Question

Assume that the complete combustion of one mole of fructose, a monosaccharide, to carbon dioxide and water liberates 2810 kJ of energy (Δ?°′=−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 Δ?°′compound X=−75.7 kJ/mol . Round your answer to two significant figures.

Assume that the complete combustion of one mole of fructose, a monosaccharide, to carbon dioxide and water liberates = -2810 kJ/mol) 2810 kJ of energy (AG 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 AG compouad X-75.7 kJ/mol Round your answer to two significant figures moles

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Answer 1

The reaction is as follows: C6H12O6(S) + 60₂ (g) 6co, (q) + 6 hoce The total energy Librated is - 2810 kJ Energy required to synthesize mole at compound x is = -75.7kJ I mo) No. of moles of compound a total Energy => n = -2810 KJ & - 25.7 Kulmal n = 37.120 mol or 37 mol