Assume that the complete combustion of one mole of fructose, a monosaccharide, to carbon dioxide and water liberates 2810 kj (δg°\' = –2810 kj/mol). if the energy generated by the combustion of fructose 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 δg°\'compound x = − 64.1 kj/mol kj/mol. round your answer to two significant figures.

Explanation:

The reaction equation will be as follows.

It is given that the total energy liberated is -2810 kJ/mol. As the sign is negative this means that energy is being released. Also, it is given that the energy required to synthesis is -64.1 kJ/mol.

Therefore, calculate the number of moles of compound as follows.

         No. of moles =

                               =

                               = 43.83 mol

                               = 44 mol (approx)

Thus, we can conclude that the number of moles of compound is 44 mol.

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