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Ca(NO3)2 + H2(SO4) = HNO3 + Ca(SO4)

Input interpretation

Ca(NO_3)_2 calcium nitrate + H_2SO_4 sulfuric acid ⟶ HNO_3 nitric acid + CaSO_4 calcium sulfate
Ca(NO_3)_2 calcium nitrate + H_2SO_4 sulfuric acid ⟶ HNO_3 nitric acid + CaSO_4 calcium sulfate

Balanced equation

Balance the chemical equation algebraically: Ca(NO_3)_2 + H_2SO_4 ⟶ HNO_3 + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(NO_3)_2 + c_2 H_2SO_4 ⟶ c_3 HNO_3 + c_4 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, N, O, H and S: Ca: | c_1 = c_4 N: | 2 c_1 = c_3 O: | 6 c_1 + 4 c_2 = 3 c_3 + 4 c_4 H: | 2 c_2 = c_3 S: | 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_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: |   | Ca(NO_3)_2 + H_2SO_4 ⟶ 2 HNO_3 + CaSO_4
Balance the chemical equation algebraically: Ca(NO_3)_2 + H_2SO_4 ⟶ HNO_3 + CaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Ca(NO_3)_2 + c_2 H_2SO_4 ⟶ c_3 HNO_3 + c_4 CaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, N, O, H and S: Ca: | c_1 = c_4 N: | 2 c_1 = c_3 O: | 6 c_1 + 4 c_2 = 3 c_3 + 4 c_4 H: | 2 c_2 = c_3 S: | 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_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: | | Ca(NO_3)_2 + H_2SO_4 ⟶ 2 HNO_3 + CaSO_4

Structures

 + ⟶ +
+ ⟶ +

Names

calcium nitrate + sulfuric acid ⟶ nitric acid + calcium sulfate
calcium nitrate + sulfuric acid ⟶ nitric acid + calcium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Ca(NO_3)_2 + H_2SO_4 ⟶ HNO_3 + CaSO_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: Ca(NO_3)_2 + H_2SO_4 ⟶ 2 HNO_3 + CaSO_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 Ca(NO_3)_2 | 1 | -1 H_2SO_4 | 1 | -1 HNO_3 | 2 | 2 CaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(NO_3)_2 | 1 | -1 | ([Ca(NO3)2])^(-1) H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 CaSO_4 | 1 | 1 | [CaSO4] 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 = ([Ca(NO3)2])^(-1) ([H2SO4])^(-1) ([HNO3])^2 [CaSO4] = (([HNO3])^2 [CaSO4])/([Ca(NO3)2] [H2SO4])
Construct the equilibrium constant, K, expression for: Ca(NO_3)_2 + H_2SO_4 ⟶ HNO_3 + CaSO_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: Ca(NO_3)_2 + H_2SO_4 ⟶ 2 HNO_3 + CaSO_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 Ca(NO_3)_2 | 1 | -1 H_2SO_4 | 1 | -1 HNO_3 | 2 | 2 CaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Ca(NO_3)_2 | 1 | -1 | ([Ca(NO3)2])^(-1) H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 CaSO_4 | 1 | 1 | [CaSO4] 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 = ([Ca(NO3)2])^(-1) ([H2SO4])^(-1) ([HNO3])^2 [CaSO4] = (([HNO3])^2 [CaSO4])/([Ca(NO3)2] [H2SO4])

Rate of reaction

Construct the rate of reaction expression for: Ca(NO_3)_2 + H_2SO_4 ⟶ HNO_3 + CaSO_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: Ca(NO_3)_2 + H_2SO_4 ⟶ 2 HNO_3 + CaSO_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 Ca(NO_3)_2 | 1 | -1 H_2SO_4 | 1 | -1 HNO_3 | 2 | 2 CaSO_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 Ca(NO_3)_2 | 1 | -1 | -(Δ[Ca(NO3)2])/(Δt) H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[Ca(NO3)2])/(Δt) = -(Δ[H2SO4])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Ca(NO_3)_2 + H_2SO_4 ⟶ HNO_3 + CaSO_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: Ca(NO_3)_2 + H_2SO_4 ⟶ 2 HNO_3 + CaSO_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 Ca(NO_3)_2 | 1 | -1 H_2SO_4 | 1 | -1 HNO_3 | 2 | 2 CaSO_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 Ca(NO_3)_2 | 1 | -1 | -(Δ[Ca(NO3)2])/(Δt) H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) CaSO_4 | 1 | 1 | (Δ[CaSO4])/(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[Ca(NO3)2])/(Δt) = -(Δ[H2SO4])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[CaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | calcium nitrate | sulfuric acid | nitric acid | calcium sulfate formula | Ca(NO_3)_2 | H_2SO_4 | HNO_3 | CaSO_4 Hill formula | CaN_2O_6 | H_2O_4S | HNO_3 | CaO_4S name | calcium nitrate | sulfuric acid | nitric acid | calcium sulfate IUPAC name | calcium dinitrate | sulfuric acid | nitric acid | calcium sulfate
| calcium nitrate | sulfuric acid | nitric acid | calcium sulfate formula | Ca(NO_3)_2 | H_2SO_4 | HNO_3 | CaSO_4 Hill formula | CaN_2O_6 | H_2O_4S | HNO_3 | CaO_4S name | calcium nitrate | sulfuric acid | nitric acid | calcium sulfate IUPAC name | calcium dinitrate | sulfuric acid | nitric acid | calcium sulfate

Substance properties

 | calcium nitrate | sulfuric acid | nitric acid | calcium sulfate molar mass | 164.09 g/mol | 98.07 g/mol | 63.012 g/mol | 136.13 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) |  melting point | 562 °C | 10.371 °C | -41.6 °C |  boiling point | | 279.6 °C | 83 °C |  density | 2.5 g/cm^3 | 1.8305 g/cm^3 | 1.5129 g/cm^3 |  solubility in water | soluble | very soluble | miscible | slightly soluble surface tension | | 0.0735 N/m | |  dynamic viscosity | | 0.021 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) |  odor | | odorless | | odorless
| calcium nitrate | sulfuric acid | nitric acid | calcium sulfate molar mass | 164.09 g/mol | 98.07 g/mol | 63.012 g/mol | 136.13 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | melting point | 562 °C | 10.371 °C | -41.6 °C | boiling point | | 279.6 °C | 83 °C | density | 2.5 g/cm^3 | 1.8305 g/cm^3 | 1.5129 g/cm^3 | solubility in water | soluble | very soluble | miscible | slightly soluble surface tension | | 0.0735 N/m | | dynamic viscosity | | 0.021 Pa s (at 25 °C) | 7.6×10^-4 Pa s (at 25 °C) | odor | | odorless | | odorless

Units