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H2SO4 + Ca = H2O + S + Ca2SO4

Input interpretation

H_2SO_4 sulfuric acid + Ca calcium ⟶ H_2O water + S mixed sulfur + Ca2SO4
H_2SO_4 sulfuric acid + Ca calcium ⟶ H_2O water + S mixed sulfur + Ca2SO4

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + Ca ⟶ H_2O + S + Ca2SO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Ca ⟶ c_3 H_2O + c_4 S + c_5 Ca2SO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Ca: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 4 c_5 S: | c_1 = c_4 + c_5 Ca: | c_2 = 2 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 6 c_3 = 4 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 6 Ca ⟶ 4 H_2O + S + 3 Ca2SO4
Balance the chemical equation algebraically: H_2SO_4 + Ca ⟶ H_2O + S + Ca2SO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Ca ⟶ c_3 H_2O + c_4 S + c_5 Ca2SO4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Ca: H: | 2 c_1 = 2 c_3 O: | 4 c_1 = c_3 + 4 c_5 S: | c_1 = c_4 + c_5 Ca: | c_2 = 2 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 6 c_3 = 4 c_4 = 1 c_5 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2SO_4 + 6 Ca ⟶ 4 H_2O + S + 3 Ca2SO4

Structures

+ ⟶ + + Ca2SO4
+ ⟶ + + Ca2SO4

Names

sulfuric acid + calcium ⟶ water + mixed sulfur + Ca2SO4
sulfuric acid + calcium ⟶ water + mixed sulfur + Ca2SO4

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + Ca ⟶ H_2O + S + Ca2SO4 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: 4 H_2SO_4 + 6 Ca ⟶ 4 H_2O + S + 3 Ca2SO4 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 H_2SO_4 | 4 | -4 Ca | 6 | -6 H_2O | 4 | 4 S | 1 | 1 Ca2SO4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) Ca | 6 | -6 | ([Ca])^(-6) H_2O | 4 | 4 | ([H2O])^4 S | 1 | 1 | [S] Ca2SO4 | 3 | 3 | ([Ca2SO4])^3 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 = ([H2SO4])^(-4) ([Ca])^(-6) ([H2O])^4 [S] ([Ca2SO4])^3 = (([H2O])^4 [S] ([Ca2SO4])^3)/(([H2SO4])^4 ([Ca])^6)
Construct the equilibrium constant, K, expression for: H_2SO_4 + Ca ⟶ H_2O + S + Ca2SO4 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: 4 H_2SO_4 + 6 Ca ⟶ 4 H_2O + S + 3 Ca2SO4 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 H_2SO_4 | 4 | -4 Ca | 6 | -6 H_2O | 4 | 4 S | 1 | 1 Ca2SO4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 4 | -4 | ([H2SO4])^(-4) Ca | 6 | -6 | ([Ca])^(-6) H_2O | 4 | 4 | ([H2O])^4 S | 1 | 1 | [S] Ca2SO4 | 3 | 3 | ([Ca2SO4])^3 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 = ([H2SO4])^(-4) ([Ca])^(-6) ([H2O])^4 [S] ([Ca2SO4])^3 = (([H2O])^4 [S] ([Ca2SO4])^3)/(([H2SO4])^4 ([Ca])^6)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + Ca ⟶ H_2O + S + Ca2SO4 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: 4 H_2SO_4 + 6 Ca ⟶ 4 H_2O + S + 3 Ca2SO4 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 H_2SO_4 | 4 | -4 Ca | 6 | -6 H_2O | 4 | 4 S | 1 | 1 Ca2SO4 | 3 | 3 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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) Ca | 6 | -6 | -1/6 (Δ[Ca])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Ca2SO4 | 3 | 3 | 1/3 (Δ[Ca2SO4])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -1/6 (Δ[Ca])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[S])/(Δt) = 1/3 (Δ[Ca2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + Ca ⟶ H_2O + S + Ca2SO4 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: 4 H_2SO_4 + 6 Ca ⟶ 4 H_2O + S + 3 Ca2SO4 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 H_2SO_4 | 4 | -4 Ca | 6 | -6 H_2O | 4 | 4 S | 1 | 1 Ca2SO4 | 3 | 3 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 H_2SO_4 | 4 | -4 | -1/4 (Δ[H2SO4])/(Δt) Ca | 6 | -6 | -1/6 (Δ[Ca])/(Δt) H_2O | 4 | 4 | 1/4 (Δ[H2O])/(Δt) S | 1 | 1 | (Δ[S])/(Δt) Ca2SO4 | 3 | 3 | 1/3 (Δ[Ca2SO4])/(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 = -1/4 (Δ[H2SO4])/(Δt) = -1/6 (Δ[Ca])/(Δt) = 1/4 (Δ[H2O])/(Δt) = (Δ[S])/(Δt) = 1/3 (Δ[Ca2SO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | calcium | water | mixed sulfur | Ca2SO4 formula | H_2SO_4 | Ca | H_2O | S | Ca2SO4 Hill formula | H_2O_4S | Ca | H_2O | S | Ca2O4S name | sulfuric acid | calcium | water | mixed sulfur | IUPAC name | sulfuric acid | calcium | water | sulfur |
| sulfuric acid | calcium | water | mixed sulfur | Ca2SO4 formula | H_2SO_4 | Ca | H_2O | S | Ca2SO4 Hill formula | H_2O_4S | Ca | H_2O | S | Ca2O4S name | sulfuric acid | calcium | water | mixed sulfur | IUPAC name | sulfuric acid | calcium | water | sulfur |

Substance properties

| sulfuric acid | calcium | water | mixed sulfur | Ca2SO4 molar mass | 98.07 g/mol | 40.078 g/mol | 18.015 g/mol | 32.06 g/mol | 176.21 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 10.371 °C | 850 °C | 0 °C | 112.8 °C | boiling point | 279.6 °C | 1484 °C | 99.9839 °C | 444.7 °C | density | 1.8305 g/cm^3 | 1.54 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 | solubility in water | very soluble | decomposes | | | surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |
| sulfuric acid | calcium | water | mixed sulfur | Ca2SO4 molar mass | 98.07 g/mol | 40.078 g/mol | 18.015 g/mol | 32.06 g/mol | 176.21 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | melting point | 10.371 °C | 850 °C | 0 °C | 112.8 °C | boiling point | 279.6 °C | 1484 °C | 99.9839 °C | 444.7 °C | density | 1.8305 g/cm^3 | 1.54 g/cm^3 | 1 g/cm^3 | 2.07 g/cm^3 | solubility in water | very soluble | decomposes | | | surface tension | 0.0735 N/m | | 0.0728 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | odorless | | odorless | |

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