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Cl2 + NaOH + NH2OH = H2O + NaCl + N2

Input interpretation

Cl_2 chlorine + NaOH sodium hydroxide + NH_2OH hydroxylamine ⟶ H_2O water + NaCl sodium chloride + N_2 nitrogen
Cl_2 chlorine + NaOH sodium hydroxide + NH_2OH hydroxylamine ⟶ H_2O water + NaCl sodium chloride + N_2 nitrogen

Balanced equation

Balance the chemical equation algebraically: Cl_2 + NaOH + NH_2OH ⟶ H_2O + NaCl + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 NaOH + c_3 NH_2OH ⟶ c_4 H_2O + c_5 NaCl + c_6 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O and N: Cl: | 2 c_1 = c_5 H: | c_2 + 3 c_3 = 2 c_4 Na: | c_2 = c_5 O: | c_2 + c_3 = c_4 N: | c_3 = 2 c_6 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 = 2 c_3 = 2 c_4 = 4 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 2 NaOH + 2 NH_2OH ⟶ 4 H_2O + 2 NaCl + N_2
Balance the chemical equation algebraically: Cl_2 + NaOH + NH_2OH ⟶ H_2O + NaCl + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 NaOH + c_3 NH_2OH ⟶ c_4 H_2O + c_5 NaCl + c_6 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O and N: Cl: | 2 c_1 = c_5 H: | c_2 + 3 c_3 = 2 c_4 Na: | c_2 = c_5 O: | c_2 + c_3 = c_4 N: | c_3 = 2 c_6 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 = 2 c_3 = 2 c_4 = 4 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 2 NaOH + 2 NH_2OH ⟶ 4 H_2O + 2 NaCl + N_2

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

chlorine + sodium hydroxide + hydroxylamine ⟶ water + sodium chloride + nitrogen
chlorine + sodium hydroxide + hydroxylamine ⟶ water + sodium chloride + nitrogen

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + NaOH + NH_2OH ⟶ H_2O + NaCl + N_2 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: Cl_2 + 2 NaOH + 2 NH_2OH ⟶ 4 H_2O + 2 NaCl + N_2 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 Cl_2 | 1 | -1 NaOH | 2 | -2 NH_2OH | 2 | -2 H_2O | 4 | 4 NaCl | 2 | 2 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) NaOH | 2 | -2 | ([NaOH])^(-2) NH_2OH | 2 | -2 | ([NH2OH])^(-2) H_2O | 4 | 4 | ([H2O])^4 NaCl | 2 | 2 | ([NaCl])^2 N_2 | 1 | 1 | [N2] 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 = ([Cl2])^(-1) ([NaOH])^(-2) ([NH2OH])^(-2) ([H2O])^4 ([NaCl])^2 [N2] = (([H2O])^4 ([NaCl])^2 [N2])/([Cl2] ([NaOH])^2 ([NH2OH])^2)
Construct the equilibrium constant, K, expression for: Cl_2 + NaOH + NH_2OH ⟶ H_2O + NaCl + N_2 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: Cl_2 + 2 NaOH + 2 NH_2OH ⟶ 4 H_2O + 2 NaCl + N_2 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 Cl_2 | 1 | -1 NaOH | 2 | -2 NH_2OH | 2 | -2 H_2O | 4 | 4 NaCl | 2 | 2 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) NaOH | 2 | -2 | ([NaOH])^(-2) NH_2OH | 2 | -2 | ([NH2OH])^(-2) H_2O | 4 | 4 | ([H2O])^4 NaCl | 2 | 2 | ([NaCl])^2 N_2 | 1 | 1 | [N2] 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 = ([Cl2])^(-1) ([NaOH])^(-2) ([NH2OH])^(-2) ([H2O])^4 ([NaCl])^2 [N2] = (([H2O])^4 ([NaCl])^2 [N2])/([Cl2] ([NaOH])^2 ([NH2OH])^2)

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + NaOH + NH_2OH ⟶ H_2O + NaCl + N_2 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: Cl_2 + 2 NaOH + 2 NH_2OH ⟶ 4 H_2O + 2 NaCl + N_2 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 Cl_2 | 1 | -1 NaOH | 2 | -2 NH_2OH | 2 | -2 H_2O | 4 | 4 NaCl | 2 | 2 N_2 | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) NH_2OH | 2 | -2 | -1/2 (Δ[NH2OH])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) NaCl | 2 | 2 | 1/2 (Δ[NaCl])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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[Cl2])/(Δt) = -1/2 (Δ[NaOH])/(Δt) = -1/2 (Δ[NH2OH])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/2 (Δ[NaCl])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + NaOH + NH_2OH ⟶ H_2O + NaCl + N_2 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: Cl_2 + 2 NaOH + 2 NH_2OH ⟶ 4 H_2O + 2 NaCl + N_2 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 Cl_2 | 1 | -1 NaOH | 2 | -2 NH_2OH | 2 | -2 H_2O | 4 | 4 NaCl | 2 | 2 N_2 | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) NH_2OH | 2 | -2 | -1/2 (Δ[NH2OH])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) NaCl | 2 | 2 | 1/2 (Δ[NaCl])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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[Cl2])/(Δt) = -1/2 (Δ[NaOH])/(Δt) = -1/2 (Δ[NH2OH])/(Δt) = 1/4 (Δ[H2O])/(Δt) = 1/2 (Δ[NaCl])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | nitrogen formula | Cl_2 | NaOH | NH_2OH | H_2O | NaCl | N_2 Hill formula | Cl_2 | HNaO | H_3NO | H_2O | ClNa | N_2 name | chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | nitrogen IUPAC name | molecular chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | molecular nitrogen
| chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | nitrogen formula | Cl_2 | NaOH | NH_2OH | H_2O | NaCl | N_2 Hill formula | Cl_2 | HNaO | H_3NO | H_2O | ClNa | N_2 name | chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | nitrogen IUPAC name | molecular chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | molecular nitrogen

Substance properties

| chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | nitrogen molar mass | 70.9 g/mol | 39.997 g/mol | 33.03 g/mol | 18.015 g/mol | 58.44 g/mol | 28.014 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) | gas (at STP) melting point | -101 °C | 323 °C | | 0 °C | 801 °C | -210 °C boiling point | -34 °C | 1390 °C | 100 °C | 99.9839 °C | 1413 °C | -195.79 °C density | 0.003214 g/cm^3 (at 0 °C) | 2.13 g/cm^3 | 1.078 g/cm^3 | 1 g/cm^3 | 2.16 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | | soluble | very soluble | | soluble | insoluble surface tension | | 0.07435 N/m | | 0.0728 N/m | | 0.0066 N/m dynamic viscosity | | 0.004 Pa s (at 350 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | | odorless | odorless | odorless
| chlorine | sodium hydroxide | hydroxylamine | water | sodium chloride | nitrogen molar mass | 70.9 g/mol | 39.997 g/mol | 33.03 g/mol | 18.015 g/mol | 58.44 g/mol | 28.014 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) | gas (at STP) melting point | -101 °C | 323 °C | | 0 °C | 801 °C | -210 °C boiling point | -34 °C | 1390 °C | 100 °C | 99.9839 °C | 1413 °C | -195.79 °C density | 0.003214 g/cm^3 (at 0 °C) | 2.13 g/cm^3 | 1.078 g/cm^3 | 1 g/cm^3 | 2.16 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | | soluble | very soluble | | soluble | insoluble surface tension | | 0.07435 N/m | | 0.0728 N/m | | 0.0066 N/m dynamic viscosity | | 0.004 Pa s (at 350 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | | odorless | odorless | odorless

Units

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