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H2O + SO2 + Ca(ClO)2 = H2SO4 + CaCl2

Input interpretation

H_2O water + SO_2 sulfur dioxide + Ca(ClO)2 ⟶ H_2SO_4 sulfuric acid + CaCl_2 calcium chloride
H_2O water + SO_2 sulfur dioxide + Ca(ClO)2 ⟶ H_2SO_4 sulfuric acid + CaCl_2 calcium chloride

Balanced equation

Balance the chemical equation algebraically: H_2O + SO_2 + Ca(ClO)2 ⟶ H_2SO_4 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 Ca(ClO)2 ⟶ c_4 H_2SO_4 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Ca and Cl: H: | 2 c_1 = 2 c_4 O: | c_1 + 2 c_2 + 2 c_3 = 4 c_4 S: | c_2 = c_4 Ca: | c_3 = c_5 Cl: | 2 c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 SO_2 + Ca(ClO)2 ⟶ 2 H_2SO_4 + CaCl_2
Balance the chemical equation algebraically: H_2O + SO_2 + Ca(ClO)2 ⟶ H_2SO_4 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 SO_2 + c_3 Ca(ClO)2 ⟶ c_4 H_2SO_4 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Ca and Cl: H: | 2 c_1 = 2 c_4 O: | c_1 + 2 c_2 + 2 c_3 = 4 c_4 S: | c_2 = c_4 Ca: | c_3 = c_5 Cl: | 2 c_3 = 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 SO_2 + Ca(ClO)2 ⟶ 2 H_2SO_4 + CaCl_2

Structures

+ + Ca(ClO)2 ⟶ +
+ + Ca(ClO)2 ⟶ +

Names

water + sulfur dioxide + Ca(ClO)2 ⟶ sulfuric acid + calcium chloride
water + sulfur dioxide + Ca(ClO)2 ⟶ sulfuric acid + calcium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + SO_2 + Ca(ClO)2 ⟶ H_2SO_4 + CaCl_2 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 H_2O + 2 SO_2 + Ca(ClO)2 ⟶ 2 H_2SO_4 + CaCl_2 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_2O | 2 | -2 SO_2 | 2 | -2 Ca(ClO)2 | 1 | -1 H_2SO_4 | 2 | 2 CaCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) SO_2 | 2 | -2 | ([SO2])^(-2) Ca(ClO)2 | 1 | -1 | ([Ca(ClO)2])^(-1) H_2SO_4 | 2 | 2 | ([H2SO4])^2 CaCl_2 | 1 | 1 | [CaCl2] 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 = ([H2O])^(-2) ([SO2])^(-2) ([Ca(ClO)2])^(-1) ([H2SO4])^2 [CaCl2] = (([H2SO4])^2 [CaCl2])/(([H2O])^2 ([SO2])^2 [Ca(ClO)2])
Construct the equilibrium constant, K, expression for: H_2O + SO_2 + Ca(ClO)2 ⟶ H_2SO_4 + CaCl_2 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 H_2O + 2 SO_2 + Ca(ClO)2 ⟶ 2 H_2SO_4 + CaCl_2 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_2O | 2 | -2 SO_2 | 2 | -2 Ca(ClO)2 | 1 | -1 H_2SO_4 | 2 | 2 CaCl_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) SO_2 | 2 | -2 | ([SO2])^(-2) Ca(ClO)2 | 1 | -1 | ([Ca(ClO)2])^(-1) H_2SO_4 | 2 | 2 | ([H2SO4])^2 CaCl_2 | 1 | 1 | [CaCl2] 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 = ([H2O])^(-2) ([SO2])^(-2) ([Ca(ClO)2])^(-1) ([H2SO4])^2 [CaCl2] = (([H2SO4])^2 [CaCl2])/(([H2O])^2 ([SO2])^2 [Ca(ClO)2])

Rate of reaction

Construct the rate of reaction expression for: H_2O + SO_2 + Ca(ClO)2 ⟶ H_2SO_4 + CaCl_2 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 H_2O + 2 SO_2 + Ca(ClO)2 ⟶ 2 H_2SO_4 + CaCl_2 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_2O | 2 | -2 SO_2 | 2 | -2 Ca(ClO)2 | 1 | -1 H_2SO_4 | 2 | 2 CaCl_2 | 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) SO_2 | 2 | -2 | -1/2 (Δ[SO2])/(Δt) Ca(ClO)2 | 1 | -1 | -(Δ[Ca(ClO)2])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) CaCl_2 | 1 | 1 | (Δ[CaCl2])/(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[H2O])/(Δt) = -1/2 (Δ[SO2])/(Δt) = -(Δ[Ca(ClO)2])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + SO_2 + Ca(ClO)2 ⟶ H_2SO_4 + CaCl_2 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 H_2O + 2 SO_2 + Ca(ClO)2 ⟶ 2 H_2SO_4 + CaCl_2 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_2O | 2 | -2 SO_2 | 2 | -2 Ca(ClO)2 | 1 | -1 H_2SO_4 | 2 | 2 CaCl_2 | 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) SO_2 | 2 | -2 | -1/2 (Δ[SO2])/(Δt) Ca(ClO)2 | 1 | -1 | -(Δ[Ca(ClO)2])/(Δt) H_2SO_4 | 2 | 2 | 1/2 (Δ[H2SO4])/(Δt) CaCl_2 | 1 | 1 | (Δ[CaCl2])/(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[H2O])/(Δt) = -1/2 (Δ[SO2])/(Δt) = -(Δ[Ca(ClO)2])/(Δt) = 1/2 (Δ[H2SO4])/(Δt) = (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | sulfur dioxide | Ca(ClO)2 | sulfuric acid | calcium chloride formula | H_2O | SO_2 | Ca(ClO)2 | H_2SO_4 | CaCl_2 Hill formula | H_2O | O_2S | CaCl2O2 | H_2O_4S | CaCl_2 name | water | sulfur dioxide | | sulfuric acid | calcium chloride IUPAC name | water | sulfur dioxide | | sulfuric acid | calcium dichloride
| water | sulfur dioxide | Ca(ClO)2 | sulfuric acid | calcium chloride formula | H_2O | SO_2 | Ca(ClO)2 | H_2SO_4 | CaCl_2 Hill formula | H_2O | O_2S | CaCl2O2 | H_2O_4S | CaCl_2 name | water | sulfur dioxide | | sulfuric acid | calcium chloride IUPAC name | water | sulfur dioxide | | sulfuric acid | calcium dichloride

Substance properties

| water | sulfur dioxide | Ca(ClO)2 | sulfuric acid | calcium chloride molar mass | 18.015 g/mol | 64.06 g/mol | 143 g/mol | 98.07 g/mol | 111 g/mol phase | liquid (at STP) | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | 0 °C | -73 °C | | 10.371 °C | 772 °C boiling point | 99.9839 °C | -10 °C | | 279.6 °C | density | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | | 1.8305 g/cm^3 | 2.15 g/cm^3 solubility in water | | | | very soluble | soluble surface tension | 0.0728 N/m | 0.02859 N/m | | 0.0735 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | odor | odorless | | | odorless |
| water | sulfur dioxide | Ca(ClO)2 | sulfuric acid | calcium chloride molar mass | 18.015 g/mol | 64.06 g/mol | 143 g/mol | 98.07 g/mol | 111 g/mol phase | liquid (at STP) | gas (at STP) | | liquid (at STP) | solid (at STP) melting point | 0 °C | -73 °C | | 10.371 °C | 772 °C boiling point | 99.9839 °C | -10 °C | | 279.6 °C | density | 1 g/cm^3 | 0.002619 g/cm^3 (at 25 °C) | | 1.8305 g/cm^3 | 2.15 g/cm^3 solubility in water | | | | very soluble | soluble surface tension | 0.0728 N/m | 0.02859 N/m | | 0.0735 N/m | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | 1.282×10^-5 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | odor | odorless | | | odorless |

Units

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H2SO4 + K2Cr2O7 + SnCl2 = H2O + K2SO4 + CrCl3 + Sn(SO4)2