Input interpretation
![Cr(OH)2 ⟶ H_2O water + CrO](../image_source/7ee557b6b2277e1919a5c40512307e3b.png)
Cr(OH)2 ⟶ H_2O water + CrO
Balanced equation
![Balance the chemical equation algebraically: Cr(OH)2 ⟶ H_2O + CrO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cr(OH)2 ⟶ c_2 H_2O + c_3 CrO Set the number of atoms in the reactants equal to the number of atoms in the products for Cr, O and H: Cr: | c_1 = c_3 O: | 2 c_1 = c_2 + c_3 H: | 2 c_1 = 2 c_2 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cr(OH)2 ⟶ H_2O + CrO](../image_source/8353df8b45a71707f7e36b1250808216.png)
Balance the chemical equation algebraically: Cr(OH)2 ⟶ H_2O + CrO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cr(OH)2 ⟶ c_2 H_2O + c_3 CrO Set the number of atoms in the reactants equal to the number of atoms in the products for Cr, O and H: Cr: | c_1 = c_3 O: | 2 c_1 = c_2 + c_3 H: | 2 c_1 = 2 c_2 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 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cr(OH)2 ⟶ H_2O + CrO
Structures
![Cr(OH)2 ⟶ + CrO](../image_source/fa9e04e3e41f022530dc5149dd50131a.png)
Cr(OH)2 ⟶ + CrO
Names
![Cr(OH)2 ⟶ water + CrO](../image_source/3774a03cd5c56cc5c5256204ba0d2c99.png)
Cr(OH)2 ⟶ water + CrO
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Cr(OH)2 ⟶ H_2O + CrO 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: Cr(OH)2 ⟶ H_2O + CrO 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 Cr(OH)2 | 1 | -1 H_2O | 1 | 1 CrO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cr(OH)2 | 1 | -1 | ([Cr(OH)2])^(-1) H_2O | 1 | 1 | [H2O] CrO | 1 | 1 | [CrO] 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 = ([Cr(OH)2])^(-1) [H2O] [CrO] = ([H2O] [CrO])/([Cr(OH)2])](../image_source/5aa04499cd97d4799a3c49d99850c212.png)
Construct the equilibrium constant, K, expression for: Cr(OH)2 ⟶ H_2O + CrO 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: Cr(OH)2 ⟶ H_2O + CrO 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 Cr(OH)2 | 1 | -1 H_2O | 1 | 1 CrO | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cr(OH)2 | 1 | -1 | ([Cr(OH)2])^(-1) H_2O | 1 | 1 | [H2O] CrO | 1 | 1 | [CrO] 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 = ([Cr(OH)2])^(-1) [H2O] [CrO] = ([H2O] [CrO])/([Cr(OH)2])
Rate of reaction
![Construct the rate of reaction expression for: Cr(OH)2 ⟶ H_2O + CrO 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: Cr(OH)2 ⟶ H_2O + CrO 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 Cr(OH)2 | 1 | -1 H_2O | 1 | 1 CrO | 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 Cr(OH)2 | 1 | -1 | -(Δ[Cr(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CrO | 1 | 1 | (Δ[CrO])/(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[Cr(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CrO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/1640b30b9338905e524be2632e20b03e.png)
Construct the rate of reaction expression for: Cr(OH)2 ⟶ H_2O + CrO 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: Cr(OH)2 ⟶ H_2O + CrO 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 Cr(OH)2 | 1 | -1 H_2O | 1 | 1 CrO | 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 Cr(OH)2 | 1 | -1 | -(Δ[Cr(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CrO | 1 | 1 | (Δ[CrO])/(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[Cr(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CrO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| Cr(OH)2 | water | CrO formula | Cr(OH)2 | H_2O | CrO Hill formula | H2CrO2 | H_2O | CrO name | | water |](../image_source/dad422e94f7b629413c2595c120b1fe9.png)
| Cr(OH)2 | water | CrO formula | Cr(OH)2 | H_2O | CrO Hill formula | H2CrO2 | H_2O | CrO name | | water |
Substance properties
![| Cr(OH)2 | water | CrO molar mass | 86.01 g/mol | 18.015 g/mol | 67.995 g/mol phase | | liquid (at STP) | melting point | | 0 °C | boiling point | | 99.9839 °C | density | | 1 g/cm^3 | surface tension | | 0.0728 N/m | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless |](../image_source/541d1205959f7e6c4c4d8c1f898f0df6.png)
| Cr(OH)2 | water | CrO molar mass | 86.01 g/mol | 18.015 g/mol | 67.995 g/mol phase | | liquid (at STP) | melting point | | 0 °C | boiling point | | 99.9839 °C | density | | 1 g/cm^3 | surface tension | | 0.0728 N/m | dynamic viscosity | | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless |
Units