1. The problem statement, all variables and given/known data Hydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and oxygen, another method is the reaction between water and oxygen. Given the ΔG°rxn values for each reaction, which method (reaction 1 or 2) requires less energy under standard conditions? 1. H2(gas) + O2(gas) <---> H2O2(liquid) ΔG°rxn = -120.4 kJ 2. H2O(liquid) + 1/2 O2(gas) <---> H2O2(liquid) ΔG°rxn = +116.7 kJ 2. Relevant equations N/A 3. The attempt at a solution Would the answer be reaction 2 because it is lower in magnitude? I know that a negative free energy value corresponds to a spontaneous reaction and a positive value a nonspontaneous reaction but is the sign significant in this case?