Input interpretation
![NH_3 ammonia + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4](../image_source/f00ddcf99240db287a0431ad42f9bb06.png)
NH_3 ammonia + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4
Balanced equation
![Balance the chemical equation algebraically: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 Cu(H2O)6SO4 ⟶ c_3 CuNH3(H2O)6SO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, Cu, O and S: H: | 3 c_1 + 12 c_2 = 15 c_3 N: | c_1 = c_3 Cu: | c_2 = c_3 O: | 10 c_2 = 10 c_3 S: | c_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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4](../image_source/d4229987d6061b5344e5d396c1be1d1c.png)
Balance the chemical equation algebraically: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 Cu(H2O)6SO4 ⟶ c_3 CuNH3(H2O)6SO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, Cu, O and S: H: | 3 c_1 + 12 c_2 = 15 c_3 N: | c_1 = c_3 Cu: | c_2 = c_3 O: | 10 c_2 = 10 c_3 S: | c_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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4
Structures
![+ Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4](../image_source/bb3aa69fe15dc5ea2aac0bf4bb52e1f7.png)
+ Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4
Names
![ammonia + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4](../image_source/5fe354394d4bb2430d8ed5e1241a4faa.png)
ammonia + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4
Equilibrium constant
![Construct the equilibrium constant, K, expression for: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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 NH_3 | 1 | -1 Cu(H2O)6SO4 | 1 | -1 CuNH3(H2O)6SO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 1 | -1 | ([NH3])^(-1) Cu(H2O)6SO4 | 1 | -1 | ([Cu(H2O)6SO4])^(-1) CuNH3(H2O)6SO4 | 1 | 1 | [CuNH3(H2O)6SO4] 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 = ([NH3])^(-1) ([Cu(H2O)6SO4])^(-1) [CuNH3(H2O)6SO4] = ([CuNH3(H2O)6SO4])/([NH3] [Cu(H2O)6SO4])](../image_source/8c31c640c7891046debf40b52248b36c.png)
Construct the equilibrium constant, K, expression for: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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 NH_3 | 1 | -1 Cu(H2O)6SO4 | 1 | -1 CuNH3(H2O)6SO4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 1 | -1 | ([NH3])^(-1) Cu(H2O)6SO4 | 1 | -1 | ([Cu(H2O)6SO4])^(-1) CuNH3(H2O)6SO4 | 1 | 1 | [CuNH3(H2O)6SO4] 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 = ([NH3])^(-1) ([Cu(H2O)6SO4])^(-1) [CuNH3(H2O)6SO4] = ([CuNH3(H2O)6SO4])/([NH3] [Cu(H2O)6SO4])
Rate of reaction
![Construct the rate of reaction expression for: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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 NH_3 | 1 | -1 Cu(H2O)6SO4 | 1 | -1 CuNH3(H2O)6SO4 | 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 NH_3 | 1 | -1 | -(Δ[NH3])/(Δt) Cu(H2O)6SO4 | 1 | -1 | -(Δ[Cu(H2O)6SO4])/(Δt) CuNH3(H2O)6SO4 | 1 | 1 | (Δ[CuNH3(H2O)6SO4])/(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[NH3])/(Δt) = -(Δ[Cu(H2O)6SO4])/(Δt) = (Δ[CuNH3(H2O)6SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/ae1f396d4575fed4e5f951e44b4b6cd2.png)
Construct the rate of reaction expression for: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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: NH_3 + Cu(H2O)6SO4 ⟶ CuNH3(H2O)6SO4 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 NH_3 | 1 | -1 Cu(H2O)6SO4 | 1 | -1 CuNH3(H2O)6SO4 | 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 NH_3 | 1 | -1 | -(Δ[NH3])/(Δt) Cu(H2O)6SO4 | 1 | -1 | -(Δ[Cu(H2O)6SO4])/(Δt) CuNH3(H2O)6SO4 | 1 | 1 | (Δ[CuNH3(H2O)6SO4])/(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[NH3])/(Δt) = -(Δ[Cu(H2O)6SO4])/(Δt) = (Δ[CuNH3(H2O)6SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| ammonia | Cu(H2O)6SO4 | CuNH3(H2O)6SO4 formula | NH_3 | Cu(H2O)6SO4 | CuNH3(H2O)6SO4 Hill formula | H_3N | H12CuO10S | H15CuNO10S name | ammonia | |](../image_source/c16d23daecb6656892ece2dae69c6f8f.png)
| ammonia | Cu(H2O)6SO4 | CuNH3(H2O)6SO4 formula | NH_3 | Cu(H2O)6SO4 | CuNH3(H2O)6SO4 Hill formula | H_3N | H12CuO10S | H15CuNO10S name | ammonia | |
Substance properties
![| ammonia | Cu(H2O)6SO4 | CuNH3(H2O)6SO4 molar mass | 17.031 g/mol | 267.69 g/mol | 284.72 g/mol phase | gas (at STP) | | melting point | -77.73 °C | | boiling point | -33.33 °C | | density | 6.96×10^-4 g/cm^3 (at 25 °C) | | surface tension | 0.0234 N/m | | dynamic viscosity | 1.009×10^-5 Pa s (at 25 °C) | |](../image_source/15c950691814f2d537146345b7eb15a2.png)
| ammonia | Cu(H2O)6SO4 | CuNH3(H2O)6SO4 molar mass | 17.031 g/mol | 267.69 g/mol | 284.72 g/mol phase | gas (at STP) | | melting point | -77.73 °C | | boiling point | -33.33 °C | | density | 6.96×10^-4 g/cm^3 (at 25 °C) | | surface tension | 0.0234 N/m | | dynamic viscosity | 1.009×10^-5 Pa s (at 25 °C) | |
Units