Input interpretation
![H_2SO_4 sulfuric acid + Ni(OH)_2 nickel(II) hydroxide ⟶ H_2O water + NiSO_4 nickel(II) sulfate](../image_source/a7d295ac94dea0ba662708c70db6176e.png)
H_2SO_4 sulfuric acid + Ni(OH)_2 nickel(II) hydroxide ⟶ H_2O water + NiSO_4 nickel(II) sulfate
Balanced equation
![Balance the chemical equation algebraically: H_2SO_4 + Ni(OH)_2 ⟶ H_2O + NiSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Ni(OH)_2 ⟶ c_3 H_2O + c_4 NiSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Ni: H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 S: | c_1 = c_4 Ni: | 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: | | H_2SO_4 + Ni(OH)_2 ⟶ 2 H_2O + NiSO_4](../image_source/850dba750bcc8204d5e0572fd98d7981.png)
Balance the chemical equation algebraically: H_2SO_4 + Ni(OH)_2 ⟶ H_2O + NiSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Ni(OH)_2 ⟶ c_3 H_2O + c_4 NiSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Ni: H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 S: | c_1 = c_4 Ni: | 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: | | H_2SO_4 + Ni(OH)_2 ⟶ 2 H_2O + NiSO_4
Structures
![+ ⟶ +](../image_source/e67632dc827d9551c4eddab435837b3a.png)
+ ⟶ +
Names
![sulfuric acid + nickel(II) hydroxide ⟶ water + nickel(II) sulfate](../image_source/c58ed1954347568cc59e4edac54c629c.png)
sulfuric acid + nickel(II) hydroxide ⟶ water + nickel(II) sulfate
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2SO_4 + Ni(OH)_2 ⟶ H_2O + NiSO_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: H_2SO_4 + Ni(OH)_2 ⟶ 2 H_2O + NiSO_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 H_2SO_4 | 1 | -1 Ni(OH)_2 | 1 | -1 H_2O | 2 | 2 NiSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) Ni(OH)_2 | 1 | -1 | ([Ni(OH)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 NiSO_4 | 1 | 1 | [NiSO4] 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 = ([H2SO4])^(-1) ([Ni(OH)2])^(-1) ([H2O])^2 [NiSO4] = (([H2O])^2 [NiSO4])/([H2SO4] [Ni(OH)2])](../image_source/b89eecb72dedf8bebd01410f8c0636e1.png)
Construct the equilibrium constant, K, expression for: H_2SO_4 + Ni(OH)_2 ⟶ H_2O + NiSO_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: H_2SO_4 + Ni(OH)_2 ⟶ 2 H_2O + NiSO_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 H_2SO_4 | 1 | -1 Ni(OH)_2 | 1 | -1 H_2O | 2 | 2 NiSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) Ni(OH)_2 | 1 | -1 | ([Ni(OH)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 NiSO_4 | 1 | 1 | [NiSO4] 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 = ([H2SO4])^(-1) ([Ni(OH)2])^(-1) ([H2O])^2 [NiSO4] = (([H2O])^2 [NiSO4])/([H2SO4] [Ni(OH)2])
Rate of reaction
![Construct the rate of reaction expression for: H_2SO_4 + Ni(OH)_2 ⟶ H_2O + NiSO_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: H_2SO_4 + Ni(OH)_2 ⟶ 2 H_2O + NiSO_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 H_2SO_4 | 1 | -1 Ni(OH)_2 | 1 | -1 H_2O | 2 | 2 NiSO_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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) Ni(OH)_2 | 1 | -1 | -(Δ[Ni(OH)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NiSO_4 | 1 | 1 | (Δ[NiSO4])/(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[H2SO4])/(Δt) = -(Δ[Ni(OH)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NiSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/7eaadefa724d621946b362dd8a20ae25.png)
Construct the rate of reaction expression for: H_2SO_4 + Ni(OH)_2 ⟶ H_2O + NiSO_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: H_2SO_4 + Ni(OH)_2 ⟶ 2 H_2O + NiSO_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 H_2SO_4 | 1 | -1 Ni(OH)_2 | 1 | -1 H_2O | 2 | 2 NiSO_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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) Ni(OH)_2 | 1 | -1 | -(Δ[Ni(OH)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NiSO_4 | 1 | 1 | (Δ[NiSO4])/(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[H2SO4])/(Δt) = -(Δ[Ni(OH)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[NiSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| sulfuric acid | nickel(II) hydroxide | water | nickel(II) sulfate formula | H_2SO_4 | Ni(OH)_2 | H_2O | NiSO_4 Hill formula | H_2O_4S | H_2NiO_2 | H_2O | NiO_4S name | sulfuric acid | nickel(II) hydroxide | water | nickel(II) sulfate IUPAC name | sulfuric acid | | water | nickelous sulfate](../image_source/f91911a8795a206fcd3a3e82b0dbdf9f.png)
| sulfuric acid | nickel(II) hydroxide | water | nickel(II) sulfate formula | H_2SO_4 | Ni(OH)_2 | H_2O | NiSO_4 Hill formula | H_2O_4S | H_2NiO_2 | H_2O | NiO_4S name | sulfuric acid | nickel(II) hydroxide | water | nickel(II) sulfate IUPAC name | sulfuric acid | | water | nickelous sulfate
Substance properties
![| sulfuric acid | nickel(II) hydroxide | water | nickel(II) sulfate molar mass | 98.07 g/mol | 92.707 g/mol | 18.015 g/mol | 154.75 g/mol phase | liquid (at STP) | | liquid (at STP) | solid (at STP) melting point | 10.371 °C | | 0 °C | boiling point | 279.6 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | | 1 g/cm^3 | 4.01 g/cm^3 solubility in water | very soluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |](../image_source/572d3130a31e2274d4dc3a54c1145fb2.png)
| sulfuric acid | nickel(II) hydroxide | water | nickel(II) sulfate molar mass | 98.07 g/mol | 92.707 g/mol | 18.015 g/mol | 154.75 g/mol phase | liquid (at STP) | | liquid (at STP) | solid (at STP) melting point | 10.371 °C | | 0 °C | boiling point | 279.6 °C | | 99.9839 °C | density | 1.8305 g/cm^3 | | 1 g/cm^3 | 4.01 g/cm^3 solubility in water | very soluble | | | surface tension | 0.0735 N/m | | 0.0728 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |
Units