Question

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.

Answer 1

Step-by-step explanation:

The reaction equation will be as follows.

`C_(6)H)_(12)O_(6)(s) + 6O_(2)(g) \rightarrow 6CO_(2)(g) + 6H_(2)O(l)`

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 =
`\frac{\text{total energy}}{\text{energy necessary to synthesise 1 mole of compound X}}`

=
`(-2810 kJ)/(-64.1 kJ/mol)`

= 43.83 mol

= 44 mol (approx)

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