Input interpretation
zinc + copper(II) nitrate ⟶ copper + Zn(NO3)2
Balanced equation
Balance the chemical equation algebraically: + ⟶ + Zn(NO3)2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 ⟶ c_3 + c_4 Zn(NO3)2 Set the number of atoms in the reactants equal to the number of atoms in the products for Zn, Cu, N and O: Zn: | c_1 = c_4 Cu: | c_2 = c_3 N: | 2 c_2 = 2 c_4 O: | 6 c_2 = 6 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: | | + ⟶ + Zn(NO3)2
Structures
+ ⟶ + Zn(NO3)2
Names
zinc + copper(II) nitrate ⟶ copper + Zn(NO3)2
Chemical names and formulas
| zinc | copper(II) nitrate | copper | Zn(NO3)2 formula | | | | Zn(NO3)2 Hill formula | Zn | CuN_2O_6 | Cu | N2O6Zn name | zinc | copper(II) nitrate | copper |
Substance properties
| zinc | copper(II) nitrate | copper | Zn(NO3)2 molar mass | 65.38 g/mol | 187.55 g/mol | 63.546 g/mol | 189.4 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 420 °C | | 1083 °C | boiling point | 907 °C | | 2567 °C | density | 7.14 g/cm^3 | | 8.96 g/cm^3 | solubility in water | insoluble | | insoluble | odor | odorless | | odorless |
Units
