NaOH + Na2O2 + Mo(NO3)3 = H2O + NaNO3 + Na2MoO4

NaOH sodium hydroxide + Na_2O_2 sodium peroxide + Mo(NO3)3 ⟶ H_2O water + NaNO_3 sodium nitrate + Na_2MoO_4 sodium molybdate

Balance the chemical equation algebraically: NaOH + Na_2O_2 + Mo(NO3)3 ⟶ H_2O + NaNO_3 + Na_2MoO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Na_2O_2 + c_3 Mo(NO3)3 ⟶ c_4 H_2O + c_5 NaNO_3 + c_6 Na_2MoO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Mo and N: H: | c_1 = 2 c_4 Na: | c_1 + 2 c_2 = c_5 + 2 c_6 O: | c_1 + 2 c_2 + 9 c_3 = c_4 + 3 c_5 + 4 c_6 Mo: | c_3 = c_6 N: | 3 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3/2 c_3 = 1 c_4 = 1 c_5 = 3 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 4 c_2 = 3 c_3 = 2 c_4 = 2 c_5 = 6 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + 3 Na_2O_2 + 2 Mo(NO3)3 ⟶ 2 H_2O + 6 NaNO_3 + 2 Na_2MoO_4

+ + Mo(NO3)3 ⟶ + +

sodium hydroxide + sodium peroxide + Mo(NO3)3 ⟶ water + sodium nitrate + sodium molybdate

Construct the equilibrium constant, K, expression for: NaOH + Na_2O_2 + Mo(NO3)3 ⟶ H_2O + NaNO_3 + Na_2MoO_4 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: 4 NaOH + 3 Na_2O_2 + 2 Mo(NO3)3 ⟶ 2 H_2O + 6 NaNO_3 + 2 Na_2MoO_4 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 | 4 | -4 Na_2O_2 | 3 | -3 Mo(NO3)3 | 2 | -2 H_2O | 2 | 2 NaNO_3 | 6 | 6 Na_2MoO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 4 | -4 | ([NaOH])^(-4) Na_2O_2 | 3 | -3 | ([Na2O2])^(-3) Mo(NO3)3 | 2 | -2 | ([Mo(NO3)3])^(-2) H_2O | 2 | 2 | ([H2O])^2 NaNO_3 | 6 | 6 | ([NaNO3])^6 Na_2MoO_4 | 2 | 2 | ([Na2MoO4])^2 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])^(-4) ([Na2O2])^(-3) ([Mo(NO3)3])^(-2) ([H2O])^2 ([NaNO3])^6 ([Na2MoO4])^2 = (([H2O])^2 ([NaNO3])^6 ([Na2MoO4])^2)/(([NaOH])^4 ([Na2O2])^3 ([Mo(NO3)3])^2)

Construct the rate of reaction expression for: NaOH + Na_2O_2 + Mo(NO3)3 ⟶ H_2O + NaNO_3 + Na_2MoO_4 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: 4 NaOH + 3 Na_2O_2 + 2 Mo(NO3)3 ⟶ 2 H_2O + 6 NaNO_3 + 2 Na_2MoO_4 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 | 4 | -4 Na_2O_2 | 3 | -3 Mo(NO3)3 | 2 | -2 H_2O | 2 | 2 NaNO_3 | 6 | 6 Na_2MoO_4 | 2 | 2 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 | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) Na_2O_2 | 3 | -3 | -1/3 (Δ[Na2O2])/(Δt) Mo(NO3)3 | 2 | -2 | -1/2 (Δ[Mo(NO3)3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NaNO_3 | 6 | 6 | 1/6 (Δ[NaNO3])/(Δt) Na_2MoO_4 | 2 | 2 | 1/2 (Δ[Na2MoO4])/(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 = -1/4 (Δ[NaOH])/(Δt) = -1/3 (Δ[Na2O2])/(Δt) = -1/2 (Δ[Mo(NO3)3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/6 (Δ[NaNO3])/(Δt) = 1/2 (Δ[Na2MoO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hydroxide | sodium peroxide | Mo(NO3)3 | water | sodium nitrate | sodium molybdate formula | NaOH | Na_2O_2 | Mo(NO3)3 | H_2O | NaNO_3 | Na_2MoO_4 Hill formula | HNaO | Na_2O_2 | MoN3O9 | H_2O | NNaO_3 | MoNa_2O_4 name | sodium hydroxide | sodium peroxide | | water | sodium nitrate | sodium molybdate IUPAC name | sodium hydroxide | disodium peroxide | | water | sodium nitrate | disodium dioxido-dioxomolybdenum

| sodium hydroxide | sodium peroxide | Mo(NO3)3 | water | sodium nitrate | sodium molybdate molar mass | 39.997 g/mol | 77.978 g/mol | 282 g/mol | 18.015 g/mol | 84.994 g/mol | 205.9 g/mol phase | solid (at STP) | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | 660 °C | | 0 °C | 306 °C | 687 °C boiling point | 1390 °C | | | 99.9839 °C | | density | 2.13 g/cm^3 | 2.805 g/cm^3 | | 1 g/cm^3 | 2.26 g/cm^3 | 3.78 g/cm^3 solubility in water | soluble | reacts | | | soluble | surface tension | 0.07435 N/m | | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | 8.9×10^-4 Pa s (at 25 °C) | 0.003 Pa s (at 250 °C) | odor | | | | odorless | |