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Zn + H2NO3 = H2O + Zn(NO3)2 + (NH4)NO3

Input interpretation

Zn zinc + H2NO3 ⟶ H_2O water + Zn(NO3)2 + NH_4NO_3 ammonium nitrate
Zn zinc + H2NO3 ⟶ H_2O water + Zn(NO3)2 + NH_4NO_3 ammonium nitrate

Balanced equation

Balance the chemical equation algebraically: Zn + H2NO3 ⟶ H_2O + Zn(NO3)2 + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 H2NO3 ⟶ c_3 H_2O + c_4 Zn(NO3)2 + c_5 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, H, N and O: Zn: | c_1 = c_4 H: | 2 c_2 = 2 c_3 + 4 c_5 N: | c_2 = 2 c_4 + 2 c_5 O: | 3 c_2 = c_3 + 6 c_4 + 3 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 5 c_3 = 3 c_4 = 3/2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 10 c_3 = 6 c_4 = 3 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Zn + 10 H2NO3 ⟶ 6 H_2O + 3 Zn(NO3)2 + 2 NH_4NO_3
Balance the chemical equation algebraically: Zn + H2NO3 ⟶ H_2O + Zn(NO3)2 + NH_4NO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn + c_2 H2NO3 ⟶ c_3 H_2O + c_4 Zn(NO3)2 + c_5 NH_4NO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, H, N and O: Zn: | c_1 = c_4 H: | 2 c_2 = 2 c_3 + 4 c_5 N: | c_2 = 2 c_4 + 2 c_5 O: | 3 c_2 = c_3 + 6 c_4 + 3 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3/2 c_2 = 5 c_3 = 3 c_4 = 3/2 c_5 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 3 c_2 = 10 c_3 = 6 c_4 = 3 c_5 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 Zn + 10 H2NO3 ⟶ 6 H_2O + 3 Zn(NO3)2 + 2 NH_4NO_3

Structures

+ H2NO3 ⟶ + Zn(NO3)2 +
+ H2NO3 ⟶ + Zn(NO3)2 +

Names

zinc + H2NO3 ⟶ water + Zn(NO3)2 + ammonium nitrate
zinc + H2NO3 ⟶ water + Zn(NO3)2 + ammonium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Zn + H2NO3 ⟶ H_2O + Zn(NO3)2 + NH_4NO_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: 3 Zn + 10 H2NO3 ⟶ 6 H_2O + 3 Zn(NO3)2 + 2 NH_4NO_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 Zn | 3 | -3 H2NO3 | 10 | -10 H_2O | 6 | 6 Zn(NO3)2 | 3 | 3 NH_4NO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn | 3 | -3 | ([Zn])^(-3) H2NO3 | 10 | -10 | ([H2NO3])^(-10) H_2O | 6 | 6 | ([H2O])^6 Zn(NO3)2 | 3 | 3 | ([Zn(NO3)2])^3 NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 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 = ([Zn])^(-3) ([H2NO3])^(-10) ([H2O])^6 ([Zn(NO3)2])^3 ([NH4NO3])^2 = (([H2O])^6 ([Zn(NO3)2])^3 ([NH4NO3])^2)/(([Zn])^3 ([H2NO3])^10)
Construct the equilibrium constant, K, expression for: Zn + H2NO3 ⟶ H_2O + Zn(NO3)2 + NH_4NO_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: 3 Zn + 10 H2NO3 ⟶ 6 H_2O + 3 Zn(NO3)2 + 2 NH_4NO_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 Zn | 3 | -3 H2NO3 | 10 | -10 H_2O | 6 | 6 Zn(NO3)2 | 3 | 3 NH_4NO_3 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn | 3 | -3 | ([Zn])^(-3) H2NO3 | 10 | -10 | ([H2NO3])^(-10) H_2O | 6 | 6 | ([H2O])^6 Zn(NO3)2 | 3 | 3 | ([Zn(NO3)2])^3 NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 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 = ([Zn])^(-3) ([H2NO3])^(-10) ([H2O])^6 ([Zn(NO3)2])^3 ([NH4NO3])^2 = (([H2O])^6 ([Zn(NO3)2])^3 ([NH4NO3])^2)/(([Zn])^3 ([H2NO3])^10)

Rate of reaction

Construct the rate of reaction expression for: Zn + H2NO3 ⟶ H_2O + Zn(NO3)2 + NH_4NO_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: 3 Zn + 10 H2NO3 ⟶ 6 H_2O + 3 Zn(NO3)2 + 2 NH_4NO_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 Zn | 3 | -3 H2NO3 | 10 | -10 H_2O | 6 | 6 Zn(NO3)2 | 3 | 3 NH_4NO_3 | 2 | 2 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 Zn | 3 | -3 | -1/3 (Δ[Zn])/(Δt) H2NO3 | 10 | -10 | -1/10 (Δ[H2NO3])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) Zn(NO3)2 | 3 | 3 | 1/3 (Δ[Zn(NO3)2])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(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[Zn])/(Δt) = -1/10 (Δ[H2NO3])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/3 (Δ[Zn(NO3)2])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Zn + H2NO3 ⟶ H_2O + Zn(NO3)2 + NH_4NO_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: 3 Zn + 10 H2NO3 ⟶ 6 H_2O + 3 Zn(NO3)2 + 2 NH_4NO_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 Zn | 3 | -3 H2NO3 | 10 | -10 H_2O | 6 | 6 Zn(NO3)2 | 3 | 3 NH_4NO_3 | 2 | 2 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 Zn | 3 | -3 | -1/3 (Δ[Zn])/(Δt) H2NO3 | 10 | -10 | -1/10 (Δ[H2NO3])/(Δt) H_2O | 6 | 6 | 1/6 (Δ[H2O])/(Δt) Zn(NO3)2 | 3 | 3 | 1/3 (Δ[Zn(NO3)2])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(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[Zn])/(Δt) = -1/10 (Δ[H2NO3])/(Δt) = 1/6 (Δ[H2O])/(Δt) = 1/3 (Δ[Zn(NO3)2])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| zinc | H2NO3 | water | Zn(NO3)2 | ammonium nitrate formula | Zn | H2NO3 | H_2O | Zn(NO3)2 | NH_4NO_3 Hill formula | Zn | H2NO3 | H_2O | N2O6Zn | H_4N_2O_3 name | zinc | | water | | ammonium nitrate
| zinc | H2NO3 | water | Zn(NO3)2 | ammonium nitrate formula | Zn | H2NO3 | H_2O | Zn(NO3)2 | NH_4NO_3 Hill formula | Zn | H2NO3 | H_2O | N2O6Zn | H_4N_2O_3 name | zinc | | water | | ammonium nitrate

Substance properties

| zinc | H2NO3 | water | Zn(NO3)2 | ammonium nitrate molar mass | 65.38 g/mol | 64.02 g/mol | 18.015 g/mol | 189.4 g/mol | 80.04 g/mol phase | solid (at STP) | | liquid (at STP) | | solid (at STP) melting point | 420 °C | | 0 °C | | 169 °C boiling point | 907 °C | | 99.9839 °C | | 210 °C density | 7.14 g/cm^3 | | 1 g/cm^3 | | 1.73 g/cm^3 solubility in water | insoluble | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | | odorless
| zinc | H2NO3 | water | Zn(NO3)2 | ammonium nitrate molar mass | 65.38 g/mol | 64.02 g/mol | 18.015 g/mol | 189.4 g/mol | 80.04 g/mol phase | solid (at STP) | | liquid (at STP) | | solid (at STP) melting point | 420 °C | | 0 °C | | 169 °C boiling point | 907 °C | | 99.9839 °C | | 210 °C density | 7.14 g/cm^3 | | 1 g/cm^3 | | 1.73 g/cm^3 solubility in water | insoluble | | | | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | | odorless

Units

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