 182.94 g/mol | 18.015 g/mol | 84.994 g/mol | 90.931 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 323 °C | -0.43 °C | 55 °C | 0 °C | 306 °C | boiling point | 1390 °C | 150.2 °C | | 99.9839 °C | | density | 2.13 g/cm^3 | 1.44 g/cm^3 | 2.49 g/cm^3 | 1 g/cm^3 | 2.26 g/cm^3 | solubility in water | soluble | miscible | soluble | | soluble | surface tension | 0.07435 N/m | 0.0804 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 0.003 Pa s (at 250 °C) | odor | | | | odorless | |

Units

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