Search

HNO3 + [Ag(NH3)2]Cl = NH4NO3 + AgCl

Input interpretation

HNO_3 nitric acid + Ag(NH3)2Cl ⟶ NH_4NO_3 ammonium nitrate + AgCl silver chloride
HNO_3 nitric acid + Ag(NH3)2Cl ⟶ NH_4NO_3 ammonium nitrate + AgCl silver chloride

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Ag(NH3)2Cl ⟶ NH_4NO_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Ag(NH3)2Cl ⟶ c_3 NH_4NO_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Ag and Cl: H: | c_1 + 6 c_2 = 4 c_3 N: | c_1 + 2 c_2 = 2 c_3 O: | 3 c_1 = 3 c_3 Ag: | c_2 = c_4 Cl: | 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 HNO_3 + Ag(NH3)2Cl ⟶ 2 NH_4NO_3 + AgCl
Balance the chemical equation algebraically: HNO_3 + Ag(NH3)2Cl ⟶ NH_4NO_3 + AgCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Ag(NH3)2Cl ⟶ c_3 NH_4NO_3 + c_4 AgCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Ag and Cl: H: | c_1 + 6 c_2 = 4 c_3 N: | c_1 + 2 c_2 = 2 c_3 O: | 3 c_1 = 3 c_3 Ag: | c_2 = c_4 Cl: | 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 HNO_3 + Ag(NH3)2Cl ⟶ 2 NH_4NO_3 + AgCl

Structures

+ Ag(NH3)2Cl ⟶ +
+ Ag(NH3)2Cl ⟶ +

Names

nitric acid + Ag(NH3)2Cl ⟶ ammonium nitrate + silver chloride
nitric acid + Ag(NH3)2Cl ⟶ ammonium nitrate + silver chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Ag(NH3)2Cl ⟶ NH_4NO_3 + AgCl 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 HNO_3 + Ag(NH3)2Cl ⟶ 2 NH_4NO_3 + AgCl 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 HNO_3 | 2 | -2 Ag(NH3)2Cl | 1 | -1 NH_4NO_3 | 2 | 2 AgCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) Ag(NH3)2Cl | 1 | -1 | ([Ag(NH3)2Cl])^(-1) NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 AgCl | 1 | 1 | [AgCl] 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 = ([HNO3])^(-2) ([Ag(NH3)2Cl])^(-1) ([NH4NO3])^2 [AgCl] = (([NH4NO3])^2 [AgCl])/(([HNO3])^2 [Ag(NH3)2Cl])
Construct the equilibrium constant, K, expression for: HNO_3 + Ag(NH3)2Cl ⟶ NH_4NO_3 + AgCl 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 HNO_3 + Ag(NH3)2Cl ⟶ 2 NH_4NO_3 + AgCl 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 HNO_3 | 2 | -2 Ag(NH3)2Cl | 1 | -1 NH_4NO_3 | 2 | 2 AgCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) Ag(NH3)2Cl | 1 | -1 | ([Ag(NH3)2Cl])^(-1) NH_4NO_3 | 2 | 2 | ([NH4NO3])^2 AgCl | 1 | 1 | [AgCl] 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 = ([HNO3])^(-2) ([Ag(NH3)2Cl])^(-1) ([NH4NO3])^2 [AgCl] = (([NH4NO3])^2 [AgCl])/(([HNO3])^2 [Ag(NH3)2Cl])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Ag(NH3)2Cl ⟶ NH_4NO_3 + AgCl 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 HNO_3 + Ag(NH3)2Cl ⟶ 2 NH_4NO_3 + AgCl 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 HNO_3 | 2 | -2 Ag(NH3)2Cl | 1 | -1 NH_4NO_3 | 2 | 2 AgCl | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) Ag(NH3)2Cl | 1 | -1 | -(Δ[Ag(NH3)2Cl])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(Δt) AgCl | 1 | 1 | (Δ[AgCl])/(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[HNO3])/(Δt) = -(Δ[Ag(NH3)2Cl])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) = (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Ag(NH3)2Cl ⟶ NH_4NO_3 + AgCl 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 HNO_3 + Ag(NH3)2Cl ⟶ 2 NH_4NO_3 + AgCl 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 HNO_3 | 2 | -2 Ag(NH3)2Cl | 1 | -1 NH_4NO_3 | 2 | 2 AgCl | 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 HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) Ag(NH3)2Cl | 1 | -1 | -(Δ[Ag(NH3)2Cl])/(Δt) NH_4NO_3 | 2 | 2 | 1/2 (Δ[NH4NO3])/(Δt) AgCl | 1 | 1 | (Δ[AgCl])/(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[HNO3])/(Δt) = -(Δ[Ag(NH3)2Cl])/(Δt) = 1/2 (Δ[NH4NO3])/(Δt) = (Δ[AgCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | Ag(NH3)2Cl | ammonium nitrate | silver chloride formula | HNO_3 | Ag(NH3)2Cl | NH_4NO_3 | AgCl Hill formula | HNO_3 | H6AgClN2 | H_4N_2O_3 | AgCl name | nitric acid | | ammonium nitrate | silver chloride IUPAC name | nitric acid | | | chlorosilver
| nitric acid | Ag(NH3)2Cl | ammonium nitrate | silver chloride formula | HNO_3 | Ag(NH3)2Cl | NH_4NO_3 | AgCl Hill formula | HNO_3 | H6AgClN2 | H_4N_2O_3 | AgCl name | nitric acid | | ammonium nitrate | silver chloride IUPAC name | nitric acid | | | chlorosilver

Substance properties

| nitric acid | Ag(NH3)2Cl | ammonium nitrate | silver chloride molar mass | 63.012 g/mol | 177.38 g/mol | 80.04 g/mol | 143.32 g/mol phase | liquid (at STP) | | solid (at STP) | solid (at STP) melting point | -41.6 °C | | 169 °C | 455 °C boiling point | 83 °C | | 210 °C | 1554 °C density | 1.5129 g/cm^3 | | 1.73 g/cm^3 | 5.56 g/cm^3 solubility in water | miscible | | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | | odor | | | odorless |
| nitric acid | Ag(NH3)2Cl | ammonium nitrate | silver chloride molar mass | 63.012 g/mol | 177.38 g/mol | 80.04 g/mol | 143.32 g/mol phase | liquid (at STP) | | solid (at STP) | solid (at STP) melting point | -41.6 °C | | 169 °C | 455 °C boiling point | 83 °C | | 210 °C | 1554 °C density | 1.5129 g/cm^3 | | 1.73 g/cm^3 | 5.56 g/cm^3 solubility in water | miscible | | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | | odor | | | odorless |

Units

Random Queries

name of stannic chloride pentahydrate
bond types of phosphonium iodide
name of yttrium(III) cation
group of oxygen vs chlorine
vertex coordinates water
color of tantalum vs molybdenum
InChI identifier of benzyl cyanide-d 7
(name of superoxide anion)/(net ionic charge of superoxide anion)
chemical types of oxygen difluoride vs 1-chloro-1-fluoroethylene
alternate names of iron(II) bromide