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.

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 .

the second one and the forth one are in the purple because they are opinions and the rest are in the yellow

explanation:

force is mass*acceleration.

we have a very small mass: 11.4*0.001 kg

if we want 0.035n of force, we need an acceleration:

0.035 = 11.4*0.001*a

a = 0.035/(11.4*0.001) m/s^2