Ca(OH)2 + HNO2 = H2O + Ca(NO2)2

Input interpretation

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Ca(OH)_2 calcium hydroxide + HNO_2 nitrous acid ⟶ H_2O water + Ca(NO_2)_2 calcium nitrite

Balanced equation

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Balance the chemical equation algebraically: Ca(OH)_2 + HNO_2 ⟶ H_2O + Ca(NO_2)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(OH)_2 + c_2 HNO_2 ⟶ c_3 H_2O + c_4 Ca(NO_2)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, H, O and N: Ca: | c_1 = c_4 H: | 2 c_1 + c_2 = 2 c_3 O: | 2 c_1 + 2 c_2 = c_3 + 4 c_4 N: | c_2 = 2 c_4 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 = 2 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Ca(OH)_2 + 2 HNO_2 ⟶ 2 H_2O + Ca(NO_2)_2

+ ⟶ +

Names

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calcium hydroxide + nitrous acid ⟶ water + calcium nitrite

Equilibrium constant

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Construct the equilibrium constant, K, expression for: Ca(OH)_2 + HNO_2 ⟶ H_2O + Ca(NO_2)_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: Ca(OH)_2 + 2 HNO_2 ⟶ 2 H_2O + Ca(NO_2)_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 Ca(OH)_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 Ca(NO_2)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(OH)_2 | 1 | -1 | ([Ca(OH)2])^(-1) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 Ca(NO_2)_2 | 1 | 1 | [Ca(NO2)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 = ([Ca(OH)2])^(-1) ([HNO2])^(-2) ([H2O])^2 [Ca(NO2)2] = (([H2O])^2 [Ca(NO2)2])/([Ca(OH)2] ([HNO2])^2)

Rate of reaction

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Construct the rate of reaction expression for: Ca(OH)_2 + HNO_2 ⟶ H_2O + Ca(NO_2)_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: Ca(OH)_2 + 2 HNO_2 ⟶ 2 H_2O + Ca(NO_2)_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 Ca(OH)_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 Ca(NO_2)_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 Ca(OH)_2 | 1 | -1 | -(Δ[Ca(OH)2])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Ca(NO_2)_2 | 1 | 1 | (Δ[Ca(NO2)2])/(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[Ca(OH)2])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[Ca(NO2)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)