Search

HCl + SnCl2 + HNO2 = H2O + NO + SnCl4

Input interpretation

HCl hydrogen chloride + SnCl_2 stannous chloride + HNO_2 nitrous acid ⟶ H_2O water + NO nitric oxide + SnCl_4 stannic chloride
HCl hydrogen chloride + SnCl_2 stannous chloride + HNO_2 nitrous acid ⟶ H_2O water + NO nitric oxide + SnCl_4 stannic chloride

Balanced equation

Balance the chemical equation algebraically: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 SnCl_2 + c_3 HNO_2 ⟶ c_4 H_2O + c_5 NO + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Sn, N and O: Cl: | c_1 + 2 c_2 = 4 c_6 H: | c_1 + c_3 = 2 c_4 Sn: | c_2 = c_6 N: | c_3 = c_5 O: | 2 c_3 = c_4 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4
Balance the chemical equation algebraically: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 SnCl_2 + c_3 HNO_2 ⟶ c_4 H_2O + c_5 NO + c_6 SnCl_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Sn, N and O: Cl: | c_1 + 2 c_2 = 4 c_6 H: | c_1 + c_3 = 2 c_4 Sn: | c_2 = c_6 N: | c_3 = c_5 O: | 2 c_3 = c_4 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 2 c_6 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4

Structures

+ + ⟶ + +
+ + ⟶ + +

Names

hydrogen chloride + stannous chloride + nitrous acid ⟶ water + nitric oxide + stannic chloride
hydrogen chloride + stannous chloride + nitrous acid ⟶ water + nitric oxide + stannic chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 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 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4 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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) SnCl_2 | 1 | -1 | ([SnCl2])^(-1) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO | 2 | 2 | ([NO])^2 SnCl_4 | 1 | 1 | [SnCl4] 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 = ([HCl])^(-2) ([SnCl2])^(-1) ([HNO2])^(-2) ([H2O])^2 ([NO])^2 [SnCl4] = (([H2O])^2 ([NO])^2 [SnCl4])/(([HCl])^2 [SnCl2] ([HNO2])^2)
Construct the equilibrium constant, K, expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 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 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4 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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) SnCl_2 | 1 | -1 | ([SnCl2])^(-1) HNO_2 | 2 | -2 | ([HNO2])^(-2) H_2O | 2 | 2 | ([H2O])^2 NO | 2 | 2 | ([NO])^2 SnCl_4 | 1 | 1 | [SnCl4] 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 = ([HCl])^(-2) ([SnCl2])^(-1) ([HNO2])^(-2) ([H2O])^2 ([NO])^2 [SnCl4] = (([H2O])^2 ([NO])^2 [SnCl4])/(([HCl])^2 [SnCl2] ([HNO2])^2)

Rate of reaction

Construct the rate of reaction expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 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 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4 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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(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[HCl])/(Δt) = -(Δ[SnCl2])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + SnCl_2 + HNO_2 ⟶ H_2O + NO + SnCl_4 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 HCl + SnCl_2 + 2 HNO_2 ⟶ 2 H_2O + 2 NO + SnCl_4 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 HCl | 2 | -2 SnCl_2 | 1 | -1 HNO_2 | 2 | -2 H_2O | 2 | 2 NO | 2 | 2 SnCl_4 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) SnCl_2 | 1 | -1 | -(Δ[SnCl2])/(Δt) HNO_2 | 2 | -2 | -1/2 (Δ[HNO2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NO | 2 | 2 | 1/2 (Δ[NO])/(Δt) SnCl_4 | 1 | 1 | (Δ[SnCl4])/(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[HCl])/(Δt) = -(Δ[SnCl2])/(Δt) = -1/2 (Δ[HNO2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/2 (Δ[NO])/(Δt) = (Δ[SnCl4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride formula | HCl | SnCl_2 | HNO_2 | H_2O | NO | SnCl_4 Hill formula | ClH | Cl_2Sn | HNO_2 | H_2O | NO | Cl_4Sn name | hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride IUPAC name | hydrogen chloride | dichlorotin | nitrous acid | water | nitric oxide | tetrachlorostannane
| hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride formula | HCl | SnCl_2 | HNO_2 | H_2O | NO | SnCl_4 Hill formula | ClH | Cl_2Sn | HNO_2 | H_2O | NO | Cl_4Sn name | hydrogen chloride | stannous chloride | nitrous acid | water | nitric oxide | stannic chloride IUPAC name | hydrogen chloride | dichlorotin | nitrous acid | water | nitric oxide | tetrachlorostannane

Random Queries

melting point of ethyl ether vs beta-naphthoflavone
formula of carbon dioxide
van der Waals radius moscovium
CAS number of rhodium(III) bromide
molar mass of carbon monoxide vs hydrogen chloride
net ionic charge of indium(III) cation
group of zirconium vs palladium
half-life of Nd-143 vs Nb-93
lead(II) cation
atomic number of ferromagnetic elements