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HNO3 + Ca = H2O + Ca(NO3)2 + HN4NO3

Input interpretation

HNO_3 nitric acid + Ca calcium ⟶ H_2O water + Ca(NO_3)_2 calcium nitrate + HN4NO3
HNO_3 nitric acid + Ca calcium ⟶ H_2O water + Ca(NO_3)_2 calcium nitrate + HN4NO3

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Ca ⟶ H_2O + Ca(NO_3)_2 + HN4NO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Ca ⟶ c_3 H_2O + c_4 Ca(NO_3)_2 + c_5 HN4NO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Ca: H: | c_1 = 2 c_3 + c_5 N: | c_1 = 2 c_4 + 5 c_5 O: | 3 c_1 = c_3 + 6 c_4 + 3 c_5 Ca: | 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 25 c_2 = 10 c_3 = 12 c_4 = 10 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 25 HNO_3 + 10 Ca ⟶ 12 H_2O + 10 Ca(NO_3)_2 + HN4NO3
Balance the chemical equation algebraically: HNO_3 + Ca ⟶ H_2O + Ca(NO_3)_2 + HN4NO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Ca ⟶ c_3 H_2O + c_4 Ca(NO_3)_2 + c_5 HN4NO3 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Ca: H: | c_1 = 2 c_3 + c_5 N: | c_1 = 2 c_4 + 5 c_5 O: | 3 c_1 = c_3 + 6 c_4 + 3 c_5 Ca: | 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 25 c_2 = 10 c_3 = 12 c_4 = 10 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 25 HNO_3 + 10 Ca ⟶ 12 H_2O + 10 Ca(NO_3)_2 + HN4NO3

Structures

+ ⟶ + + HN4NO3
+ ⟶ + + HN4NO3

Names

nitric acid + calcium ⟶ water + calcium nitrate + HN4NO3
nitric acid + calcium ⟶ water + calcium nitrate + HN4NO3

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Ca ⟶ H_2O + Ca(NO_3)_2 + HN4NO3 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: 25 HNO_3 + 10 Ca ⟶ 12 H_2O + 10 Ca(NO_3)_2 + HN4NO3 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 | 25 | -25 Ca | 10 | -10 H_2O | 12 | 12 Ca(NO_3)_2 | 10 | 10 HN4NO3 | 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 | 25 | -25 | ([HNO3])^(-25) Ca | 10 | -10 | ([Ca])^(-10) H_2O | 12 | 12 | ([H2O])^12 Ca(NO_3)_2 | 10 | 10 | ([Ca(NO3)2])^10 HN4NO3 | 1 | 1 | [HN4NO3] 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])^(-25) ([Ca])^(-10) ([H2O])^12 ([Ca(NO3)2])^10 [HN4NO3] = (([H2O])^12 ([Ca(NO3)2])^10 [HN4NO3])/(([HNO3])^25 ([Ca])^10)
Construct the equilibrium constant, K, expression for: HNO_3 + Ca ⟶ H_2O + Ca(NO_3)_2 + HN4NO3 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: 25 HNO_3 + 10 Ca ⟶ 12 H_2O + 10 Ca(NO_3)_2 + HN4NO3 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 | 25 | -25 Ca | 10 | -10 H_2O | 12 | 12 Ca(NO_3)_2 | 10 | 10 HN4NO3 | 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 | 25 | -25 | ([HNO3])^(-25) Ca | 10 | -10 | ([Ca])^(-10) H_2O | 12 | 12 | ([H2O])^12 Ca(NO_3)_2 | 10 | 10 | ([Ca(NO3)2])^10 HN4NO3 | 1 | 1 | [HN4NO3] 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])^(-25) ([Ca])^(-10) ([H2O])^12 ([Ca(NO3)2])^10 [HN4NO3] = (([H2O])^12 ([Ca(NO3)2])^10 [HN4NO3])/(([HNO3])^25 ([Ca])^10)

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Ca ⟶ H_2O + Ca(NO_3)_2 + HN4NO3 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: 25 HNO_3 + 10 Ca ⟶ 12 H_2O + 10 Ca(NO_3)_2 + HN4NO3 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 | 25 | -25 Ca | 10 | -10 H_2O | 12 | 12 Ca(NO_3)_2 | 10 | 10 HN4NO3 | 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 | 25 | -25 | -1/25 (Δ[HNO3])/(Δt) Ca | 10 | -10 | -1/10 (Δ[Ca])/(Δt) H_2O | 12 | 12 | 1/12 (Δ[H2O])/(Δt) Ca(NO_3)_2 | 10 | 10 | 1/10 (Δ[Ca(NO3)2])/(Δt) HN4NO3 | 1 | 1 | (Δ[HN4NO3])/(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 = -1/25 (Δ[HNO3])/(Δt) = -1/10 (Δ[Ca])/(Δt) = 1/12 (Δ[H2O])/(Δt) = 1/10 (Δ[Ca(NO3)2])/(Δt) = (Δ[HN4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Ca ⟶ H_2O + Ca(NO_3)_2 + HN4NO3 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: 25 HNO_3 + 10 Ca ⟶ 12 H_2O + 10 Ca(NO_3)_2 + HN4NO3 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 | 25 | -25 Ca | 10 | -10 H_2O | 12 | 12 Ca(NO_3)_2 | 10 | 10 HN4NO3 | 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 | 25 | -25 | -1/25 (Δ[HNO3])/(Δt) Ca | 10 | -10 | -1/10 (Δ[Ca])/(Δt) H_2O | 12 | 12 | 1/12 (Δ[H2O])/(Δt) Ca(NO_3)_2 | 10 | 10 | 1/10 (Δ[Ca(NO3)2])/(Δt) HN4NO3 | 1 | 1 | (Δ[HN4NO3])/(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 = -1/25 (Δ[HNO3])/(Δt) = -1/10 (Δ[Ca])/(Δt) = 1/12 (Δ[H2O])/(Δt) = 1/10 (Δ[Ca(NO3)2])/(Δt) = (Δ[HN4NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | calcium | water | calcium nitrate | HN4NO3 formula | HNO_3 | Ca | H_2O | Ca(NO_3)_2 | HN4NO3 Hill formula | HNO_3 | Ca | H_2O | CaN_2O_6 | HN5O3 name | nitric acid | calcium | water | calcium nitrate | IUPAC name | nitric acid | calcium | water | calcium dinitrate |
| nitric acid | calcium | water | calcium nitrate | HN4NO3 formula | HNO_3 | Ca | H_2O | Ca(NO_3)_2 | HN4NO3 Hill formula | HNO_3 | Ca | H_2O | CaN_2O_6 | HN5O3 name | nitric acid | calcium | water | calcium nitrate | IUPAC name | nitric acid | calcium | water | calcium dinitrate |

Substance properties

| nitric acid | calcium | water | calcium nitrate | HN4NO3 molar mass | 63.012 g/mol | 40.078 g/mol | 18.015 g/mol | 164.09 g/mol | 119.04 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | -41.6 °C | 850 °C | 0 °C | 562 °C | boiling point | 83 °C | 1484 °C | 99.9839 °C | | density | 1.5129 g/cm^3 | 1.54 g/cm^3 | 1 g/cm^3 | 2.5 g/cm^3 | solubility in water | miscible | decomposes | | soluble | surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |
| nitric acid | calcium | water | calcium nitrate | HN4NO3 molar mass | 63.012 g/mol | 40.078 g/mol | 18.015 g/mol | 164.09 g/mol | 119.04 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | -41.6 °C | 850 °C | 0 °C | 562 °C | boiling point | 83 °C | 1484 °C | 99.9839 °C | | density | 1.5129 g/cm^3 | 1.54 g/cm^3 | 1 g/cm^3 | 2.5 g/cm^3 | solubility in water | miscible | decomposes | | soluble | surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | |

Units

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