Assume that the complete combustion of one mole of stearic acid, a fatty acid, to carbon dioxide and water liberates 11400 kJ (?G°\' = -11400 kJ/mol). If the energy generated by the combustion of stearic acid is entirely converted to the synthesis of a hypothetical compound X, calculate the number of moles of the compound that could theoretically be generated. Use the value ?G°\'compound X = -62.3 kJ/mol. Round your answer to two significant figures.

The complete combustion of stearic acid generates 11400 kJ/mol. Assume, for this question, that all this energy is available for the synthesis of a hypothetical compound called \"compound X.\" You are given the energy required for the synthesis of this compound.