Search

Cl2 + NH4OH = H2O + N2 + NH4Cl

Input interpretation

Cl_2 chlorine + NH_4OH ammonium hydroxide ⟶ H_2O water + N_2 nitrogen + NH_4Cl ammonium chloride
Cl_2 chlorine + NH_4OH ammonium hydroxide ⟶ H_2O water + N_2 nitrogen + NH_4Cl ammonium chloride

Balanced equation

Balance the chemical equation algebraically: Cl_2 + NH_4OH ⟶ H_2O + N_2 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 NH_4OH ⟶ c_3 H_2O + c_4 N_2 + c_5 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | 2 c_1 = c_5 H: | 5 c_2 = 2 c_3 + 4 c_5 N: | c_2 = 2 c_4 + c_5 O: | 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 8 c_3 = 8 c_4 = 1 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Cl_2 + 8 NH_4OH ⟶ 8 H_2O + N_2 + 6 NH_4Cl
Balance the chemical equation algebraically: Cl_2 + NH_4OH ⟶ H_2O + N_2 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 NH_4OH ⟶ c_3 H_2O + c_4 N_2 + c_5 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N and O: Cl: | 2 c_1 = c_5 H: | 5 c_2 = 2 c_3 + 4 c_5 N: | c_2 = 2 c_4 + c_5 O: | 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 8 c_3 = 8 c_4 = 1 c_5 = 6 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Cl_2 + 8 NH_4OH ⟶ 8 H_2O + N_2 + 6 NH_4Cl

Structures

+ ⟶ + +
+ ⟶ + +

Names

chlorine + ammonium hydroxide ⟶ water + nitrogen + ammonium chloride
chlorine + ammonium hydroxide ⟶ water + nitrogen + ammonium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: Cl_2 + NH_4OH ⟶ H_2O + N_2 + NH_4Cl 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: 3 Cl_2 + 8 NH_4OH ⟶ 8 H_2O + N_2 + 6 NH_4Cl 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 | 3 | -3 NH_4OH | 8 | -8 H_2O | 8 | 8 N_2 | 1 | 1 NH_4Cl | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 3 | -3 | ([Cl2])^(-3) NH_4OH | 8 | -8 | ([NH4OH])^(-8) H_2O | 8 | 8 | ([H2O])^8 N_2 | 1 | 1 | [N2] NH_4Cl | 6 | 6 | ([NH4Cl])^6 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])^(-3) ([NH4OH])^(-8) ([H2O])^8 [N2] ([NH4Cl])^6 = (([H2O])^8 [N2] ([NH4Cl])^6)/(([Cl2])^3 ([NH4OH])^8)
Construct the equilibrium constant, K, expression for: Cl_2 + NH_4OH ⟶ H_2O + N_2 + NH_4Cl 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: 3 Cl_2 + 8 NH_4OH ⟶ 8 H_2O + N_2 + 6 NH_4Cl 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 | 3 | -3 NH_4OH | 8 | -8 H_2O | 8 | 8 N_2 | 1 | 1 NH_4Cl | 6 | 6 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 3 | -3 | ([Cl2])^(-3) NH_4OH | 8 | -8 | ([NH4OH])^(-8) H_2O | 8 | 8 | ([H2O])^8 N_2 | 1 | 1 | [N2] NH_4Cl | 6 | 6 | ([NH4Cl])^6 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])^(-3) ([NH4OH])^(-8) ([H2O])^8 [N2] ([NH4Cl])^6 = (([H2O])^8 [N2] ([NH4Cl])^6)/(([Cl2])^3 ([NH4OH])^8)

Rate of reaction

Construct the rate of reaction expression for: Cl_2 + NH_4OH ⟶ H_2O + N_2 + NH_4Cl 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: 3 Cl_2 + 8 NH_4OH ⟶ 8 H_2O + N_2 + 6 NH_4Cl 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 | 3 | -3 NH_4OH | 8 | -8 H_2O | 8 | 8 N_2 | 1 | 1 NH_4Cl | 6 | 6 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 | 3 | -3 | -1/3 (Δ[Cl2])/(Δt) NH_4OH | 8 | -8 | -1/8 (Δ[NH4OH])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(Δt) NH_4Cl | 6 | 6 | 1/6 (Δ[NH4Cl])/(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 = -1/3 (Δ[Cl2])/(Δt) = -1/8 (Δ[NH4OH])/(Δt) = 1/8 (Δ[H2O])/(Δt) = (Δ[N2])/(Δt) = 1/6 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Cl_2 + NH_4OH ⟶ H_2O + N_2 + NH_4Cl 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: 3 Cl_2 + 8 NH_4OH ⟶ 8 H_2O + N_2 + 6 NH_4Cl 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 | 3 | -3 NH_4OH | 8 | -8 H_2O | 8 | 8 N_2 | 1 | 1 NH_4Cl | 6 | 6 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 | 3 | -3 | -1/3 (Δ[Cl2])/(Δt) NH_4OH | 8 | -8 | -1/8 (Δ[NH4OH])/(Δt) H_2O | 8 | 8 | 1/8 (Δ[H2O])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(Δt) NH_4Cl | 6 | 6 | 1/6 (Δ[NH4Cl])/(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 = -1/3 (Δ[Cl2])/(Δt) = -1/8 (Δ[NH4OH])/(Δt) = 1/8 (Δ[H2O])/(Δt) = (Δ[N2])/(Δt) = 1/6 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| chlorine | ammonium hydroxide | water | nitrogen | ammonium chloride formula | Cl_2 | NH_4OH | H_2O | N_2 | NH_4Cl Hill formula | Cl_2 | H_5NO | H_2O | N_2 | ClH_4N name | chlorine | ammonium hydroxide | water | nitrogen | ammonium chloride IUPAC name | molecular chlorine | ammonium hydroxide | water | molecular nitrogen | ammonium chloride
| chlorine | ammonium hydroxide | water | nitrogen | ammonium chloride formula | Cl_2 | NH_4OH | H_2O | N_2 | NH_4Cl Hill formula | Cl_2 | H_5NO | H_2O | N_2 | ClH_4N name | chlorine | ammonium hydroxide | water | nitrogen | ammonium chloride IUPAC name | molecular chlorine | ammonium hydroxide | water | molecular nitrogen | ammonium chloride

Substance properties

| chlorine | ammonium hydroxide | water | nitrogen | ammonium chloride molar mass | 70.9 g/mol | 35.046 g/mol | 18.015 g/mol | 28.014 g/mol | 53.49 g/mol phase | gas (at STP) | aqueous (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -101 °C | -57.5 °C | 0 °C | -210 °C | 340 °C boiling point | -34 °C | 36 °C | 99.9839 °C | -195.79 °C | density | 0.003214 g/cm^3 (at 0 °C) | 0.9 g/cm^3 | 1 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) | 1.5256 g/cm^3 solubility in water | | very soluble | | insoluble | soluble surface tension | | | 0.0728 N/m | 0.0066 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 1.78×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |
| chlorine | ammonium hydroxide | water | nitrogen | ammonium chloride molar mass | 70.9 g/mol | 35.046 g/mol | 18.015 g/mol | 28.014 g/mol | 53.49 g/mol phase | gas (at STP) | aqueous (at STP) | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -101 °C | -57.5 °C | 0 °C | -210 °C | 340 °C boiling point | -34 °C | 36 °C | 99.9839 °C | -195.79 °C | density | 0.003214 g/cm^3 (at 0 °C) | 0.9 g/cm^3 | 1 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) | 1.5256 g/cm^3 solubility in water | | very soluble | | insoluble | soluble surface tension | | | 0.0728 N/m | 0.0066 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | 1.78×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |

Units

Random Queries

formula of tin(II) cation vs stannite anion
Hill formula of sodium
density of ethanol vs hydrogen bromide
name of lithium-6Li hydroxide monohydrate vs strontium selenate
critical temperature of sulfur
odor of oxygen vs carbon dioxide
chemical types of manganese(II) perchlorate hydrate vs hydrazine-15 N2 monohydrate
name of phosphorus pentachloride
phases of heteronuclear diatomic molecules
half-life of Be-13 vs No-259