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HCl + HNO3 + Pt = H2O + NO + H2N + PtCl

Input interpretation

HCl hydrogen chloride + HNO_3 nitric acid + Pt platinum ⟶ H_2O water + NO nitric oxide + H2N + PtCl
HCl hydrogen chloride + HNO_3 nitric acid + Pt platinum ⟶ H_2O water + NO nitric oxide + H2N + PtCl

Balanced equation

Balance the chemical equation algebraically: HCl + HNO_3 + Pt ⟶ H_2O + NO + H2N + PtCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 Pt ⟶ c_4 H_2O + c_5 NO + c_6 H2N + c_7 PtCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and Pt: Cl: | c_1 = c_7 H: | c_1 + c_2 = 2 c_4 + 2 c_6 N: | c_2 = c_5 + c_6 O: | 3 c_2 = c_4 + c_5 Pt: | c_3 = c_7 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_5 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1/7 + 4/7 c_3 = c_1 c_4 = (3 c_1)/7 + 5/7 c_5 = 1 c_6 = c_1/7 - 3/7 c_7 = c_1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 24 and solve for the remaining coefficients: c_1 = 24 c_2 = 4 c_3 = 24 c_4 = 11 c_5 = 1 c_6 = 3 c_7 = 24 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 24 HCl + 4 HNO_3 + 24 Pt ⟶ 11 H_2O + NO + 3 H2N + 24 PtCl
Balance the chemical equation algebraically: HCl + HNO_3 + Pt ⟶ H_2O + NO + H2N + PtCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 HNO_3 + c_3 Pt ⟶ c_4 H_2O + c_5 NO + c_6 H2N + c_7 PtCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and Pt: Cl: | c_1 = c_7 H: | c_1 + c_2 = 2 c_4 + 2 c_6 N: | c_2 = c_5 + c_6 O: | 3 c_2 = c_4 + c_5 Pt: | c_3 = c_7 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_5 = 1 and solve the system of equations for the remaining coefficients: c_2 = c_1/7 + 4/7 c_3 = c_1 c_4 = (3 c_1)/7 + 5/7 c_5 = 1 c_6 = c_1/7 - 3/7 c_7 = c_1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 24 and solve for the remaining coefficients: c_1 = 24 c_2 = 4 c_3 = 24 c_4 = 11 c_5 = 1 c_6 = 3 c_7 = 24 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 24 HCl + 4 HNO_3 + 24 Pt ⟶ 11 H_2O + NO + 3 H2N + 24 PtCl

Structures

+ + ⟶ + + H2N + PtCl
+ + ⟶ + + H2N + PtCl

Names

hydrogen chloride + nitric acid + platinum ⟶ water + nitric oxide + H2N + PtCl
hydrogen chloride + nitric acid + platinum ⟶ water + nitric oxide + H2N + PtCl

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + HNO_3 + Pt ⟶ H_2O + NO + H2N + PtCl 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: 24 HCl + 4 HNO_3 + 24 Pt ⟶ 11 H_2O + NO + 3 H2N + 24 PtCl 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 | 24 | -24 HNO_3 | 4 | -4 Pt | 24 | -24 H_2O | 11 | 11 NO | 1 | 1 H2N | 3 | 3 PtCl | 24 | 24 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 24 | -24 | ([HCl])^(-24) HNO_3 | 4 | -4 | ([HNO3])^(-4) Pt | 24 | -24 | ([Pt])^(-24) H_2O | 11 | 11 | ([H2O])^11 NO | 1 | 1 | [NO] H2N | 3 | 3 | ([H2N])^3 PtCl | 24 | 24 | ([PtCl])^24 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])^(-24) ([HNO3])^(-4) ([Pt])^(-24) ([H2O])^11 [NO] ([H2N])^3 ([PtCl])^24 = (([H2O])^11 [NO] ([H2N])^3 ([PtCl])^24)/(([HCl])^24 ([HNO3])^4 ([Pt])^24)
Construct the equilibrium constant, K, expression for: HCl + HNO_3 + Pt ⟶ H_2O + NO + H2N + PtCl 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: 24 HCl + 4 HNO_3 + 24 Pt ⟶ 11 H_2O + NO + 3 H2N + 24 PtCl 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 | 24 | -24 HNO_3 | 4 | -4 Pt | 24 | -24 H_2O | 11 | 11 NO | 1 | 1 H2N | 3 | 3 PtCl | 24 | 24 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 24 | -24 | ([HCl])^(-24) HNO_3 | 4 | -4 | ([HNO3])^(-4) Pt | 24 | -24 | ([Pt])^(-24) H_2O | 11 | 11 | ([H2O])^11 NO | 1 | 1 | [NO] H2N | 3 | 3 | ([H2N])^3 PtCl | 24 | 24 | ([PtCl])^24 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])^(-24) ([HNO3])^(-4) ([Pt])^(-24) ([H2O])^11 [NO] ([H2N])^3 ([PtCl])^24 = (([H2O])^11 [NO] ([H2N])^3 ([PtCl])^24)/(([HCl])^24 ([HNO3])^4 ([Pt])^24)

Rate of reaction

Construct the rate of reaction expression for: HCl + HNO_3 + Pt ⟶ H_2O + NO + H2N + PtCl 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: 24 HCl + 4 HNO_3 + 24 Pt ⟶ 11 H_2O + NO + 3 H2N + 24 PtCl 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 | 24 | -24 HNO_3 | 4 | -4 Pt | 24 | -24 H_2O | 11 | 11 NO | 1 | 1 H2N | 3 | 3 PtCl | 24 | 24 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 | 24 | -24 | -1/24 (Δ[HCl])/(Δt) HNO_3 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) Pt | 24 | -24 | -1/24 (Δ[Pt])/(Δt) H_2O | 11 | 11 | 1/11 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) H2N | 3 | 3 | 1/3 (Δ[H2N])/(Δt) PtCl | 24 | 24 | 1/24 (Δ[PtCl])/(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 = -1/24 (Δ[HCl])/(Δt) = -1/4 (Δ[HNO3])/(Δt) = -1/24 (Δ[Pt])/(Δt) = 1/11 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = 1/3 (Δ[H2N])/(Δt) = 1/24 (Δ[PtCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + HNO_3 + Pt ⟶ H_2O + NO + H2N + PtCl 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: 24 HCl + 4 HNO_3 + 24 Pt ⟶ 11 H_2O + NO + 3 H2N + 24 PtCl 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 | 24 | -24 HNO_3 | 4 | -4 Pt | 24 | -24 H_2O | 11 | 11 NO | 1 | 1 H2N | 3 | 3 PtCl | 24 | 24 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 | 24 | -24 | -1/24 (Δ[HCl])/(Δt) HNO_3 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) Pt | 24 | -24 | -1/24 (Δ[Pt])/(Δt) H_2O | 11 | 11 | 1/11 (Δ[H2O])/(Δt) NO | 1 | 1 | (Δ[NO])/(Δt) H2N | 3 | 3 | 1/3 (Δ[H2N])/(Δt) PtCl | 24 | 24 | 1/24 (Δ[PtCl])/(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 = -1/24 (Δ[HCl])/(Δt) = -1/4 (Δ[HNO3])/(Δt) = -1/24 (Δ[Pt])/(Δt) = 1/11 (Δ[H2O])/(Δt) = (Δ[NO])/(Δt) = 1/3 (Δ[H2N])/(Δt) = 1/24 (Δ[PtCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | nitric acid | platinum | water | nitric oxide | H2N | PtCl formula | HCl | HNO_3 | Pt | H_2O | NO | H2N | PtCl Hill formula | ClH | HNO_3 | Pt | H_2O | NO | H2N | ClPt name | hydrogen chloride | nitric acid | platinum | water | nitric oxide | |
| hydrogen chloride | nitric acid | platinum | water | nitric oxide | H2N | PtCl formula | HCl | HNO_3 | Pt | H_2O | NO | H2N | PtCl Hill formula | ClH | HNO_3 | Pt | H_2O | NO | H2N | ClPt name | hydrogen chloride | nitric acid | platinum | water | nitric oxide | |

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