Search

H2O2 + CaOCl2 = H2O + O2 + CaCl2

Input interpretation

H_2O_2 hydrogen peroxide + CaOCl2 ⟶ H_2O water + O_2 oxygen + CaCl_2 calcium chloride
H_2O_2 hydrogen peroxide + CaOCl2 ⟶ H_2O water + O_2 oxygen + CaCl_2 calcium chloride

Balanced equation

Balance the chemical equation algebraically: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 CaOCl2 ⟶ c_3 H_2O + c_4 O_2 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ca and Cl: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + c_2 = c_3 + 2 c_4 Ca: | c_2 = c_5 Cl: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 1 c_4 = c_2/2 + 1/2 c_5 = c_2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 1 and solve for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + CaCl_2
Balance the chemical equation algebraically: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + CaCl_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O_2 + c_2 CaOCl2 ⟶ c_3 H_2O + c_4 O_2 + c_5 CaCl_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Ca and Cl: H: | 2 c_1 = 2 c_3 O: | 2 c_1 + c_2 = c_3 + 2 c_4 Ca: | c_2 = c_5 Cl: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_3 = 1 c_4 = c_2/2 + 1/2 c_5 = c_2 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_2 = 1 and solve for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + CaCl_2

Structures

+ CaOCl2 ⟶ + +
+ CaOCl2 ⟶ + +

Names

hydrogen peroxide + CaOCl2 ⟶ water + oxygen + calcium chloride
hydrogen peroxide + CaOCl2 ⟶ water + oxygen + calcium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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 | 1 | -1 CaOCl2 | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 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 | 1 | -1 | ([H2O2])^(-1) CaOCl2 | 1 | -1 | ([CaOCl2])^(-1) H_2O | 1 | 1 | [H2O] O_2 | 1 | 1 | [O2] 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 = ([H2O2])^(-1) ([CaOCl2])^(-1) [H2O] [O2] [CaCl2] = ([H2O] [O2] [CaCl2])/([H2O2] [CaOCl2])
Construct the equilibrium constant, K, expression for: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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 | 1 | -1 CaOCl2 | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 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 | 1 | -1 | ([H2O2])^(-1) CaOCl2 | 1 | -1 | ([CaOCl2])^(-1) H_2O | 1 | 1 | [H2O] O_2 | 1 | 1 | [O2] 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 = ([H2O2])^(-1) ([CaOCl2])^(-1) [H2O] [O2] [CaCl2] = ([H2O] [O2] [CaCl2])/([H2O2] [CaOCl2])

Rate of reaction

Construct the rate of reaction expression for: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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 | 1 | -1 CaOCl2 | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 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 | 1 | -1 | -(Δ[H2O2])/(Δt) CaOCl2 | 1 | -1 | -(Δ[CaOCl2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(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 = -(Δ[H2O2])/(Δt) = -(Δ[CaOCl2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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: H_2O_2 + CaOCl2 ⟶ H_2O + O_2 + 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 | 1 | -1 CaOCl2 | 1 | -1 H_2O | 1 | 1 O_2 | 1 | 1 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 | 1 | -1 | -(Δ[H2O2])/(Δt) CaOCl2 | 1 | -1 | -(Δ[CaOCl2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(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 = -(Δ[H2O2])/(Δt) = -(Δ[CaOCl2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = (Δ[CaCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen peroxide | CaOCl2 | water | oxygen | calcium chloride formula | H_2O_2 | CaOCl2 | H_2O | O_2 | CaCl_2 Hill formula | H_2O_2 | CaCl2O | H_2O | O_2 | CaCl_2 name | hydrogen peroxide | | water | oxygen | calcium chloride IUPAC name | hydrogen peroxide | | water | molecular oxygen | calcium dichloride
| hydrogen peroxide | CaOCl2 | water | oxygen | calcium chloride formula | H_2O_2 | CaOCl2 | H_2O | O_2 | CaCl_2 Hill formula | H_2O_2 | CaCl2O | H_2O | O_2 | CaCl_2 name | hydrogen peroxide | | water | oxygen | calcium chloride IUPAC name | hydrogen peroxide | | water | molecular oxygen | calcium dichloride

Substance properties

| hydrogen peroxide | CaOCl2 | water | oxygen | calcium chloride molar mass | 34.014 g/mol | 127 g/mol | 18.015 g/mol | 31.998 g/mol | 111 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -0.43 °C | | 0 °C | -218 °C | 772 °C boiling point | 150.2 °C | | 99.9839 °C | -183 °C | density | 1.44 g/cm^3 | | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 2.15 g/cm^3 solubility in water | miscible | | | | soluble surface tension | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |
| hydrogen peroxide | CaOCl2 | water | oxygen | calcium chloride molar mass | 34.014 g/mol | 127 g/mol | 18.015 g/mol | 31.998 g/mol | 111 g/mol phase | liquid (at STP) | | liquid (at STP) | gas (at STP) | solid (at STP) melting point | -0.43 °C | | 0 °C | -218 °C | 772 °C boiling point | 150.2 °C | | 99.9839 °C | -183 °C | density | 1.44 g/cm^3 | | 1 g/cm^3 | 0.001429 g/cm^3 (at 0 °C) | 2.15 g/cm^3 solubility in water | miscible | | | | soluble surface tension | 0.0804 N/m | | 0.0728 N/m | 0.01347 N/m | dynamic viscosity | 0.001249 Pa s (at 20 °C) | | 8.9×10^-4 Pa s (at 25 °C) | 2.055×10^-5 Pa s (at 25 °C) | odor | | | odorless | odorless |

Units

Random Queries

hydrogen carbonate anion vs copper(II) cation vs iodide anion
formula of tetrahydrogenorthotellurate anion
absolute boiling point of group 4 elements
H2 + MoO = H2O + Mo
prices of platinum metals
chemical types of lithium cobalt(III) oxide vs lM seed protectant
boiling point of molybdenum trioxide
phase of iodotrimethylsilane
net ionic charge of hexaiodoplatinate(IV) anion
name of calcium nitrate vs zirconium(II) iodide