Search

AgNO3 + HgCl2 = AgCl + Hg(NO3)2

Input interpretation

AgNO_3 silver nitrate + HgCl_2 mercuric chloride ⟶ AgCl silver chloride + Hg(NO_3)_2 mercury(II) nitrate
AgNO_3 silver nitrate + HgCl_2 mercuric chloride ⟶ AgCl silver chloride + Hg(NO_3)_2 mercury(II) nitrate

Balanced equation

Balance the chemical equation algebraically: AgNO_3 + HgCl_2 ⟶ AgCl + Hg(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 HgCl_2 ⟶ c_3 AgCl + c_4 Hg(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Cl and Hg: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 6 c_4 Cl: | 2 c_2 = c_3 Hg: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + HgCl_2 ⟶ 2 AgCl + Hg(NO_3)_2
Balance the chemical equation algebraically: AgNO_3 + HgCl_2 ⟶ AgCl + Hg(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 HgCl_2 ⟶ c_3 AgCl + c_4 Hg(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Cl and Hg: Ag: | c_1 = c_3 N: | c_1 = 2 c_4 O: | 3 c_1 = 6 c_4 Cl: | 2 c_2 = c_3 Hg: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 AgNO_3 + HgCl_2 ⟶ 2 AgCl + Hg(NO_3)_2

Structures

+ ⟶ +
+ ⟶ +

Names

silver nitrate + mercuric chloride ⟶ silver chloride + mercury(II) nitrate
silver nitrate + mercuric chloride ⟶ silver chloride + mercury(II) nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: AgNO_3 + HgCl_2 ⟶ AgCl + Hg(NO_3)_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: 2 AgNO_3 + HgCl_2 ⟶ 2 AgCl + Hg(NO_3)_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 AgNO_3 | 2 | -2 HgCl_2 | 1 | -1 AgCl | 2 | 2 Hg(NO_3)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 2 | -2 | ([AgNO3])^(-2) HgCl_2 | 1 | -1 | ([HgCl2])^(-1) AgCl | 2 | 2 | ([AgCl])^2 Hg(NO_3)_2 | 1 | 1 | [Hg(NO3)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 = ([AgNO3])^(-2) ([HgCl2])^(-1) ([AgCl])^2 [Hg(NO3)2] = (([AgCl])^2 [Hg(NO3)2])/(([AgNO3])^2 [HgCl2])
Construct the equilibrium constant, K, expression for: AgNO_3 + HgCl_2 ⟶ AgCl + Hg(NO_3)_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: 2 AgNO_3 + HgCl_2 ⟶ 2 AgCl + Hg(NO_3)_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 AgNO_3 | 2 | -2 HgCl_2 | 1 | -1 AgCl | 2 | 2 Hg(NO_3)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 2 | -2 | ([AgNO3])^(-2) HgCl_2 | 1 | -1 | ([HgCl2])^(-1) AgCl | 2 | 2 | ([AgCl])^2 Hg(NO_3)_2 | 1 | 1 | [Hg(NO3)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 = ([AgNO3])^(-2) ([HgCl2])^(-1) ([AgCl])^2 [Hg(NO3)2] = (([AgCl])^2 [Hg(NO3)2])/(([AgNO3])^2 [HgCl2])

Rate of reaction

Construct the rate of reaction expression for: AgNO_3 + HgCl_2 ⟶ AgCl + Hg(NO_3)_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: 2 AgNO_3 + HgCl_2 ⟶ 2 AgCl + Hg(NO_3)_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 AgNO_3 | 2 | -2 HgCl_2 | 1 | -1 AgCl | 2 | 2 Hg(NO_3)_2 | 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 AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) HgCl_2 | 1 | -1 | -(Δ[HgCl2])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(Δt) Hg(NO_3)_2 | 1 | 1 | (Δ[Hg(NO3)2])/(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[AgNO3])/(Δt) = -(Δ[HgCl2])/(Δt) = 1/2 (Δ[AgCl])/(Δt) = (Δ[Hg(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: AgNO_3 + HgCl_2 ⟶ AgCl + Hg(NO_3)_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: 2 AgNO_3 + HgCl_2 ⟶ 2 AgCl + Hg(NO_3)_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 AgNO_3 | 2 | -2 HgCl_2 | 1 | -1 AgCl | 2 | 2 Hg(NO_3)_2 | 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 AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) HgCl_2 | 1 | -1 | -(Δ[HgCl2])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(Δt) Hg(NO_3)_2 | 1 | 1 | (Δ[Hg(NO3)2])/(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[AgNO3])/(Δt) = -(Δ[HgCl2])/(Δt) = 1/2 (Δ[AgCl])/(Δt) = (Δ[Hg(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| silver nitrate | mercuric chloride | silver chloride | mercury(II) nitrate formula | AgNO_3 | HgCl_2 | AgCl | Hg(NO_3)_2 Hill formula | AgNO_3 | Cl_2Hg | AgCl | HgN_2O_6 name | silver nitrate | mercuric chloride | silver chloride | mercury(II) nitrate IUPAC name | silver nitrate | dichloromercury | chlorosilver | mercury(+2) cation dinitrate
| silver nitrate | mercuric chloride | silver chloride | mercury(II) nitrate formula | AgNO_3 | HgCl_2 | AgCl | Hg(NO_3)_2 Hill formula | AgNO_3 | Cl_2Hg | AgCl | HgN_2O_6 name | silver nitrate | mercuric chloride | silver chloride | mercury(II) nitrate IUPAC name | silver nitrate | dichloromercury | chlorosilver | mercury(+2) cation dinitrate

Substance properties

| silver nitrate | mercuric chloride | silver chloride | mercury(II) nitrate molar mass | 169.87 g/mol | 271.49 g/mol | 143.32 g/mol | 324.6 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 277 °C | 455 °C | 79 °C boiling point | | 302 °C | 1554 °C | density | | 5.44 g/cm^3 | 5.56 g/cm^3 | 4.3 g/cm^3 solubility in water | soluble | | | soluble odor | odorless | odorless | |
| silver nitrate | mercuric chloride | silver chloride | mercury(II) nitrate molar mass | 169.87 g/mol | 271.49 g/mol | 143.32 g/mol | 324.6 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 212 °C | 277 °C | 455 °C | 79 °C boiling point | | 302 °C | 1554 °C | density | | 5.44 g/cm^3 | 5.56 g/cm^3 | 4.3 g/cm^3 solubility in water | soluble | | | soluble odor | odorless | odorless | |

Units

Random Queries

visible atomic spectrum of manganese
name of spodumene vs polylithionite
freezing point of sodium mercury amalgam vs potassium dihydrogen arsenate
mass fractions of (pentafluorophenyl)triethoxysilane
sulfur vs chlorine vs neon
top 10 chemicals by NFPA health rating
selenium hexafluoride vs 4-(trifluoromethyl)benzoic acid
chemical types of sec-butanol vs (R)-(-)-dihydro-5-(p-tolylsulfonyloxymethyl)-2(3 H)-furanone
IUPAC name of beryllium oxide vs bismuth sulfide
name of titanium disulfide vs strontium thiosulfate pentahydrate