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NH3 + Ca(OCl)2 = H2O + N2 + CaCl2

Input interpretation

NH_3 ammonia + Ca(OCl)2 ⟶ H_2O water + N_2 nitrogen + CaCl_2 calcium chloride
NH_3 ammonia + Ca(OCl)2 ⟶ H_2O water + N_2 nitrogen + CaCl_2 calcium chloride

Balanced equation

Balance the chemical equation algebraically: NH_3 + Ca(OCl)2 ⟶ H_2O + N_2 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 Ca(OCl)2 ⟶ c_3 H_2O + c_4 N_2 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, Ca, O and Cl: H: | 3 c_1 = 2 c_3 N: | c_1 = 2 c_4 Ca: | c_2 = c_5 O: | 2 c_2 = c_3 Cl: | 2 c_2 = 2 c_5 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 = 2 c_2 = 3/2 c_3 = 3 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 4 c_2 = 3 c_3 = 6 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NH_3 + 3 Ca(OCl)2 ⟶ 6 H_2O + 2 N_2 + 3 CaCl_2
Balance the chemical equation algebraically: NH_3 + Ca(OCl)2 ⟶ H_2O + N_2 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_3 + c_2 Ca(OCl)2 ⟶ c_3 H_2O + c_4 N_2 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, Ca, O and Cl: H: | 3 c_1 = 2 c_3 N: | c_1 = 2 c_4 Ca: | c_2 = c_5 O: | 2 c_2 = c_3 Cl: | 2 c_2 = 2 c_5 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 = 2 c_2 = 3/2 c_3 = 3 c_4 = 1 c_5 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 4 c_2 = 3 c_3 = 6 c_4 = 2 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NH_3 + 3 Ca(OCl)2 ⟶ 6 H_2O + 2 N_2 + 3 CaCl_2

Structures

+ Ca(OCl)2 ⟶ + +
+ Ca(OCl)2 ⟶ + +

Names

ammonia + Ca(OCl)2 ⟶ water + nitrogen + calcium chloride
ammonia + Ca(OCl)2 ⟶ water + nitrogen + calcium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: NH_3 + Ca(OCl)2 ⟶ H_2O + N_2 + CaCl_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: 4 NH_3 + 3 Ca(OCl)2 ⟶ 6 H_2O + 2 N_2 + 3 CaCl_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 | 4 | -4 Ca(OCl)2 | 3 | -3 H_2O | 6 | 6 N_2 | 2 | 2 CaCl_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 4 | -4 | ([NH3])^(-4) Ca(OCl)2 | 3 | -3 | ([Ca(OCl)2])^(-3) H_2O | 6 | 6 | ([H2O])^6 N_2 | 2 | 2 | ([N2])^2 CaCl_2 | 3 | 3 | ([CaCl2])^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 = ([NH3])^(-4) ([Ca(OCl)2])^(-3) ([H2O])^6 ([N2])^2 ([CaCl2])^3 = (([H2O])^6 ([N2])^2 ([CaCl2])^3)/(([NH3])^4 ([Ca(OCl)2])^3)
Construct the equilibrium constant, K, expression for: NH_3 + Ca(OCl)2 ⟶ H_2O + N_2 + CaCl_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: 4 NH_3 + 3 Ca(OCl)2 ⟶ 6 H_2O + 2 N_2 + 3 CaCl_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 | 4 | -4 Ca(OCl)2 | 3 | -3 H_2O | 6 | 6 N_2 | 2 | 2 CaCl_2 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH_3 | 4 | -4 | ([NH3])^(-4) Ca(OCl)2 | 3 | -3 | ([Ca(OCl)2])^(-3) H_2O | 6 | 6 | ([H2O])^6 N_2 | 2 | 2 | ([N2])^2 CaCl_2 | 3 | 3 | ([CaCl2])^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 = ([NH3])^(-4) ([Ca(OCl)2])^(-3) ([H2O])^6 ([N2])^2 ([CaCl2])^3 = (([H2O])^6 ([N2])^2 ([CaCl2])^3)/(([NH3])^4 ([Ca(OCl)2])^3)

Rate of reaction

Construct the rate of reaction expression for: NH_3 + Ca(OCl)2 ⟶ H_2O + N_2 + CaCl_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: 4 NH_3 + 3 Ca(OCl)2 ⟶ 6 H_2O + 2 N_2 + 3 CaCl_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 | 4 | -4 Ca(OCl)2 | 3 | -3 H_2O | 6 | 6 N_2 | 2 | 2 CaCl_2 | 3 | 3 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 | 4 | -4 | -1/4 (Δ[NH3])/(Δt) Ca(OCl)2 | 3 | -3 | -1/3 (Δ[Ca(OCl)2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) N_2 | 2 | 2 | 1/2 (Δ[N2])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(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 = -1/4 (Δ[NH3])/(Δt) = -1/3 (Δ[Ca(OCl)2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/2 (Δ[N2])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NH_3 + Ca(OCl)2 ⟶ H_2O + N_2 + CaCl_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: 4 NH_3 + 3 Ca(OCl)2 ⟶ 6 H_2O + 2 N_2 + 3 CaCl_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 | 4 | -4 Ca(OCl)2 | 3 | -3 H_2O | 6 | 6 N_2 | 2 | 2 CaCl_2 | 3 | 3 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 | 4 | -4 | -1/4 (Δ[NH3])/(Δt) Ca(OCl)2 | 3 | -3 | -1/3 (Δ[Ca(OCl)2])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) N_2 | 2 | 2 | 1/2 (Δ[N2])/(Δt) CaCl_2 | 3 | 3 | 1/3 (Δ[CaCl2])/(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 = -1/4 (Δ[NH3])/(Δt) = -1/3 (Δ[Ca(OCl)2])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/2 (Δ[N2])/(Δt) = 1/3 (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| ammonia | Ca(OCl)2 | water | nitrogen | calcium chloride formula | NH_3 | Ca(OCl)2 | H_2O | N_2 | CaCl_2 Hill formula | H_3N | CaCl2O2 | H_2O | N_2 | CaCl_2 name | ammonia | | water | nitrogen | calcium chloride IUPAC name | ammonia | | water | molecular nitrogen | calcium dichloride
| ammonia | Ca(OCl)2 | water | nitrogen | calcium chloride formula | NH_3 | Ca(OCl)2 | H_2O | N_2 | CaCl_2 Hill formula | H_3N | CaCl2O2 | H_2O | N_2 | CaCl_2 name | ammonia | | water | nitrogen | calcium chloride IUPAC name | ammonia | | water | molecular nitrogen | calcium dichloride

Substance properties

| ammonia | Ca(OCl)2 | water | nitrogen | calcium chloride molar mass | 17.031 g/mol | 143 g/mol | 18.015 g/mol | 28.014 g/mol | 111 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -77.73 °C | | 0 °C | -210 °C | 772 °C boiling point | -33.33 °C | | 99.9839 °C | -195.79 °C | density | 6.96×10^-4 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) | 2.15 g/cm^3 solubility in water | | | | insoluble | soluble 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 |
| ammonia | Ca(OCl)2 | water | nitrogen | calcium chloride molar mass | 17.031 g/mol | 143 g/mol | 18.015 g/mol | 28.014 g/mol | 111 g/mol phase | gas (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -77.73 °C | | 0 °C | -210 °C | 772 °C boiling point | -33.33 °C | | 99.9839 °C | -195.79 °C | density | 6.96×10^-4 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) | 2.15 g/cm^3 solubility in water | | | | insoluble | soluble 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 |

Units

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