CO + CuO = CO2 + Cu

carbon monoxide + cupric oxide ⟶ carbon dioxide + copper

Balance the chemical equation algebraically: + ⟶ + Add stoichiometric coefficients, c_i, to the reactants and products: c_1 + c_2 ⟶ c_3 + c_4 Set the number of atoms in the reactants equal to the number of atoms in the products for C, O and Cu: C: | c_1 = c_3 O: | c_1 + c_2 = 2 c_3 Cu: | c_2 = 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: | | + ⟶ +

+ ⟶ +

carbon monoxide + cupric oxide ⟶ carbon dioxide + copper

| carbon monoxide | cupric oxide | carbon dioxide | copper molecular enthalpy | -110.5 kJ/mol | -157.3 kJ/mol | -393.5 kJ/mol | 0 kJ/mol total enthalpy | -110.5 kJ/mol | -157.3 kJ/mol | -393.5 kJ/mol | 0 kJ/mol | H_initial = -267.8 kJ/mol | | H_final = -393.5 kJ/mol | ΔH_rxn^0 | -393.5 kJ/mol - -267.8 kJ/mol = -125.7 kJ/mol (exothermic) | | |

| carbon monoxide | cupric oxide | carbon dioxide | copper molecular entropy | 198 J/(mol K) | 43 J/(mol K) | 214 J/(mol K) | 33 J/(mol K) total entropy | 198 J/(mol K) | 43 J/(mol K) | 214 J/(mol K) | 33 J/(mol K) | S_initial = 241 J/(mol K) | | S_final = 247 J/(mol K) | ΔS_rxn^0 | 247 J/(mol K) - 241 J/(mol K) = 6 J/(mol K) (endoentropic) | | |

| carbon monoxide | cupric oxide | carbon dioxide | copper Hill formula | CO | CuO | CO_2 | Cu name | carbon monoxide | cupric oxide | carbon dioxide | copper