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Assume that the complete combustion of one mole of stearic acid, a fatty acid, to carbon dioxide and water liberates 11400 kJ of energy (Δ????°′=−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 Δ????°′compound X=−37.5 kJ/mol . Round your answer to two significant figures.

Respuesta :

Answer:

310 moles

Explanation:

Combustion of one mole of stearic acid gives out calories equivalent to

11400 kJ of energy. On the other hand Synthesis of compound requires energy . One mole of compound X requires energy of 37.5 kJ

So no of moles of X which can be synthesized

= Energy liberated / energy required per mole

= 11400 / 37.5

= 304 moles

≈ 310 moles .

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