Cu(NO3)2 + K2S = KNO3 + CuS

Cu(NO_3)_2 copper(II) nitrate + K2S ⟶ KNO_3 potassium nitrate + CuS cupric sulfide

Balance the chemical equation algebraically: Cu(NO_3)_2 + K2S ⟶ KNO_3 + CuS Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cu(NO_3)_2 + c_2 K2S ⟶ c_3 KNO_3 + c_4 CuS Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, N, O, K and S: Cu: | c_1 = c_4 N: | 2 c_1 = c_3 O: | 6 c_1 = 3 c_3 K: | 2 c_2 = c_3 S: | c_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 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cu(NO_3)_2 + K2S ⟶ 2 KNO_3 + CuS

+ K2S ⟶ +

copper(II) nitrate + K2S ⟶ potassium nitrate + cupric sulfide

Construct the equilibrium constant, K, expression for: Cu(NO_3)_2 + K2S ⟶ KNO_3 + CuS 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 + K2S ⟶ 2 KNO_3 + CuS 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 K2S | 1 | -1 KNO_3 | 2 | 2 CuS | 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) K2S | 1 | -1 | ([K2S])^(-1) KNO_3 | 2 | 2 | ([KNO3])^2 CuS | 1 | 1 | [CuS] 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) ([K2S])^(-1) ([KNO3])^2 [CuS] = (([KNO3])^2 [CuS])/([Cu(NO3)2] [K2S])

Construct the rate of reaction expression for: Cu(NO_3)_2 + K2S ⟶ KNO_3 + CuS 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 + K2S ⟶ 2 KNO_3 + CuS 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 K2S | 1 | -1 KNO_3 | 2 | 2 CuS | 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) K2S | 1 | -1 | -(Δ[K2S])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) CuS | 1 | 1 | (Δ[CuS])/(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[K2S])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = (Δ[CuS])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| copper(II) nitrate | K2S | potassium nitrate | cupric sulfide formula | Cu(NO_3)_2 | K2S | KNO_3 | CuS Hill formula | CuN_2O_6 | K2S | KNO_3 | CuS name | copper(II) nitrate | | potassium nitrate | cupric sulfide

| copper(II) nitrate | K2S | potassium nitrate | cupric sulfide molar mass | 187.55 g/mol | 110.26 g/mol | 101.1 g/mol | 95.61 g/mol phase | | | solid (at STP) | solid (at STP) melting point | | | 334 °C | 220 °C density | | | | 4.6 g/cm^3 solubility in water | | | soluble | dynamic viscosity | | | | 3.68×10^-5 Pa s (at 1250 °C) odor | | | odorless |