Search

NaOH + Br2 + Na[Cr(OH)4(H2O)2] = H2O + NaBr + Na2CrO4

Input interpretation

NaOH sodium hydroxide + Br_2 bromine + NaCr(OH)4(H2O)2 ⟶ H_2O water + NaBr sodium bromide + Na_2CrO_4 sodium chromate
NaOH sodium hydroxide + Br_2 bromine + NaCr(OH)4(H2O)2 ⟶ H_2O water + NaBr sodium bromide + Na_2CrO_4 sodium chromate

Balanced equation

Balance the chemical equation algebraically: NaOH + Br_2 + NaCr(OH)4(H2O)2 ⟶ H_2O + NaBr + Na_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Br_2 + c_3 NaCr(OH)4(H2O)2 ⟶ c_4 H_2O + c_5 NaBr + c_6 Na_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Br and Cr: H: | c_1 + 8 c_3 = 2 c_4 Na: | c_1 + c_3 = c_5 + 2 c_6 O: | c_1 + 6 c_3 = c_4 + 4 c_6 Br: | 2 c_2 = c_5 Cr: | c_3 = c_6 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 = 4 c_2 = 3/2 c_3 = 1 c_4 = 6 c_5 = 3 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 3 c_3 = 2 c_4 = 12 c_5 = 6 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 NaOH + 3 Br_2 + 2 NaCr(OH)4(H2O)2 ⟶ 12 H_2O + 6 NaBr + 2 Na_2CrO_4
Balance the chemical equation algebraically: NaOH + Br_2 + NaCr(OH)4(H2O)2 ⟶ H_2O + NaBr + Na_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Br_2 + c_3 NaCr(OH)4(H2O)2 ⟶ c_4 H_2O + c_5 NaBr + c_6 Na_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Br and Cr: H: | c_1 + 8 c_3 = 2 c_4 Na: | c_1 + c_3 = c_5 + 2 c_6 O: | c_1 + 6 c_3 = c_4 + 4 c_6 Br: | 2 c_2 = c_5 Cr: | c_3 = c_6 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 = 4 c_2 = 3/2 c_3 = 1 c_4 = 6 c_5 = 3 c_6 = 1 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 8 c_2 = 3 c_3 = 2 c_4 = 12 c_5 = 6 c_6 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 8 NaOH + 3 Br_2 + 2 NaCr(OH)4(H2O)2 ⟶ 12 H_2O + 6 NaBr + 2 Na_2CrO_4

Structures

+ + NaCr(OH)4(H2O)2 ⟶ + +
+ + NaCr(OH)4(H2O)2 ⟶ + +

Names

sodium hydroxide + bromine + NaCr(OH)4(H2O)2 ⟶ water + sodium bromide + sodium chromate
sodium hydroxide + bromine + NaCr(OH)4(H2O)2 ⟶ water + sodium bromide + sodium chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + Br_2 + NaCr(OH)4(H2O)2 ⟶ H_2O + NaBr + Na_2CrO_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: 8 NaOH + 3 Br_2 + 2 NaCr(OH)4(H2O)2 ⟶ 12 H_2O + 6 NaBr + 2 Na_2CrO_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 NaOH | 8 | -8 Br_2 | 3 | -3 NaCr(OH)4(H2O)2 | 2 | -2 H_2O | 12 | 12 NaBr | 6 | 6 Na_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 8 | -8 | ([NaOH])^(-8) Br_2 | 3 | -3 | ([Br2])^(-3) NaCr(OH)4(H2O)2 | 2 | -2 | ([NaCr(OH)4(H2O)2])^(-2) H_2O | 12 | 12 | ([H2O])^12 NaBr | 6 | 6 | ([NaBr])^6 Na_2CrO_4 | 2 | 2 | ([Na2CrO4])^2 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 = ([NaOH])^(-8) ([Br2])^(-3) ([NaCr(OH)4(H2O)2])^(-2) ([H2O])^12 ([NaBr])^6 ([Na2CrO4])^2 = (([H2O])^12 ([NaBr])^6 ([Na2CrO4])^2)/(([NaOH])^8 ([Br2])^3 ([NaCr(OH)4(H2O)2])^2)
Construct the equilibrium constant, K, expression for: NaOH + Br_2 + NaCr(OH)4(H2O)2 ⟶ H_2O + NaBr + Na_2CrO_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: 8 NaOH + 3 Br_2 + 2 NaCr(OH)4(H2O)2 ⟶ 12 H_2O + 6 NaBr + 2 Na_2CrO_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 NaOH | 8 | -8 Br_2 | 3 | -3 NaCr(OH)4(H2O)2 | 2 | -2 H_2O | 12 | 12 NaBr | 6 | 6 Na_2CrO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 8 | -8 | ([NaOH])^(-8) Br_2 | 3 | -3 | ([Br2])^(-3) NaCr(OH)4(H2O)2 | 2 | -2 | ([NaCr(OH)4(H2O)2])^(-2) H_2O | 12 | 12 | ([H2O])^12 NaBr | 6 | 6 | ([NaBr])^6 Na_2CrO_4 | 2 | 2 | ([Na2CrO4])^2 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 = ([NaOH])^(-8) ([Br2])^(-3) ([NaCr(OH)4(H2O)2])^(-2) ([H2O])^12 ([NaBr])^6 ([Na2CrO4])^2 = (([H2O])^12 ([NaBr])^6 ([Na2CrO4])^2)/(([NaOH])^8 ([Br2])^3 ([NaCr(OH)4(H2O)2])^2)

Rate of reaction

Construct the rate of reaction expression for: NaOH + Br_2 + NaCr(OH)4(H2O)2 ⟶ H_2O + NaBr + Na_2CrO_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: 8 NaOH + 3 Br_2 + 2 NaCr(OH)4(H2O)2 ⟶ 12 H_2O + 6 NaBr + 2 Na_2CrO_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 NaOH | 8 | -8 Br_2 | 3 | -3 NaCr(OH)4(H2O)2 | 2 | -2 H_2O | 12 | 12 NaBr | 6 | 6 Na_2CrO_4 | 2 | 2 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 NaOH | 8 | -8 | -1/8 (Δ[NaOH])/(Δt) Br_2 | 3 | -3 | -1/3 (Δ[Br2])/(Δt) NaCr(OH)4(H2O)2 | 2 | -2 | -1/2 (Δ[NaCr(OH)4(H2O)2])/(Δt) H_2O | 12 | 12 | 1/12 (Δ[H2O])/(Δt) NaBr | 6 | 6 | 1/6 (Δ[NaBr])/(Δt) Na_2CrO_4 | 2 | 2 | 1/2 (Δ[Na2CrO4])/(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 = -1/8 (Δ[NaOH])/(Δt) = -1/3 (Δ[Br2])/(Δt) = -1/2 (Δ[NaCr(OH)4(H2O)2])/(Δt) = 1/12 (Δ[H2O])/(Δt) = 1/6 (Δ[NaBr])/(Δt) = 1/2 (Δ[Na2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + Br_2 + NaCr(OH)4(H2O)2 ⟶ H_2O + NaBr + Na_2CrO_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: 8 NaOH + 3 Br_2 + 2 NaCr(OH)4(H2O)2 ⟶ 12 H_2O + 6 NaBr + 2 Na_2CrO_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 NaOH | 8 | -8 Br_2 | 3 | -3 NaCr(OH)4(H2O)2 | 2 | -2 H_2O | 12 | 12 NaBr | 6 | 6 Na_2CrO_4 | 2 | 2 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 NaOH | 8 | -8 | -1/8 (Δ[NaOH])/(Δt) Br_2 | 3 | -3 | -1/3 (Δ[Br2])/(Δt) NaCr(OH)4(H2O)2 | 2 | -2 | -1/2 (Δ[NaCr(OH)4(H2O)2])/(Δt) H_2O | 12 | 12 | 1/12 (Δ[H2O])/(Δt) NaBr | 6 | 6 | 1/6 (Δ[NaBr])/(Δt) Na_2CrO_4 | 2 | 2 | 1/2 (Δ[Na2CrO4])/(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 = -1/8 (Δ[NaOH])/(Δt) = -1/3 (Δ[Br2])/(Δt) = -1/2 (Δ[NaCr(OH)4(H2O)2])/(Δt) = 1/12 (Δ[H2O])/(Δt) = 1/6 (Δ[NaBr])/(Δt) = 1/2 (Δ[Na2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | bromine | NaCr(OH)4(H2O)2 | water | sodium bromide | sodium chromate formula | NaOH | Br_2 | NaCr(OH)4(H2O)2 | H_2O | NaBr | Na_2CrO_4 Hill formula | HNaO | Br_2 | H8CrNaO6 | H_2O | BrNa | CrNa_2O_4 name | sodium hydroxide | bromine | | water | sodium bromide | sodium chromate IUPAC name | sodium hydroxide | molecular bromine | | water | sodium bromide | disodium dioxido(dioxo)chromium
| sodium hydroxide | bromine | NaCr(OH)4(H2O)2 | water | sodium bromide | sodium chromate formula | NaOH | Br_2 | NaCr(OH)4(H2O)2 | H_2O | NaBr | Na_2CrO_4 Hill formula | HNaO | Br_2 | H8CrNaO6 | H_2O | BrNa | CrNa_2O_4 name | sodium hydroxide | bromine | | water | sodium bromide | sodium chromate IUPAC name | sodium hydroxide | molecular bromine | | water | sodium bromide | disodium dioxido(dioxo)chromium

Substance properties

| sodium hydroxide | bromine | NaCr(OH)4(H2O)2 | water | sodium bromide | sodium chromate molar mass | 39.997 g/mol | 159.81 g/mol | 179.04 g/mol | 18.015 g/mol | 102.89 g/mol | 161.97 g/mol phase | solid (at STP) | liquid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | -7.2 °C | | 0 °C | 755 °C | 780 °C boiling point | 1390 °C | 58.8 °C | | 99.9839 °C | 1396 °C | density | 2.13 g/cm^3 | 3.119 g/cm^3 | | 1 g/cm^3 | 3.2 g/cm^3 | 2.698 g/cm^3 solubility in water | soluble | insoluble | | | soluble | surface tension | 0.07435 N/m | 0.0409 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | 9.44×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | |
| sodium hydroxide | bromine | NaCr(OH)4(H2O)2 | water | sodium bromide | sodium chromate molar mass | 39.997 g/mol | 159.81 g/mol | 179.04 g/mol | 18.015 g/mol | 102.89 g/mol | 161.97 g/mol phase | solid (at STP) | liquid (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | -7.2 °C | | 0 °C | 755 °C | 780 °C boiling point | 1390 °C | 58.8 °C | | 99.9839 °C | 1396 °C | density | 2.13 g/cm^3 | 3.119 g/cm^3 | | 1 g/cm^3 | 3.2 g/cm^3 | 2.698 g/cm^3 solubility in water | soluble | insoluble | | | soluble | surface tension | 0.07435 N/m | 0.0409 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | 9.44×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | | odorless | |

Units

Random Queries

isotopes of mercury
atomic radius of aluminum vs iron
alternate names of nitrate anion vs fluoride anion
formula of succinate anion common
formula of bis(triphenylphosphoranylidene)ammonium chloride
chemical uses of dactinomycin
density of carbon vs fluorine
melting point of chloroacetic acid vs tartaric acid
decay modes of Ac-224
freezing point of tributylhexadecylphosphonium bromide