Question

Assume that the complete combustion of one mole of fructose, a monosaccharide, to carbon dioxide and water liberates 2810 kJ of energy ( Δ G ° ' = − 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 G ° ' compound X = − 70.7 kJ/mol . Round your answer to two significant figures.

Answer 1

Answer:

Step 1: Extract the data

Given,

Total Energy spent = ΔG° = -2810 kJ/mol

Energy spent per mole =-70.7 kJ/mol

Step 2: Write the balanced chemical equation

C6H12O6 + 6 O2-------> 6 CO2 + 6 H2O ; ΔH=−726kJ

Step 3:Calculation of total moles

Now,

it is given that the energy required to form 1 mol of compound X = -70.7 kJ/mol

and total energy used = -2810 kJ/mol

So,

-70.7 kJ energy used for 1 mol of Compound X

-2810 kJ energy wiil be used for=  ( 1 mol of Compound X / -70.7 kJ ) ×-2810 kJ = 40 mol (approx )

hence, the number of moles of the compound X that could theoretically generated = 40 mol