O2 + Ag = AgO

oxygen + silver ⟶ silver(II) oxide

Balance the chemical equation algebraically: + ⟶ Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 ⟶ c_3 Set the number of atoms in the reactants equal to the number of atoms in the products for O and Ag: O: | 2 c_1 = c_3 Ag: | 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 = 2 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | + 2 ⟶ 2

+ ⟶

oxygen + silver ⟶ silver(II) oxide

| oxygen | silver | silver(II) oxide molecular enthalpy | 0 kJ/mol | 0 kJ/mol | -24.3 kJ/mol total enthalpy | 0 kJ/mol | 0 kJ/mol | -48.6 kJ/mol | H_initial = 0 kJ/mol | | H_final = -48.6 kJ/mol ΔH_rxn^0 | -48.6 kJ/mol - 0 kJ/mol = -48.6 kJ/mol (exothermic) | |

| oxygen | silver | silver(II) oxide molecular entropy | 205 J/(mol K) | 42.6 J/(mol K) | 117 J/(mol K) total entropy | 205 J/(mol K) | 85.2 J/(mol K) | 234 J/(mol K) | S_initial = 290.2 J/(mol K) | | S_final = 234 J/(mol K) ΔS_rxn^0 | 234 J/(mol K) - 290.2 J/(mol K) = -56.2 J/(mol K) (exoentropic) | |

| oxygen | silver | silver(II) oxide Hill formula | O_2 | Ag | AgO name | oxygen | silver | silver(II) oxide IUPAC name | molecular oxygen | silver | oxosilver

| oxygen | silver | silver(II) oxide molar mass | 31.998 g/mol | 107.8682 g/mol | 123.867 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) melting point | -218 °C | 960 °C | 100 °C boiling point | -183 °C | 2212 °C | density | 0.001429 g/cm^3 (at 0 °C) | 10.49 g/cm^3 | 7.44 g/cm^3 solubility in water | | insoluble | surface tension | 0.01347 N/m | | dynamic viscosity | 2.055×10^-5 Pa s (at 25 °C) | | odor | odorless | |