Search

Zn(OH)2 + H2CrO4 = H2O + ZnCrO4

Input interpretation

Zn(OH)_2 zinc hydroxide + H_2CrO_4 chromic acid ⟶ H_2O water + ZnCrO_4 zinc chromate
Zn(OH)_2 zinc hydroxide + H_2CrO_4 chromic acid ⟶ H_2O water + ZnCrO_4 zinc chromate

Balanced equation

Balance the chemical equation algebraically: Zn(OH)_2 + H_2CrO_4 ⟶ H_2O + ZnCrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn(OH)_2 + c_2 H_2CrO_4 ⟶ c_3 H_2O + c_4 ZnCrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Zn and Cr: H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 2 c_1 + 4 c_2 = c_3 + 4 c_4 Zn: | c_1 = c_4 Cr: | 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: | | Zn(OH)_2 + H_2CrO_4 ⟶ 2 H_2O + ZnCrO_4
Balance the chemical equation algebraically: Zn(OH)_2 + H_2CrO_4 ⟶ H_2O + ZnCrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Zn(OH)_2 + c_2 H_2CrO_4 ⟶ c_3 H_2O + c_4 ZnCrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Zn and Cr: H: | 2 c_1 + 2 c_2 = 2 c_3 O: | 2 c_1 + 4 c_2 = c_3 + 4 c_4 Zn: | c_1 = c_4 Cr: | 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: | | Zn(OH)_2 + H_2CrO_4 ⟶ 2 H_2O + ZnCrO_4

Structures

+ ⟶ +
+ ⟶ +

Names

zinc hydroxide + chromic acid ⟶ water + zinc chromate
zinc hydroxide + chromic acid ⟶ water + zinc chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: Zn(OH)_2 + H_2CrO_4 ⟶ H_2O + ZnCrO_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: Zn(OH)_2 + H_2CrO_4 ⟶ 2 H_2O + ZnCrO_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 Zn(OH)_2 | 1 | -1 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 ZnCrO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn(OH)_2 | 1 | -1 | ([Zn(OH)2])^(-1) H_2CrO_4 | 1 | -1 | ([H2CrO4])^(-1) H_2O | 2 | 2 | ([H2O])^2 ZnCrO_4 | 1 | 1 | [ZnCrO4] 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 = ([Zn(OH)2])^(-1) ([H2CrO4])^(-1) ([H2O])^2 [ZnCrO4] = (([H2O])^2 [ZnCrO4])/([Zn(OH)2] [H2CrO4])
Construct the equilibrium constant, K, expression for: Zn(OH)_2 + H_2CrO_4 ⟶ H_2O + ZnCrO_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: Zn(OH)_2 + H_2CrO_4 ⟶ 2 H_2O + ZnCrO_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 Zn(OH)_2 | 1 | -1 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 ZnCrO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Zn(OH)_2 | 1 | -1 | ([Zn(OH)2])^(-1) H_2CrO_4 | 1 | -1 | ([H2CrO4])^(-1) H_2O | 2 | 2 | ([H2O])^2 ZnCrO_4 | 1 | 1 | [ZnCrO4] 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 = ([Zn(OH)2])^(-1) ([H2CrO4])^(-1) ([H2O])^2 [ZnCrO4] = (([H2O])^2 [ZnCrO4])/([Zn(OH)2] [H2CrO4])

Rate of reaction

Construct the rate of reaction expression for: Zn(OH)_2 + H_2CrO_4 ⟶ H_2O + ZnCrO_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: Zn(OH)_2 + H_2CrO_4 ⟶ 2 H_2O + ZnCrO_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 Zn(OH)_2 | 1 | -1 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 ZnCrO_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 Zn(OH)_2 | 1 | -1 | -(Δ[Zn(OH)2])/(Δt) H_2CrO_4 | 1 | -1 | -(Δ[H2CrO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) ZnCrO_4 | 1 | 1 | (Δ[ZnCrO4])/(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[Zn(OH)2])/(Δt) = -(Δ[H2CrO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[ZnCrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Zn(OH)_2 + H_2CrO_4 ⟶ H_2O + ZnCrO_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: Zn(OH)_2 + H_2CrO_4 ⟶ 2 H_2O + ZnCrO_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 Zn(OH)_2 | 1 | -1 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 ZnCrO_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 Zn(OH)_2 | 1 | -1 | -(Δ[Zn(OH)2])/(Δt) H_2CrO_4 | 1 | -1 | -(Δ[H2CrO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) ZnCrO_4 | 1 | 1 | (Δ[ZnCrO4])/(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[Zn(OH)2])/(Δt) = -(Δ[H2CrO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[ZnCrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| zinc hydroxide | chromic acid | water | zinc chromate formula | Zn(OH)_2 | H_2CrO_4 | H_2O | ZnCrO_4 Hill formula | H_2O_2Zn | CrH_2O_4 | H_2O | CrO_4Zn name | zinc hydroxide | chromic acid | water | zinc chromate IUPAC name | zinc dihydroxide | dihydroxy-dioxo-chromium | water | zinc dioxido-dioxo-chromium
| zinc hydroxide | chromic acid | water | zinc chromate formula | Zn(OH)_2 | H_2CrO_4 | H_2O | ZnCrO_4 Hill formula | H_2O_2Zn | CrH_2O_4 | H_2O | CrO_4Zn name | zinc hydroxide | chromic acid | water | zinc chromate IUPAC name | zinc dihydroxide | dihydroxy-dioxo-chromium | water | zinc dioxido-dioxo-chromium

Substance properties

| zinc hydroxide | chromic acid | water | zinc chromate molar mass | 99.39 g/mol | 118.01 g/mol | 18.015 g/mol | 181.4 g/mol phase | | solid (at STP) | liquid (at STP) | solid (at STP) melting point | | 196 °C | 0 °C | 316 °C boiling point | | | 99.9839 °C | 732 °C density | | 2.7 g/cm^3 | 1 g/cm^3 | 3.43 g/cm^3 solubility in water | | very soluble | | insoluble surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |
| zinc hydroxide | chromic acid | water | zinc chromate molar mass | 99.39 g/mol | 118.01 g/mol | 18.015 g/mol | 181.4 g/mol phase | | solid (at STP) | liquid (at STP) | solid (at STP) melting point | | 196 °C | 0 °C | 316 °C boiling point | | | 99.9839 °C | 732 °C density | | 2.7 g/cm^3 | 1 g/cm^3 | 3.43 g/cm^3 solubility in water | | very soluble | | insoluble surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |

Units

Random Queries

alternate names of tryptamine functional group
color of minguzzite vs wheatleyite
alternate names of 3-iodo-4,5-dimethoxybenzaldehyde
melting point of sodium erythorbate
CO2 + ZnO = ZnCO3
phase of butyric acid vs 2-(trimethylammonium)ethyl thiol
molar mass of p-anisylboronic acid vs vanadium cyclopentadienyldilactate
net ionic charge of osmide
emboss image iron
alternate names of uvite vs melilite