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NaOH + AgNO3 + Na2SnO2 = H2O + NaNO3 + Ag + Na2SnO3

Input interpretation

NaOH sodium hydroxide + AgNO_3 silver nitrate + Na2SnO2 ⟶ H_2O water + NaNO_3 sodium nitrate + Ag silver + Na_2SnO_3 sodium stannate
NaOH sodium hydroxide + AgNO_3 silver nitrate + Na2SnO2 ⟶ H_2O water + NaNO_3 sodium nitrate + Ag silver + Na_2SnO_3 sodium stannate

Balanced equation

Balance the chemical equation algebraically: NaOH + AgNO_3 + Na2SnO2 ⟶ H_2O + NaNO_3 + Ag + Na_2SnO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 AgNO_3 + c_3 Na2SnO2 ⟶ c_4 H_2O + c_5 NaNO_3 + c_6 Ag + c_7 Na_2SnO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Ag, N and Sn: H: | c_1 = 2 c_4 Na: | c_1 + 2 c_3 = c_5 + 2 c_7 O: | c_1 + 3 c_2 + 2 c_3 = c_4 + 3 c_5 + 3 c_7 Ag: | c_2 = c_6 N: | c_2 = c_5 Sn: | c_3 = c_7 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 2 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + 2 AgNO_3 + Na2SnO2 ⟶ H_2O + 2 NaNO_3 + 2 Ag + Na_2SnO_3
Balance the chemical equation algebraically: NaOH + AgNO_3 + Na2SnO2 ⟶ H_2O + NaNO_3 + Ag + Na_2SnO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 AgNO_3 + c_3 Na2SnO2 ⟶ c_4 H_2O + c_5 NaNO_3 + c_6 Ag + c_7 Na_2SnO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Ag, N and Sn: H: | c_1 = 2 c_4 Na: | c_1 + 2 c_3 = c_5 + 2 c_7 O: | c_1 + 3 c_2 + 2 c_3 = c_4 + 3 c_5 + 3 c_7 Ag: | c_2 = c_6 N: | c_2 = c_5 Sn: | c_3 = c_7 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 1 c_5 = 2 c_6 = 2 c_7 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + 2 AgNO_3 + Na2SnO2 ⟶ H_2O + 2 NaNO_3 + 2 Ag + Na_2SnO_3

Structures

+ + Na2SnO2 ⟶ + + +
+ + Na2SnO2 ⟶ + + +

Names

sodium hydroxide + silver nitrate + Na2SnO2 ⟶ water + sodium nitrate + silver + sodium stannate
sodium hydroxide + silver nitrate + Na2SnO2 ⟶ water + sodium nitrate + silver + sodium stannate

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + AgNO_3 + Na2SnO2 ⟶ H_2O + NaNO_3 + Ag + Na_2SnO_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: 2 NaOH + 2 AgNO_3 + Na2SnO2 ⟶ H_2O + 2 NaNO_3 + 2 Ag + Na_2SnO_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 NaOH | 2 | -2 AgNO_3 | 2 | -2 Na2SnO2 | 1 | -1 H_2O | 1 | 1 NaNO_3 | 2 | 2 Ag | 2 | 2 Na_2SnO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) AgNO_3 | 2 | -2 | ([AgNO3])^(-2) Na2SnO2 | 1 | -1 | ([Na2SnO2])^(-1) H_2O | 1 | 1 | [H2O] NaNO_3 | 2 | 2 | ([NaNO3])^2 Ag | 2 | 2 | ([Ag])^2 Na_2SnO_3 | 1 | 1 | [Na2SnO3] 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 = ([NaOH])^(-2) ([AgNO3])^(-2) ([Na2SnO2])^(-1) [H2O] ([NaNO3])^2 ([Ag])^2 [Na2SnO3] = ([H2O] ([NaNO3])^2 ([Ag])^2 [Na2SnO3])/(([NaOH])^2 ([AgNO3])^2 [Na2SnO2])
Construct the equilibrium constant, K, expression for: NaOH + AgNO_3 + Na2SnO2 ⟶ H_2O + NaNO_3 + Ag + Na_2SnO_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: 2 NaOH + 2 AgNO_3 + Na2SnO2 ⟶ H_2O + 2 NaNO_3 + 2 Ag + Na_2SnO_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 NaOH | 2 | -2 AgNO_3 | 2 | -2 Na2SnO2 | 1 | -1 H_2O | 1 | 1 NaNO_3 | 2 | 2 Ag | 2 | 2 Na_2SnO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) AgNO_3 | 2 | -2 | ([AgNO3])^(-2) Na2SnO2 | 1 | -1 | ([Na2SnO2])^(-1) H_2O | 1 | 1 | [H2O] NaNO_3 | 2 | 2 | ([NaNO3])^2 Ag | 2 | 2 | ([Ag])^2 Na_2SnO_3 | 1 | 1 | [Na2SnO3] 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 = ([NaOH])^(-2) ([AgNO3])^(-2) ([Na2SnO2])^(-1) [H2O] ([NaNO3])^2 ([Ag])^2 [Na2SnO3] = ([H2O] ([NaNO3])^2 ([Ag])^2 [Na2SnO3])/(([NaOH])^2 ([AgNO3])^2 [Na2SnO2])

Rate of reaction

Construct the rate of reaction expression for: NaOH + AgNO_3 + Na2SnO2 ⟶ H_2O + NaNO_3 + Ag + Na_2SnO_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: 2 NaOH + 2 AgNO_3 + Na2SnO2 ⟶ H_2O + 2 NaNO_3 + 2 Ag + Na_2SnO_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 NaOH | 2 | -2 AgNO_3 | 2 | -2 Na2SnO2 | 1 | -1 H_2O | 1 | 1 NaNO_3 | 2 | 2 Ag | 2 | 2 Na_2SnO_3 | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) Na2SnO2 | 1 | -1 | -(Δ[Na2SnO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(Δt) Na_2SnO_3 | 1 | 1 | (Δ[Na2SnO3])/(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[NaOH])/(Δt) = -1/2 (Δ[AgNO3])/(Δt) = -(Δ[Na2SnO2])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[Na2SnO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + AgNO_3 + Na2SnO2 ⟶ H_2O + NaNO_3 + Ag + Na_2SnO_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: 2 NaOH + 2 AgNO_3 + Na2SnO2 ⟶ H_2O + 2 NaNO_3 + 2 Ag + Na_2SnO_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 NaOH | 2 | -2 AgNO_3 | 2 | -2 Na2SnO2 | 1 | -1 H_2O | 1 | 1 NaNO_3 | 2 | 2 Ag | 2 | 2 Na_2SnO_3 | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) Na2SnO2 | 1 | -1 | -(Δ[Na2SnO2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(Δt) Na_2SnO_3 | 1 | 1 | (Δ[Na2SnO3])/(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[NaOH])/(Δt) = -1/2 (Δ[AgNO3])/(Δt) = -(Δ[Na2SnO2])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = 1/2 (Δ[Ag])/(Δt) = (Δ[Na2SnO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | silver nitrate | Na2SnO2 | water | sodium nitrate | silver | sodium stannate formula | NaOH | AgNO_3 | Na2SnO2 | H_2O | NaNO_3 | Ag | Na_2SnO_3 Hill formula | HNaO | AgNO_3 | Na2O2Sn | H_2O | NNaO_3 | Ag | Na_2O_3Sn name | sodium hydroxide | silver nitrate | | water | sodium nitrate | silver | sodium stannate IUPAC name | sodium hydroxide | silver nitrate | | water | sodium nitrate | silver | disodium dioxido-oxo-tin
| sodium hydroxide | silver nitrate | Na2SnO2 | water | sodium nitrate | silver | sodium stannate formula | NaOH | AgNO_3 | Na2SnO2 | H_2O | NaNO_3 | Ag | Na_2SnO_3 Hill formula | HNaO | AgNO_3 | Na2O2Sn | H_2O | NNaO_3 | Ag | Na_2O_3Sn name | sodium hydroxide | silver nitrate | | water | sodium nitrate | silver | sodium stannate IUPAC name | sodium hydroxide | silver nitrate | | water | sodium nitrate | silver | disodium dioxido-oxo-tin

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