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H2O + Mg + RbNO3 = NH3 + Mg(OH)2 + RbO2

Input interpretation

H_2O water + Mg magnesium + RbNO_3 rubidium nitrate ⟶ NH_3 ammonia + Mg(OH)_2 magnesium hydroxide + RbO_2 rubidium superoxide
H_2O water + Mg magnesium + RbNO_3 rubidium nitrate ⟶ NH_3 ammonia + Mg(OH)_2 magnesium hydroxide + RbO_2 rubidium superoxide

Balanced equation

Balance the chemical equation algebraically: H_2O + Mg + RbNO_3 ⟶ NH_3 + Mg(OH)_2 + RbO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Mg + c_3 RbNO_3 ⟶ c_4 NH_3 + c_5 Mg(OH)_2 + c_6 RbO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Mg, N and Rb: H: | 2 c_1 = 3 c_4 + 2 c_5 O: | c_1 + 3 c_3 = 2 c_5 + 2 c_6 Mg: | c_2 = c_5 N: | c_3 = c_4 Rb: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 5/2 c_3 = 1 c_4 = 1 c_5 = 5/2 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 5 c_3 = 2 c_4 = 2 c_5 = 5 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2O + 5 Mg + 2 RbNO_3 ⟶ 2 NH_3 + 5 Mg(OH)_2 + 2 RbO_2
Balance the chemical equation algebraically: H_2O + Mg + RbNO_3 ⟶ NH_3 + Mg(OH)_2 + RbO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Mg + c_3 RbNO_3 ⟶ c_4 NH_3 + c_5 Mg(OH)_2 + c_6 RbO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Mg, N and Rb: H: | 2 c_1 = 3 c_4 + 2 c_5 O: | c_1 + 3 c_3 = 2 c_5 + 2 c_6 Mg: | c_2 = c_5 N: | c_3 = c_4 Rb: | c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 5/2 c_3 = 1 c_4 = 1 c_5 = 5/2 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 5 c_3 = 2 c_4 = 2 c_5 = 5 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 H_2O + 5 Mg + 2 RbNO_3 ⟶ 2 NH_3 + 5 Mg(OH)_2 + 2 RbO_2

Structures

+ + ⟶ + + RbO_2
+ + ⟶ + + RbO_2

Names

water + magnesium + rubidium nitrate ⟶ ammonia + magnesium hydroxide + rubidium superoxide
water + magnesium + rubidium nitrate ⟶ ammonia + magnesium hydroxide + rubidium superoxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Mg + RbNO_3 ⟶ NH_3 + Mg(OH)_2 + RbO_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: 8 H_2O + 5 Mg + 2 RbNO_3 ⟶ 2 NH_3 + 5 Mg(OH)_2 + 2 RbO_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 | 8 | -8 Mg | 5 | -5 RbNO_3 | 2 | -2 NH_3 | 2 | 2 Mg(OH)_2 | 5 | 5 RbO_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 8 | -8 | ([H2O])^(-8) Mg | 5 | -5 | ([Mg])^(-5) RbNO_3 | 2 | -2 | ([RbNO3])^(-2) NH_3 | 2 | 2 | ([NH3])^2 Mg(OH)_2 | 5 | 5 | ([Mg(OH)2])^5 RbO_2 | 2 | 2 | ([RbO2])^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 = ([H2O])^(-8) ([Mg])^(-5) ([RbNO3])^(-2) ([NH3])^2 ([Mg(OH)2])^5 ([RbO2])^2 = (([NH3])^2 ([Mg(OH)2])^5 ([RbO2])^2)/(([H2O])^8 ([Mg])^5 ([RbNO3])^2)
Construct the equilibrium constant, K, expression for: H_2O + Mg + RbNO_3 ⟶ NH_3 + Mg(OH)_2 + RbO_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: 8 H_2O + 5 Mg + 2 RbNO_3 ⟶ 2 NH_3 + 5 Mg(OH)_2 + 2 RbO_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 | 8 | -8 Mg | 5 | -5 RbNO_3 | 2 | -2 NH_3 | 2 | 2 Mg(OH)_2 | 5 | 5 RbO_2 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 8 | -8 | ([H2O])^(-8) Mg | 5 | -5 | ([Mg])^(-5) RbNO_3 | 2 | -2 | ([RbNO3])^(-2) NH_3 | 2 | 2 | ([NH3])^2 Mg(OH)_2 | 5 | 5 | ([Mg(OH)2])^5 RbO_2 | 2 | 2 | ([RbO2])^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 = ([H2O])^(-8) ([Mg])^(-5) ([RbNO3])^(-2) ([NH3])^2 ([Mg(OH)2])^5 ([RbO2])^2 = (([NH3])^2 ([Mg(OH)2])^5 ([RbO2])^2)/(([H2O])^8 ([Mg])^5 ([RbNO3])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2O + Mg + RbNO_3 ⟶ NH_3 + Mg(OH)_2 + RbO_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: 8 H_2O + 5 Mg + 2 RbNO_3 ⟶ 2 NH_3 + 5 Mg(OH)_2 + 2 RbO_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 | 8 | -8 Mg | 5 | -5 RbNO_3 | 2 | -2 NH_3 | 2 | 2 Mg(OH)_2 | 5 | 5 RbO_2 | 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 H_2O | 8 | -8 | -1/8 (Δ[H2O])/(Δt) Mg | 5 | -5 | -1/5 (Δ[Mg])/(Δt) RbNO_3 | 2 | -2 | -1/2 (Δ[RbNO3])/(Δt) NH_3 | 2 | 2 | 1/2 (Δ[NH3])/(Δt) Mg(OH)_2 | 5 | 5 | 1/5 (Δ[Mg(OH)2])/(Δt) RbO_2 | 2 | 2 | 1/2 (Δ[RbO2])/(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 = -1/8 (Δ[H2O])/(Δt) = -1/5 (Δ[Mg])/(Δt) = -1/2 (Δ[RbNO3])/(Δt) = 1/2 (Δ[NH3])/(Δt) = 1/5 (Δ[Mg(OH)2])/(Δt) = 1/2 (Δ[RbO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Mg + RbNO_3 ⟶ NH_3 + Mg(OH)_2 + RbO_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: 8 H_2O + 5 Mg + 2 RbNO_3 ⟶ 2 NH_3 + 5 Mg(OH)_2 + 2 RbO_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 | 8 | -8 Mg | 5 | -5 RbNO_3 | 2 | -2 NH_3 | 2 | 2 Mg(OH)_2 | 5 | 5 RbO_2 | 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 H_2O | 8 | -8 | -1/8 (Δ[H2O])/(Δt) Mg | 5 | -5 | -1/5 (Δ[Mg])/(Δt) RbNO_3 | 2 | -2 | -1/2 (Δ[RbNO3])/(Δt) NH_3 | 2 | 2 | 1/2 (Δ[NH3])/(Δt) Mg(OH)_2 | 5 | 5 | 1/5 (Δ[Mg(OH)2])/(Δt) RbO_2 | 2 | 2 | 1/2 (Δ[RbO2])/(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 = -1/8 (Δ[H2O])/(Δt) = -1/5 (Δ[Mg])/(Δt) = -1/2 (Δ[RbNO3])/(Δt) = 1/2 (Δ[NH3])/(Δt) = 1/5 (Δ[Mg(OH)2])/(Δt) = 1/2 (Δ[RbO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | magnesium | rubidium nitrate | ammonia | magnesium hydroxide | rubidium superoxide formula | H_2O | Mg | RbNO_3 | NH_3 | Mg(OH)_2 | RbO_2 Hill formula | H_2O | Mg | NO_3Rb | H_3N | H_2MgO_2 | O_2Rb_1 name | water | magnesium | rubidium nitrate | ammonia | magnesium hydroxide | rubidium superoxide IUPAC name | water | magnesium | rubidium(+1) cation nitrate | ammonia | magnesium dihydroxide |
| water | magnesium | rubidium nitrate | ammonia | magnesium hydroxide | rubidium superoxide formula | H_2O | Mg | RbNO_3 | NH_3 | Mg(OH)_2 | RbO_2 Hill formula | H_2O | Mg | NO_3Rb | H_3N | H_2MgO_2 | O_2Rb_1 name | water | magnesium | rubidium nitrate | ammonia | magnesium hydroxide | rubidium superoxide IUPAC name | water | magnesium | rubidium(+1) cation nitrate | ammonia | magnesium dihydroxide |

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