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ZnCl2 + Ag2CO3 = AgCl + ZnCO3

Input interpretation

ZnCl_2 zinc chloride + Ag_2CO_3 silver(I) carbonate ⟶ AgCl silver chloride + ZnCO_3 zinc carbonate
ZnCl_2 zinc chloride + Ag_2CO_3 silver(I) carbonate ⟶ AgCl silver chloride + ZnCO_3 zinc carbonate

Balanced equation

Balance the chemical equation algebraically: ZnCl_2 + Ag_2CO_3 ⟶ AgCl + ZnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ZnCl_2 + c_2 Ag_2CO_3 ⟶ c_3 AgCl + c_4 ZnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Zn, Ag, C and O: Cl: | 2 c_1 = c_3 Zn: | c_1 = c_4 Ag: | 2 c_2 = c_3 C: | c_2 = c_4 O: | 3 c_2 = 3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | ZnCl_2 + Ag_2CO_3 ⟶ 2 AgCl + ZnCO_3
Balance the chemical equation algebraically: ZnCl_2 + Ag_2CO_3 ⟶ AgCl + ZnCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 ZnCl_2 + c_2 Ag_2CO_3 ⟶ c_3 AgCl + c_4 ZnCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Zn, Ag, C and O: Cl: | 2 c_1 = c_3 Zn: | c_1 = c_4 Ag: | 2 c_2 = c_3 C: | c_2 = c_4 O: | 3 c_2 = 3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | ZnCl_2 + Ag_2CO_3 ⟶ 2 AgCl + ZnCO_3

Structures

+ ⟶ +
+ ⟶ +

Names

zinc chloride + silver(I) carbonate ⟶ silver chloride + zinc carbonate
zinc chloride + silver(I) carbonate ⟶ silver chloride + zinc carbonate

Equilibrium constant

Construct the equilibrium constant, K, expression for: ZnCl_2 + Ag_2CO_3 ⟶ AgCl + ZnCO_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: ZnCl_2 + Ag_2CO_3 ⟶ 2 AgCl + ZnCO_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 ZnCl_2 | 1 | -1 Ag_2CO_3 | 1 | -1 AgCl | 2 | 2 ZnCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression ZnCl_2 | 1 | -1 | ([ZnCl2])^(-1) Ag_2CO_3 | 1 | -1 | ([Ag2CO3])^(-1) AgCl | 2 | 2 | ([AgCl])^2 ZnCO_3 | 1 | 1 | [ZnCO3] 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 = ([ZnCl2])^(-1) ([Ag2CO3])^(-1) ([AgCl])^2 [ZnCO3] = (([AgCl])^2 [ZnCO3])/([ZnCl2] [Ag2CO3])
Construct the equilibrium constant, K, expression for: ZnCl_2 + Ag_2CO_3 ⟶ AgCl + ZnCO_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: ZnCl_2 + Ag_2CO_3 ⟶ 2 AgCl + ZnCO_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 ZnCl_2 | 1 | -1 Ag_2CO_3 | 1 | -1 AgCl | 2 | 2 ZnCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression ZnCl_2 | 1 | -1 | ([ZnCl2])^(-1) Ag_2CO_3 | 1 | -1 | ([Ag2CO3])^(-1) AgCl | 2 | 2 | ([AgCl])^2 ZnCO_3 | 1 | 1 | [ZnCO3] 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 = ([ZnCl2])^(-1) ([Ag2CO3])^(-1) ([AgCl])^2 [ZnCO3] = (([AgCl])^2 [ZnCO3])/([ZnCl2] [Ag2CO3])

Rate of reaction

Construct the rate of reaction expression for: ZnCl_2 + Ag_2CO_3 ⟶ AgCl + ZnCO_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: ZnCl_2 + Ag_2CO_3 ⟶ 2 AgCl + ZnCO_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 ZnCl_2 | 1 | -1 Ag_2CO_3 | 1 | -1 AgCl | 2 | 2 ZnCO_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 ZnCl_2 | 1 | -1 | -(Δ[ZnCl2])/(Δt) Ag_2CO_3 | 1 | -1 | -(Δ[Ag2CO3])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(Δt) ZnCO_3 | 1 | 1 | (Δ[ZnCO3])/(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 = -(Δ[ZnCl2])/(Δt) = -(Δ[Ag2CO3])/(Δt) = 1/2 (Δ[AgCl])/(Δt) = (Δ[ZnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: ZnCl_2 + Ag_2CO_3 ⟶ AgCl + ZnCO_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: ZnCl_2 + Ag_2CO_3 ⟶ 2 AgCl + ZnCO_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 ZnCl_2 | 1 | -1 Ag_2CO_3 | 1 | -1 AgCl | 2 | 2 ZnCO_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 ZnCl_2 | 1 | -1 | -(Δ[ZnCl2])/(Δt) Ag_2CO_3 | 1 | -1 | -(Δ[Ag2CO3])/(Δt) AgCl | 2 | 2 | 1/2 (Δ[AgCl])/(Δt) ZnCO_3 | 1 | 1 | (Δ[ZnCO3])/(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 = -(Δ[ZnCl2])/(Δt) = -(Δ[Ag2CO3])/(Δt) = 1/2 (Δ[AgCl])/(Δt) = (Δ[ZnCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| zinc chloride | silver(I) carbonate | silver chloride | zinc carbonate formula | ZnCl_2 | Ag_2CO_3 | AgCl | ZnCO_3 Hill formula | Cl_2Zn | Ag_2CO_3 | AgCl | CO_3Zn name | zinc chloride | silver(I) carbonate | silver chloride | zinc carbonate IUPAC name | zinc dichloride | disilver; carbonate | chlorosilver | zinc carbonate
| zinc chloride | silver(I) carbonate | silver chloride | zinc carbonate formula | ZnCl_2 | Ag_2CO_3 | AgCl | ZnCO_3 Hill formula | Cl_2Zn | Ag_2CO_3 | AgCl | CO_3Zn name | zinc chloride | silver(I) carbonate | silver chloride | zinc carbonate IUPAC name | zinc dichloride | disilver; carbonate | chlorosilver | zinc carbonate

Substance properties

| zinc chloride | silver(I) carbonate | silver chloride | zinc carbonate molar mass | 136.3 g/mol | 275.744 g/mol | 143.32 g/mol | 125.4 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 293 °C | 210 °C | 455 °C | boiling point | | | 1554 °C | density | | 6.08 g/cm^3 | 5.56 g/cm^3 | 4.3476 g/cm^3 solubility in water | soluble | insoluble | | insoluble odor | odorless | | |
| zinc chloride | silver(I) carbonate | silver chloride | zinc carbonate molar mass | 136.3 g/mol | 275.744 g/mol | 143.32 g/mol | 125.4 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 293 °C | 210 °C | 455 °C | boiling point | | | 1554 °C | density | | 6.08 g/cm^3 | 5.56 g/cm^3 | 4.3476 g/cm^3 solubility in water | soluble | insoluble | | insoluble odor | odorless | | |

Units

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