Glucose is the primary sugar in your bloodstream, supplying energy to your body. Dieticians therefore may need to investigate the enthalpy changes that accompany its reactions. A constant-volume bomb calorimeter was used to measure the heat generated by the combustion of 1.000 mol glucose molecules in the reaction C₆H₁₂O₆(s) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O(g), and found it to be 2559 kJ at 298 K; so ΔU = 22559 kJ. What is the change in enthalpy for the same reaction?

ANTICIPATE Because there is a net formation of gas (from 6 mol to 12 mol), you should expect ΔH to be less negative than ΔU.

What should you assume? Assume that each gas is ideal.