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KOH + AgNO3 = H2O + KNO3 + Ag2O

Input interpretation

KOH potassium hydroxide + AgNO_3 silver nitrate ⟶ H_2O water + KNO_3 potassium nitrate + Ag_2O silver(I) oxide
KOH potassium hydroxide + AgNO_3 silver nitrate ⟶ H_2O water + KNO_3 potassium nitrate + Ag_2O silver(I) oxide

Balanced equation

Balance the chemical equation algebraically: KOH + AgNO_3 ⟶ H_2O + KNO_3 + Ag_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 AgNO_3 ⟶ c_3 H_2O + c_4 KNO_3 + c_5 Ag_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Ag and N: H: | c_1 = 2 c_3 K: | c_1 = c_4 O: | c_1 + 3 c_2 = c_3 + 3 c_4 + c_5 Ag: | c_2 = 2 c_5 N: | c_2 = c_4 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 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + 2 AgNO_3 ⟶ H_2O + 2 KNO_3 + Ag_2O
Balance the chemical equation algebraically: KOH + AgNO_3 ⟶ H_2O + KNO_3 + Ag_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 AgNO_3 ⟶ c_3 H_2O + c_4 KNO_3 + c_5 Ag_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Ag and N: H: | c_1 = 2 c_3 K: | c_1 = c_4 O: | c_1 + 3 c_2 = c_3 + 3 c_4 + c_5 Ag: | c_2 = 2 c_5 N: | c_2 = c_4 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 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + 2 AgNO_3 ⟶ H_2O + 2 KNO_3 + Ag_2O

Structures

+ ⟶ + +
+ ⟶ + +

Names

potassium hydroxide + silver nitrate ⟶ water + potassium nitrate + silver(I) oxide
potassium hydroxide + silver nitrate ⟶ water + potassium nitrate + silver(I) oxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + AgNO_3 ⟶ H_2O + KNO_3 + Ag_2O 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 KOH + 2 AgNO_3 ⟶ H_2O + 2 KNO_3 + Ag_2O 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 KOH | 2 | -2 AgNO_3 | 2 | -2 H_2O | 1 | 1 KNO_3 | 2 | 2 Ag_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) AgNO_3 | 2 | -2 | ([AgNO3])^(-2) H_2O | 1 | 1 | [H2O] KNO_3 | 2 | 2 | ([KNO3])^2 Ag_2O | 1 | 1 | [Ag2O] 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 = ([KOH])^(-2) ([AgNO3])^(-2) [H2O] ([KNO3])^2 [Ag2O] = ([H2O] ([KNO3])^2 [Ag2O])/(([KOH])^2 ([AgNO3])^2)
Construct the equilibrium constant, K, expression for: KOH + AgNO_3 ⟶ H_2O + KNO_3 + Ag_2O 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 KOH + 2 AgNO_3 ⟶ H_2O + 2 KNO_3 + Ag_2O 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 KOH | 2 | -2 AgNO_3 | 2 | -2 H_2O | 1 | 1 KNO_3 | 2 | 2 Ag_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) AgNO_3 | 2 | -2 | ([AgNO3])^(-2) H_2O | 1 | 1 | [H2O] KNO_3 | 2 | 2 | ([KNO3])^2 Ag_2O | 1 | 1 | [Ag2O] 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 = ([KOH])^(-2) ([AgNO3])^(-2) [H2O] ([KNO3])^2 [Ag2O] = ([H2O] ([KNO3])^2 [Ag2O])/(([KOH])^2 ([AgNO3])^2)

Rate of reaction

Construct the rate of reaction expression for: KOH + AgNO_3 ⟶ H_2O + KNO_3 + Ag_2O 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 KOH + 2 AgNO_3 ⟶ H_2O + 2 KNO_3 + Ag_2O 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 KOH | 2 | -2 AgNO_3 | 2 | -2 H_2O | 1 | 1 KNO_3 | 2 | 2 Ag_2O | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) Ag_2O | 1 | 1 | (Δ[Ag2O])/(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[KOH])/(Δt) = -1/2 (Δ[AgNO3])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = (Δ[Ag2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + AgNO_3 ⟶ H_2O + KNO_3 + Ag_2O 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 KOH + 2 AgNO_3 ⟶ H_2O + 2 KNO_3 + Ag_2O 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 KOH | 2 | -2 AgNO_3 | 2 | -2 H_2O | 1 | 1 KNO_3 | 2 | 2 Ag_2O | 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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KNO_3 | 2 | 2 | 1/2 (Δ[KNO3])/(Δt) Ag_2O | 1 | 1 | (Δ[Ag2O])/(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[KOH])/(Δt) = -1/2 (Δ[AgNO3])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[KNO3])/(Δt) = (Δ[Ag2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | silver nitrate | water | potassium nitrate | silver(I) oxide formula | KOH | AgNO_3 | H_2O | KNO_3 | Ag_2O Hill formula | HKO | AgNO_3 | H_2O | KNO_3 | Ag_2O_1 name | potassium hydroxide | silver nitrate | water | potassium nitrate | silver(I) oxide
| potassium hydroxide | silver nitrate | water | potassium nitrate | silver(I) oxide formula | KOH | AgNO_3 | H_2O | KNO_3 | Ag_2O Hill formula | HKO | AgNO_3 | H_2O | KNO_3 | Ag_2O_1 name | potassium hydroxide | silver nitrate | water | potassium nitrate | silver(I) oxide

Substance properties

| potassium hydroxide | silver nitrate | water | potassium nitrate | silver(I) oxide molar mass | 56.105 g/mol | 169.87 g/mol | 18.015 g/mol | 101.1 g/mol | 231.7 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | 212 °C | 0 °C | 334 °C | boiling point | 1327 °C | | 99.9839 °C | | density | 2.044 g/cm^3 | | 1 g/cm^3 | | solubility in water | soluble | soluble | | soluble | surface tension | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | odorless | odorless | odorless |
| potassium hydroxide | silver nitrate | water | potassium nitrate | silver(I) oxide molar mass | 56.105 g/mol | 169.87 g/mol | 18.015 g/mol | 101.1 g/mol | 231.7 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 406 °C | 212 °C | 0 °C | 334 °C | boiling point | 1327 °C | | 99.9839 °C | | density | 2.044 g/cm^3 | | 1 g/cm^3 | | solubility in water | soluble | soluble | | soluble | surface tension | | | 0.0728 N/m | | dynamic viscosity | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | odorless | odorless | odorless |

Units

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