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CuSO4 + Ba(NO3)2 = Cu(NO3)2 + BaSO4

Input interpretation

CuSO_4 copper(II) sulfate + Ba(NO_3)_2 barium nitrate ⟶ Cu(NO_3)_2 copper(II) nitrate + BaSO_4 barium sulfate
CuSO_4 copper(II) sulfate + Ba(NO_3)_2 barium nitrate ⟶ Cu(NO_3)_2 copper(II) nitrate + BaSO_4 barium sulfate

Balanced equation

Balance the chemical equation algebraically: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuSO_4 + c_2 Ba(NO_3)_2 ⟶ c_3 Cu(NO_3)_2 + c_4 BaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, S, Ba and N: Cu: | c_1 = c_3 O: | 4 c_1 + 6 c_2 = 6 c_3 + 4 c_4 S: | c_1 = c_4 Ba: | c_2 = c_4 N: | 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: | | CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_4
Balance the chemical equation algebraically: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CuSO_4 + c_2 Ba(NO_3)_2 ⟶ c_3 Cu(NO_3)_2 + c_4 BaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, O, S, Ba and N: Cu: | c_1 = c_3 O: | 4 c_1 + 6 c_2 = 6 c_3 + 4 c_4 S: | c_1 = c_4 Ba: | c_2 = c_4 N: | 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: | | CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_4

Structures

+ ⟶ +
+ ⟶ +

Names

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

Equilibrium constant

Construct the equilibrium constant, K, expression for: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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 CuSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 BaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuSO_4 | 1 | -1 | ([CuSO4])^(-1) Ba(NO_3)_2 | 1 | -1 | ([Ba(NO3)2])^(-1) Cu(NO_3)_2 | 1 | 1 | [Cu(NO3)2] BaSO_4 | 1 | 1 | [BaSO4] 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 = ([CuSO4])^(-1) ([Ba(NO3)2])^(-1) [Cu(NO3)2] [BaSO4] = ([Cu(NO3)2] [BaSO4])/([CuSO4] [Ba(NO3)2])
Construct the equilibrium constant, K, expression for: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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 CuSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 BaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CuSO_4 | 1 | -1 | ([CuSO4])^(-1) Ba(NO_3)_2 | 1 | -1 | ([Ba(NO3)2])^(-1) Cu(NO_3)_2 | 1 | 1 | [Cu(NO3)2] BaSO_4 | 1 | 1 | [BaSO4] 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 = ([CuSO4])^(-1) ([Ba(NO3)2])^(-1) [Cu(NO3)2] [BaSO4] = ([Cu(NO3)2] [BaSO4])/([CuSO4] [Ba(NO3)2])

Rate of reaction

Construct the rate of reaction expression for: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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 CuSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 BaSO_4 | 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 CuSO_4 | 1 | -1 | -(Δ[CuSO4])/(Δt) Ba(NO_3)_2 | 1 | -1 | -(Δ[Ba(NO3)2])/(Δt) Cu(NO_3)_2 | 1 | 1 | (Δ[Cu(NO3)2])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(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[CuSO4])/(Δt) = -(Δ[Ba(NO3)2])/(Δt) = (Δ[Cu(NO3)2])/(Δt) = (Δ[BaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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: CuSO_4 + Ba(NO_3)_2 ⟶ Cu(NO_3)_2 + BaSO_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 CuSO_4 | 1 | -1 Ba(NO_3)_2 | 1 | -1 Cu(NO_3)_2 | 1 | 1 BaSO_4 | 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 CuSO_4 | 1 | -1 | -(Δ[CuSO4])/(Δt) Ba(NO_3)_2 | 1 | -1 | -(Δ[Ba(NO3)2])/(Δt) Cu(NO_3)_2 | 1 | 1 | (Δ[Cu(NO3)2])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(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[CuSO4])/(Δt) = -(Δ[Ba(NO3)2])/(Δt) = (Δ[Cu(NO3)2])/(Δt) = (Δ[BaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| copper(II) sulfate | barium nitrate | copper(II) nitrate | barium sulfate formula | CuSO_4 | Ba(NO_3)_2 | Cu(NO_3)_2 | BaSO_4 Hill formula | CuO_4S | BaN_2O_6 | CuN_2O_6 | BaO_4S name | copper(II) sulfate | barium nitrate | copper(II) nitrate | barium sulfate IUPAC name | copper sulfate | barium(+2) cation dinitrate | copper(II) nitrate | barium(+2) cation sulfate
| copper(II) sulfate | barium nitrate | copper(II) nitrate | barium sulfate formula | CuSO_4 | Ba(NO_3)_2 | Cu(NO_3)_2 | BaSO_4 Hill formula | CuO_4S | BaN_2O_6 | CuN_2O_6 | BaO_4S name | copper(II) sulfate | barium nitrate | copper(II) nitrate | barium sulfate IUPAC name | copper sulfate | barium(+2) cation dinitrate | copper(II) nitrate | barium(+2) cation sulfate

Substance properties

| copper(II) sulfate | barium nitrate | copper(II) nitrate | barium sulfate molar mass | 159.6 g/mol | 261.34 g/mol | 187.55 g/mol | 233.38 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 200 °C | 592 °C | | 1345 °C density | 3.603 g/cm^3 | 3.23 g/cm^3 | | 4.5 g/cm^3 solubility in water | | | | insoluble
| copper(II) sulfate | barium nitrate | copper(II) nitrate | barium sulfate molar mass | 159.6 g/mol | 261.34 g/mol | 187.55 g/mol | 233.38 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 200 °C | 592 °C | | 1345 °C density | 3.603 g/cm^3 | 3.23 g/cm^3 | | 4.5 g/cm^3 solubility in water | | | | insoluble

Units

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