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CrCl3 + NH4OH = NH4Cl + Cr(OH)3

Input interpretation

CrCl_3 chromic chloride + NH_4OH ammonium hydroxide ⟶ NH_4Cl ammonium chloride + Cr(OH)3
CrCl_3 chromic chloride + NH_4OH ammonium hydroxide ⟶ NH_4Cl ammonium chloride + Cr(OH)3

Balanced equation

Balance the chemical equation algebraically: CrCl_3 + NH_4OH ⟶ NH_4Cl + Cr(OH)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CrCl_3 + c_2 NH_4OH ⟶ c_3 NH_4Cl + c_4 Cr(OH)3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Cr, H, N and O: Cl: | 3 c_1 = c_3 Cr: | c_1 = c_4 H: | 5 c_2 = 4 c_3 + 3 c_4 N: | c_2 = c_3 O: | c_2 = 3 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 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CrCl_3 + 3 NH_4OH ⟶ 3 NH_4Cl + Cr(OH)3
Balance the chemical equation algebraically: CrCl_3 + NH_4OH ⟶ NH_4Cl + Cr(OH)3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CrCl_3 + c_2 NH_4OH ⟶ c_3 NH_4Cl + c_4 Cr(OH)3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Cr, H, N and O: Cl: | 3 c_1 = c_3 Cr: | c_1 = c_4 H: | 5 c_2 = 4 c_3 + 3 c_4 N: | c_2 = c_3 O: | c_2 = 3 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 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CrCl_3 + 3 NH_4OH ⟶ 3 NH_4Cl + Cr(OH)3

Structures

+ ⟶ + Cr(OH)3
+ ⟶ + Cr(OH)3

Names

chromic chloride + ammonium hydroxide ⟶ ammonium chloride + Cr(OH)3
chromic chloride + ammonium hydroxide ⟶ ammonium chloride + Cr(OH)3

Equilibrium constant

Construct the equilibrium constant, K, expression for: CrCl_3 + NH_4OH ⟶ NH_4Cl + Cr(OH)3 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: CrCl_3 + 3 NH_4OH ⟶ 3 NH_4Cl + Cr(OH)3 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 CrCl_3 | 1 | -1 NH_4OH | 3 | -3 NH_4Cl | 3 | 3 Cr(OH)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CrCl_3 | 1 | -1 | ([CrCl3])^(-1) NH_4OH | 3 | -3 | ([NH4OH])^(-3) NH_4Cl | 3 | 3 | ([NH4Cl])^3 Cr(OH)3 | 1 | 1 | [Cr(OH)3] 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 = ([CrCl3])^(-1) ([NH4OH])^(-3) ([NH4Cl])^3 [Cr(OH)3] = (([NH4Cl])^3 [Cr(OH)3])/([CrCl3] ([NH4OH])^3)
Construct the equilibrium constant, K, expression for: CrCl_3 + NH_4OH ⟶ NH_4Cl + Cr(OH)3 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: CrCl_3 + 3 NH_4OH ⟶ 3 NH_4Cl + Cr(OH)3 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 CrCl_3 | 1 | -1 NH_4OH | 3 | -3 NH_4Cl | 3 | 3 Cr(OH)3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CrCl_3 | 1 | -1 | ([CrCl3])^(-1) NH_4OH | 3 | -3 | ([NH4OH])^(-3) NH_4Cl | 3 | 3 | ([NH4Cl])^3 Cr(OH)3 | 1 | 1 | [Cr(OH)3] 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 = ([CrCl3])^(-1) ([NH4OH])^(-3) ([NH4Cl])^3 [Cr(OH)3] = (([NH4Cl])^3 [Cr(OH)3])/([CrCl3] ([NH4OH])^3)

Rate of reaction

Construct the rate of reaction expression for: CrCl_3 + NH_4OH ⟶ NH_4Cl + Cr(OH)3 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: CrCl_3 + 3 NH_4OH ⟶ 3 NH_4Cl + Cr(OH)3 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 CrCl_3 | 1 | -1 NH_4OH | 3 | -3 NH_4Cl | 3 | 3 Cr(OH)3 | 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 CrCl_3 | 1 | -1 | -(Δ[CrCl3])/(Δt) NH_4OH | 3 | -3 | -1/3 (Δ[NH4OH])/(Δt) NH_4Cl | 3 | 3 | 1/3 (Δ[NH4Cl])/(Δt) Cr(OH)3 | 1 | 1 | (Δ[Cr(OH)3])/(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[CrCl3])/(Δt) = -1/3 (Δ[NH4OH])/(Δt) = 1/3 (Δ[NH4Cl])/(Δt) = (Δ[Cr(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CrCl_3 + NH_4OH ⟶ NH_4Cl + Cr(OH)3 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: CrCl_3 + 3 NH_4OH ⟶ 3 NH_4Cl + Cr(OH)3 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 CrCl_3 | 1 | -1 NH_4OH | 3 | -3 NH_4Cl | 3 | 3 Cr(OH)3 | 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 CrCl_3 | 1 | -1 | -(Δ[CrCl3])/(Δt) NH_4OH | 3 | -3 | -1/3 (Δ[NH4OH])/(Δt) NH_4Cl | 3 | 3 | 1/3 (Δ[NH4Cl])/(Δt) Cr(OH)3 | 1 | 1 | (Δ[Cr(OH)3])/(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[CrCl3])/(Δt) = -1/3 (Δ[NH4OH])/(Δt) = 1/3 (Δ[NH4Cl])/(Δt) = (Δ[Cr(OH)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chromic chloride | ammonium hydroxide | ammonium chloride | Cr(OH)3 formula | CrCl_3 | NH_4OH | NH_4Cl | Cr(OH)3 Hill formula | Cl_3Cr | H_5NO | ClH_4N | H3CrO3 name | chromic chloride | ammonium hydroxide | ammonium chloride | IUPAC name | trichlorochromium | ammonium hydroxide | ammonium chloride |
| chromic chloride | ammonium hydroxide | ammonium chloride | Cr(OH)3 formula | CrCl_3 | NH_4OH | NH_4Cl | Cr(OH)3 Hill formula | Cl_3Cr | H_5NO | ClH_4N | H3CrO3 name | chromic chloride | ammonium hydroxide | ammonium chloride | IUPAC name | trichlorochromium | ammonium hydroxide | ammonium chloride |

Substance properties

| chromic chloride | ammonium hydroxide | ammonium chloride | Cr(OH)3 molar mass | 158.3 g/mol | 35.046 g/mol | 53.49 g/mol | 103.02 g/mol phase | solid (at STP) | aqueous (at STP) | solid (at STP) | melting point | 1152 °C | -57.5 °C | 340 °C | boiling point | | 36 °C | | density | 2.87 g/cm^3 | 0.9 g/cm^3 | 1.5256 g/cm^3 | solubility in water | slightly soluble | very soluble | soluble |
| chromic chloride | ammonium hydroxide | ammonium chloride | Cr(OH)3 molar mass | 158.3 g/mol | 35.046 g/mol | 53.49 g/mol | 103.02 g/mol phase | solid (at STP) | aqueous (at STP) | solid (at STP) | melting point | 1152 °C | -57.5 °C | 340 °C | boiling point | | 36 °C | | density | 2.87 g/cm^3 | 0.9 g/cm^3 | 1.5256 g/cm^3 | solubility in water | slightly soluble | very soluble | soluble |

Units

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