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K + Ag2SO4 = K2SO4 + Ag

Input interpretation

K potassium + Ag_2SO_4 silver sulfate ⟶ K_2SO_4 potassium sulfate + Ag silver
K potassium + Ag_2SO_4 silver sulfate ⟶ K_2SO_4 potassium sulfate + Ag silver

Balanced equation

Balance the chemical equation algebraically: K + Ag_2SO_4 ⟶ K_2SO_4 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K + c_2 Ag_2SO_4 ⟶ c_3 K_2SO_4 + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for K, Ag, O and S: K: | c_1 = 2 c_3 Ag: | 2 c_2 = c_4 O: | 4 c_2 = 4 c_3 S: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: |   | 2 K + Ag_2SO_4 ⟶ K_2SO_4 + 2 Ag
Balance the chemical equation algebraically: K + Ag_2SO_4 ⟶ K_2SO_4 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K + c_2 Ag_2SO_4 ⟶ c_3 K_2SO_4 + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for K, Ag, O and S: K: | c_1 = 2 c_3 Ag: | 2 c_2 = c_4 O: | 4 c_2 = 4 c_3 S: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 K + Ag_2SO_4 ⟶ K_2SO_4 + 2 Ag

Structures

 + ⟶ +
+ ⟶ +

Names

potassium + silver sulfate ⟶ potassium sulfate + silver
potassium + silver sulfate ⟶ potassium sulfate + silver

Equilibrium constant

Construct the equilibrium constant, K, expression for: K + Ag_2SO_4 ⟶ K_2SO_4 + Ag 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: 2 K + Ag_2SO_4 ⟶ K_2SO_4 + 2 Ag 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 K | 2 | -2 Ag_2SO_4 | 1 | -1 K_2SO_4 | 1 | 1 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K | 2 | -2 | ([K])^(-2) Ag_2SO_4 | 1 | -1 | ([Ag2SO4])^(-1) K_2SO_4 | 1 | 1 | [K2SO4] Ag | 2 | 2 | ([Ag])^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 = ([K])^(-2) ([Ag2SO4])^(-1) [K2SO4] ([Ag])^2 = ([K2SO4] ([Ag])^2)/(([K])^2 [Ag2SO4])
Construct the equilibrium constant, K, expression for: K + Ag_2SO_4 ⟶ K_2SO_4 + Ag 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: 2 K + Ag_2SO_4 ⟶ K_2SO_4 + 2 Ag 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 K | 2 | -2 Ag_2SO_4 | 1 | -1 K_2SO_4 | 1 | 1 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K | 2 | -2 | ([K])^(-2) Ag_2SO_4 | 1 | -1 | ([Ag2SO4])^(-1) K_2SO_4 | 1 | 1 | [K2SO4] Ag | 2 | 2 | ([Ag])^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 = ([K])^(-2) ([Ag2SO4])^(-1) [K2SO4] ([Ag])^2 = ([K2SO4] ([Ag])^2)/(([K])^2 [Ag2SO4])

Rate of reaction

Construct the rate of reaction expression for: K + Ag_2SO_4 ⟶ K_2SO_4 + Ag 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: 2 K + Ag_2SO_4 ⟶ K_2SO_4 + 2 Ag 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 K | 2 | -2 Ag_2SO_4 | 1 | -1 K_2SO_4 | 1 | 1 Ag | 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 K | 2 | -2 | -1/2 (Δ[K])/(Δt) Ag_2SO_4 | 1 | -1 | -(Δ[Ag2SO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(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 = -1/2 (Δ[K])/(Δt) = -(Δ[Ag2SO4])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K + Ag_2SO_4 ⟶ K_2SO_4 + Ag 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: 2 K + Ag_2SO_4 ⟶ K_2SO_4 + 2 Ag 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 K | 2 | -2 Ag_2SO_4 | 1 | -1 K_2SO_4 | 1 | 1 Ag | 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 K | 2 | -2 | -1/2 (Δ[K])/(Δt) Ag_2SO_4 | 1 | -1 | -(Δ[Ag2SO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(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 = -1/2 (Δ[K])/(Δt) = -(Δ[Ag2SO4])/(Δt) = (Δ[K2SO4])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

 | potassium | silver sulfate | potassium sulfate | silver formula | K | Ag_2SO_4 | K_2SO_4 | Ag Hill formula | K | Ag_2O_4S | K_2O_4S | Ag name | potassium | silver sulfate | potassium sulfate | silver IUPAC name | potassium | disilver sulfate | dipotassium sulfate | silver
| potassium | silver sulfate | potassium sulfate | silver formula | K | Ag_2SO_4 | K_2SO_4 | Ag Hill formula | K | Ag_2O_4S | K_2O_4S | Ag name | potassium | silver sulfate | potassium sulfate | silver IUPAC name | potassium | disilver sulfate | dipotassium sulfate | silver

Substance properties

 | potassium | silver sulfate | potassium sulfate | silver molar mass | 39.0983 g/mol | 311.79 g/mol | 174.25 g/mol | 107.8682 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 64 °C | 652 °C | | 960 °C boiling point | 760 °C | | | 2212 °C density | 0.86 g/cm^3 | | | 10.49 g/cm^3 solubility in water | reacts | slightly soluble | soluble | insoluble
| potassium | silver sulfate | potassium sulfate | silver molar mass | 39.0983 g/mol | 311.79 g/mol | 174.25 g/mol | 107.8682 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 64 °C | 652 °C | | 960 °C boiling point | 760 °C | | | 2212 °C density | 0.86 g/cm^3 | | | 10.49 g/cm^3 solubility in water | reacts | slightly soluble | soluble | insoluble

Units