Search

Ag + HClO3 = H2O + AgCl + AgClO3

Input interpretation

Ag silver + HClO3 ⟶ H_2O water + AgCl silver chloride + AgClO_3 silver chlorate
Ag silver + HClO3 ⟶ H_2O water + AgCl silver chloride + AgClO_3 silver chlorate

Balanced equation

Balance the chemical equation algebraically: Ag + HClO3 ⟶ H_2O + AgCl + AgClO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 HClO3 ⟶ c_3 H_2O + c_4 AgCl + c_5 AgClO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, H, Cl and O: Ag: | c_1 = c_4 + c_5 H: | c_2 = 2 c_3 Cl: | c_2 = c_4 + c_5 O: | 3 c_2 = c_3 + 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 3 c_4 = 1 c_5 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Ag + 6 HClO3 ⟶ 3 H_2O + AgCl + 5 AgClO_3
Balance the chemical equation algebraically: Ag + HClO3 ⟶ H_2O + AgCl + AgClO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ag + c_2 HClO3 ⟶ c_3 H_2O + c_4 AgCl + c_5 AgClO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, H, Cl and O: Ag: | c_1 = c_4 + c_5 H: | c_2 = 2 c_3 Cl: | c_2 = c_4 + c_5 O: | 3 c_2 = c_3 + 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 6 c_2 = 6 c_3 = 3 c_4 = 1 c_5 = 5 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 Ag + 6 HClO3 ⟶ 3 H_2O + AgCl + 5 AgClO_3

Structures

+ HClO3 ⟶ + +
+ HClO3 ⟶ + +

Names

silver + HClO3 ⟶ water + silver chloride + silver chlorate
silver + HClO3 ⟶ water + silver chloride + silver chlorate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Ag + HClO3 ⟶ H_2O + AgCl + AgClO_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: 6 Ag + 6 HClO3 ⟶ 3 H_2O + AgCl + 5 AgClO_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 Ag | 6 | -6 HClO3 | 6 | -6 H_2O | 3 | 3 AgCl | 1 | 1 AgClO_3 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag | 6 | -6 | ([Ag])^(-6) HClO3 | 6 | -6 | ([HClO3])^(-6) H_2O | 3 | 3 | ([H2O])^3 AgCl | 1 | 1 | [AgCl] AgClO_3 | 5 | 5 | ([AgClO3])^5 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 = ([Ag])^(-6) ([HClO3])^(-6) ([H2O])^3 [AgCl] ([AgClO3])^5 = (([H2O])^3 [AgCl] ([AgClO3])^5)/(([Ag])^6 ([HClO3])^6)
Construct the equilibrium constant, K, expression for: Ag + HClO3 ⟶ H_2O + AgCl + AgClO_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: 6 Ag + 6 HClO3 ⟶ 3 H_2O + AgCl + 5 AgClO_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 Ag | 6 | -6 HClO3 | 6 | -6 H_2O | 3 | 3 AgCl | 1 | 1 AgClO_3 | 5 | 5 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ag | 6 | -6 | ([Ag])^(-6) HClO3 | 6 | -6 | ([HClO3])^(-6) H_2O | 3 | 3 | ([H2O])^3 AgCl | 1 | 1 | [AgCl] AgClO_3 | 5 | 5 | ([AgClO3])^5 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 = ([Ag])^(-6) ([HClO3])^(-6) ([H2O])^3 [AgCl] ([AgClO3])^5 = (([H2O])^3 [AgCl] ([AgClO3])^5)/(([Ag])^6 ([HClO3])^6)

Rate of reaction

Construct the rate of reaction expression for: Ag + HClO3 ⟶ H_2O + AgCl + AgClO_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: 6 Ag + 6 HClO3 ⟶ 3 H_2O + AgCl + 5 AgClO_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 Ag | 6 | -6 HClO3 | 6 | -6 H_2O | 3 | 3 AgCl | 1 | 1 AgClO_3 | 5 | 5 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 Ag | 6 | -6 | -1/6 (Δ[Ag])/(Δt) HClO3 | 6 | -6 | -1/6 (Δ[HClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) AgCl | 1 | 1 | (Δ[AgCl])/(Δt) AgClO_3 | 5 | 5 | 1/5 (Δ[AgClO3])/(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 = -1/6 (Δ[Ag])/(Δt) = -1/6 (Δ[HClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[AgCl])/(Δt) = 1/5 (Δ[AgClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Ag + HClO3 ⟶ H_2O + AgCl + AgClO_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: 6 Ag + 6 HClO3 ⟶ 3 H_2O + AgCl + 5 AgClO_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 Ag | 6 | -6 HClO3 | 6 | -6 H_2O | 3 | 3 AgCl | 1 | 1 AgClO_3 | 5 | 5 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 Ag | 6 | -6 | -1/6 (Δ[Ag])/(Δt) HClO3 | 6 | -6 | -1/6 (Δ[HClO3])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) AgCl | 1 | 1 | (Δ[AgCl])/(Δt) AgClO_3 | 5 | 5 | 1/5 (Δ[AgClO3])/(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 = -1/6 (Δ[Ag])/(Δt) = -1/6 (Δ[HClO3])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[AgCl])/(Δt) = 1/5 (Δ[AgClO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| silver | HClO3 | water | silver chloride | silver chlorate formula | Ag | HClO3 | H_2O | AgCl | AgClO_3 name | silver | | water | silver chloride | silver chlorate IUPAC name | silver | | water | chlorosilver | silver chlorate
| silver | HClO3 | water | silver chloride | silver chlorate formula | Ag | HClO3 | H_2O | AgCl | AgClO_3 name | silver | | water | silver chloride | silver chlorate IUPAC name | silver | | water | chlorosilver | silver chlorate

Substance properties

| silver | HClO3 | water | silver chloride | silver chlorate molar mass | 107.8682 g/mol | 84.45 g/mol | 18.015 g/mol | 143.32 g/mol | 191.32 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 960 °C | | 0 °C | 455 °C | 230 °C boiling point | 2212 °C | | 99.9839 °C | 1554 °C | density | 10.49 g/cm^3 | | 1 g/cm^3 | 5.56 g/cm^3 | 4.43 g/cm^3 solubility in water | insoluble | | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |
| silver | HClO3 | water | silver chloride | silver chlorate molar mass | 107.8682 g/mol | 84.45 g/mol | 18.015 g/mol | 143.32 g/mol | 191.32 g/mol phase | solid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 960 °C | | 0 °C | 455 °C | 230 °C boiling point | 2212 °C | | 99.9839 °C | 1554 °C | density | 10.49 g/cm^3 | | 1 g/cm^3 | 5.56 g/cm^3 | 4.43 g/cm^3 solubility in water | insoluble | | | | soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |

Units

Random Queries

bromide name of 2 propylzinc bromide
ionic radius of anions
alternate names of silver(I) cation vs diamminesilver(I) cation
iodine vs ruthenium vs tellurium
blocks of noble metals
1,1'-dioctadecyl-4,4'-bipyridinium diperchlorate
oil painting effect image of jennite
ion class of thallium(III) cation vs aluminum cation
name of iron(II) chromite vs digermane
half-life of Zr-92 vs Os-189