Input interpretation
magnesium + silver nitrate ⟶ silver + MgNO3
Balanced equation
Balance the chemical equation algebraically: + ⟶ + MgNO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 ⟶ c_3 + c_4 MgNO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Mg, Ag, N and O: Mg: | c_1 = c_4 Ag: | c_2 = c_3 N: | c_2 = c_4 O: | 3 c_2 = 3 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | + ⟶ + MgNO3
Structures
+ ⟶ + MgNO3
Names
magnesium + silver nitrate ⟶ silver + MgNO3
Equilibrium constant
![K_c = ([Ag] [MgNO3])/([Mg] [AgNO3])](../image_source/bf6a331658d725eb7886f53e382a3a91.png)
K_c = ([Ag] [MgNO3])/([Mg] [AgNO3])
Rate of reaction
![rate = -(Δ[Mg])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[Ag])/(Δt) = (Δ[MgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/a39be2cb7a38b6b5d51aee7acb4ba553.png)
rate = -(Δ[Mg])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[Ag])/(Δt) = (Δ[MgNO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
| magnesium | silver nitrate | silver | MgNO3 formula | | | | MgNO3 Hill formula | Mg | AgNO_3 | Ag | MgNO3 name | magnesium | silver nitrate | silver |
Substance properties
| magnesium | silver nitrate | silver | MgNO3 molar mass | 24.305 g/mol | 169.87 g/mol | 107.8682 g/mol | 86.309 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 648 °C | 212 °C | 960 °C | boiling point | 1090 °C | | 2212 °C | density | 1.738 g/cm^3 | | 10.49 g/cm^3 | solubility in water | reacts | soluble | insoluble | odor | | odorless | |
Units
