Input interpretation
Fe iron + K potassium ⟶ FeK
Balanced equation
Balance the chemical equation algebraically: Fe + K ⟶ FeK Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Fe + c_2 K ⟶ c_3 FeK Set the number of atoms in the reactants equal to the number of atoms in the products for Fe and K: Fe: | c_1 = c_3 K: | c_2 = c_3 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: | | Fe + K ⟶ FeK
Structures
+ ⟶ FeK
Names
iron + potassium ⟶ FeK
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Fe + K ⟶ FeK 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: Fe + K ⟶ FeK 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 Fe | 1 | -1 K | 1 | -1 FeK | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) K | 1 | -1 | ([K])^(-1) FeK | 1 | 1 | [FeK] 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 = ([Fe])^(-1) ([K])^(-1) [FeK] = ([FeK])/([Fe] [K])](../image_source/a5e11e66c5a2d30fe558bea60e0db45c.png)
Construct the equilibrium constant, K, expression for: Fe + K ⟶ FeK 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: Fe + K ⟶ FeK 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 Fe | 1 | -1 K | 1 | -1 FeK | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Fe | 1 | -1 | ([Fe])^(-1) K | 1 | -1 | ([K])^(-1) FeK | 1 | 1 | [FeK] 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 = ([Fe])^(-1) ([K])^(-1) [FeK] = ([FeK])/([Fe] [K])
Rate of reaction
![Construct the rate of reaction expression for: Fe + K ⟶ FeK 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: Fe + K ⟶ FeK 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 Fe | 1 | -1 K | 1 | -1 FeK | 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 Fe | 1 | -1 | -(Δ[Fe])/(Δt) K | 1 | -1 | -(Δ[K])/(Δt) FeK | 1 | 1 | (Δ[FeK])/(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[Fe])/(Δt) = -(Δ[K])/(Δt) = (Δ[FeK])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/4b4d6492f196aa952f9a1ef4fab4626d.png)
Construct the rate of reaction expression for: Fe + K ⟶ FeK 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: Fe + K ⟶ FeK 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 Fe | 1 | -1 K | 1 | -1 FeK | 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 Fe | 1 | -1 | -(Δ[Fe])/(Δt) K | 1 | -1 | -(Δ[K])/(Δt) FeK | 1 | 1 | (Δ[FeK])/(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[Fe])/(Δt) = -(Δ[K])/(Δt) = (Δ[FeK])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| iron | potassium | FeK formula | Fe | K | FeK name | iron | potassium |
Substance properties
| iron | potassium | FeK molar mass | 55.845 g/mol | 39.0983 g/mol | 94.943 g/mol phase | solid (at STP) | solid (at STP) | melting point | 1535 °C | 64 °C | boiling point | 2750 °C | 760 °C | density | 7.874 g/cm^3 | 0.86 g/cm^3 | solubility in water | insoluble | reacts |
Units
