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.

Question

Physics

Kole

15 October, 14:01

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.

+4

Answers (1)

Know the Answer?

Jenna · Answer 1

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.