Cu(NO3)2 + Ba(OH)2 = Cu(OH)2 + Ba(NO3)2

Input interpretation

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Cu(NO_3)_2 copper(II) nitrate + Ba(OH)_2 barium hydroxide ⟶ Cu(OH)_2 copper hydroxide + Ba(NO_3)_2 barium nitrate

Balanced equation

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Balance the chemical equation algebraically: Cu(NO_3)_2 + Ba(OH)_2 ⟶ Cu(OH)_2 + Ba(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu(NO_3)_2 + c_2 Ba(OH)_2 ⟶ c_3 Cu(OH)_2 + c_4 Ba(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, N, O, Ba and H: Cu: | c_1 = c_3 N: | 2 c_1 = 2 c_4 O: | 6 c_1 + 2 c_2 = 2 c_3 + 6 c_4 Ba: | c_2 = c_4 H: | 2 c_2 = 2 c_3 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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cu(NO_3)_2 + Ba(OH)_2 ⟶ Cu(OH)_2 + Ba(NO_3)_2

+ ⟶ +

Names

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copper(II) nitrate + barium hydroxide ⟶ copper hydroxide + barium nitrate

Equilibrium constant

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Construct the equilibrium constant, K, expression for: Cu(NO_3)_2 + Ba(OH)_2 ⟶ Cu(OH)_2 + Ba(NO_3)_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: Cu(NO_3)_2 + Ba(OH)_2 ⟶ Cu(OH)_2 + Ba(NO_3)_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 Cu(NO_3)_2 | 1 | -1 Ba(OH)_2 | 1 | -1 Cu(OH)_2 | 1 | 1 Ba(NO_3)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cu(NO_3)_2 | 1 | -1 | ([Cu(NO3)2])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) Cu(OH)_2 | 1 | 1 | [Cu(OH)2] Ba(NO_3)_2 | 1 | 1 | [Ba(NO3)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 = ([Cu(NO3)2])^(-1) ([Ba(OH)2])^(-1) [Cu(OH)2] [Ba(NO3)2] = ([Cu(OH)2] [Ba(NO3)2])/([Cu(NO3)2] [Ba(OH)2])

Rate of reaction

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Construct the rate of reaction expression for: Cu(NO_3)_2 + Ba(OH)_2 ⟶ Cu(OH)_2 + Ba(NO_3)_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: Cu(NO_3)_2 + Ba(OH)_2 ⟶ Cu(OH)_2 + Ba(NO_3)_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 Cu(NO_3)_2 | 1 | -1 Ba(OH)_2 | 1 | -1 Cu(OH)_2 | 1 | 1 Ba(NO_3)_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 Cu(NO_3)_2 | 1 | -1 | -(Δ[Cu(NO3)2])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) Cu(OH)_2 | 1 | 1 | (Δ[Cu(OH)2])/(Δt) Ba(NO_3)_2 | 1 | 1 | (Δ[Ba(NO3)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[Cu(NO3)2])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = (Δ[Cu(OH)2])/(Δt) = (Δ[Ba(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)