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Gelneren [198K]
3 years ago
12

Assume that the complete combustion of one mole of glucose, a monosaccharide, to carbon dioxide and water liberates 2870 kJ2870

kJ of energy (ΔG°′=−2870 kJ/mol(ΔG°′=−2870 kJ/mol ). If the energy generated by the combustion of glucose 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=−54.1 kJ/molΔG°′compound X=−54.1 kJ/mol . Round your answer to two significant figures.
Chemistry
1 answer:
Lubov Fominskaja [6]3 years ago
7 0

Answer:

number of moles of the compound \approx 53 mole

Explanation:

Given that:

The total energy liberated = - 2870 kJ  ( here , the negative sign typical implies the release of energy due to the combustion reaction)

The equation of the reaction can be represented as:

\mathbf{C_6H_{12}O_6_{(s)} + 6O_{2(g)} \to 6CO_{2(g)}+6H_2O_{(l)}}

The energy needed to synthesize 1 mole of compound X  = - 54.1 kJ.mol

Thus;

The total energy = numbers of moles of compound × Energy needed to synthesize  1 mole of compound X

Making the numbers of moles of the compound the subject; we have;

numbers of moles of compound = numbers  \ of \  moles  \ of \  compound =  \dfrac{total \ energy }{Energy \  needed  \ to  \ synthesize \   1  \ mole \  of \  compound  \ X}numbers  \ of \  moles  \ of \  compound =  \dfrac{-2870  \ kJ }{-54.1  \ kJ/mol}

number of moles of the compound = 53.04990  mole

number of moles of the compound \approx 53 mole to two significant figure

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