Search

NH3 + KClO = H2O + KCl + N2

Input interpretation

NH_3 (ammonia) + KClO ⟶ H_2O (water) + KCl (potassium chloride) + N_2 (nitrogen)
NH_3 (ammonia) + KClO ⟶ H_2O (water) + KCl (potassium chloride) + N_2 (nitrogen)

Balanced equation

Balance the chemical equation algebraically: NH_3 + KClO ⟶ H_2O + KCl + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 KClO ⟶ c_3 H_2O + c_4 KCl + c_5 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, K, Cl and O: H: | 3 c_1 = 2 c_3 N: | c_1 = 2 c_5 K: | c_2 = c_4 Cl: | c_2 = c_4 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 3 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NH_3 + 3 KClO ⟶ 3 H_2O + 3 KCl + N_2
Balance the chemical equation algebraically: NH_3 + KClO ⟶ H_2O + KCl + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 KClO ⟶ c_3 H_2O + c_4 KCl + c_5 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, K, Cl and O: H: | 3 c_1 = 2 c_3 N: | c_1 = 2 c_5 K: | c_2 = c_4 Cl: | c_2 = c_4 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 3 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NH_3 + 3 KClO ⟶ 3 H_2O + 3 KCl + N_2

Structures

+ KClO ⟶ + +
+ KClO ⟶ + +

Names

ammonia + KClO ⟶ water + potassium chloride + nitrogen
ammonia + KClO ⟶ water + potassium chloride + nitrogen

Equilibrium constant

Construct the equilibrium constant, K, expression for: NH_3 + KClO ⟶ H_2O + KCl + 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: 2 NH_3 + 3 KClO ⟶ 3 H_2O + 3 KCl + 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 NH_3 | 2 | -2 KClO | 3 | -3 H_2O | 3 | 3 KCl | 3 | 3 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 NH_3 | 2 | -2 | ([NH3])^(-2) KClO | 3 | -3 | ([KClO])^(-3) H_2O | 3 | 3 | ([H2O])^3 KCl | 3 | 3 | ([KCl])^3 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 = ([NH3])^(-2) ([KClO])^(-3) ([H2O])^3 ([KCl])^3 [N2] = (([H2O])^3 ([KCl])^3 [N2])/(([NH3])^2 ([KClO])^3)
Construct the equilibrium constant, K, expression for: NH_3 + KClO ⟶ H_2O + KCl + 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: 2 NH_3 + 3 KClO ⟶ 3 H_2O + 3 KCl + 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 NH_3 | 2 | -2 KClO | 3 | -3 H_2O | 3 | 3 KCl | 3 | 3 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 NH_3 | 2 | -2 | ([NH3])^(-2) KClO | 3 | -3 | ([KClO])^(-3) H_2O | 3 | 3 | ([H2O])^3 KCl | 3 | 3 | ([KCl])^3 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 = ([NH3])^(-2) ([KClO])^(-3) ([H2O])^3 ([KCl])^3 [N2] = (([H2O])^3 ([KCl])^3 [N2])/(([NH3])^2 ([KClO])^3)

Rate of reaction

Construct the rate of reaction expression for: NH_3 + KClO ⟶ H_2O + KCl + 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: 2 NH_3 + 3 KClO ⟶ 3 H_2O + 3 KCl + 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 NH_3 | 2 | -2 KClO | 3 | -3 H_2O | 3 | 3 KCl | 3 | 3 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 NH_3 | 2 | -2 | -1/2 (Δ[NH3])/(Δt) KClO | 3 | -3 | -1/3 (Δ[KClO])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) KCl | 3 | 3 | 1/3 (Δ[KCl])/(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 = -1/2 (Δ[NH3])/(Δt) = -1/3 (Δ[KClO])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[KCl])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NH_3 + KClO ⟶ H_2O + KCl + 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: 2 NH_3 + 3 KClO ⟶ 3 H_2O + 3 KCl + 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 NH_3 | 2 | -2 KClO | 3 | -3 H_2O | 3 | 3 KCl | 3 | 3 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 NH_3 | 2 | -2 | -1/2 (Δ[NH3])/(Δt) KClO | 3 | -3 | -1/3 (Δ[KClO])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) KCl | 3 | 3 | 1/3 (Δ[KCl])/(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 = -1/2 (Δ[NH3])/(Δt) = -1/3 (Δ[KClO])/(Δt) = 1/3 (Δ[H2O])/(Δt) = 1/3 (Δ[KCl])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| ammonia | KClO | water | potassium chloride | nitrogen formula | NH_3 | KClO | H_2O | KCl | N_2 Hill formula | H_3N | ClKO | H_2O | ClK | N_2 name | ammonia | | water | potassium chloride | nitrogen IUPAC name | ammonia | | water | potassium chloride | molecular nitrogen
| ammonia | KClO | water | potassium chloride | nitrogen formula | NH_3 | KClO | H_2O | KCl | N_2 Hill formula | H_3N | ClKO | H_2O | ClK | N_2 name | ammonia | | water | potassium chloride | nitrogen IUPAC name | ammonia | | water | potassium chloride | molecular nitrogen

Substance properties

| ammonia | KClO | water | potassium chloride | nitrogen molar mass | 17.031 g/mol | 90.55 g/mol | 18.015 g/mol | 74.55 g/mol | 28.014 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) melting point | -77.73 °C | | 0 °C | 770 °C | -210 °C boiling point | -33.33 °C | | 99.9839 °C | 1420 °C | -195.79 °C density | 6.96×10^-4 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 1.98 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | | | | soluble | insoluble surface tension | 0.0234 N/m | | 0.0728 N/m | | 0.0066 N/m dynamic viscosity | 1.009×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | odorless | odorless | odorless
| ammonia | KClO | water | potassium chloride | nitrogen molar mass | 17.031 g/mol | 90.55 g/mol | 18.015 g/mol | 74.55 g/mol | 28.014 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) | gas (at STP) melting point | -77.73 °C | | 0 °C | 770 °C | -210 °C boiling point | -33.33 °C | | 99.9839 °C | 1420 °C | -195.79 °C density | 6.96×10^-4 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 1.98 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | | | | soluble | insoluble surface tension | 0.0234 N/m | | 0.0728 N/m | | 0.0066 N/m dynamic viscosity | 1.009×10^-5 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | odorless | odorless | odorless

Units

Random Queries

alternate names of nickel perchlorate vs zinc hydroxide
NaOH + NaClO4 + NaAsO2 = H2O + NaCl + Na3AsO4
alternate names of uranium tribromide
salinity of saline water vs brackish water
molar mass of polonide(2-) anion
structure diagram of iron(II) cation vs phosphate anion
molar mass of hafnium phosphide vs praseodymium(III) nitrate
molar mass of hexachloroplumbate(IV) anion
refractive indices of kyanite vs taseqite
IUPAC name of aluminum sulfate