Chapter 4, Problem 4.54P

The oxidation of glucose provides the principal source of energy for animal cells.
Assume the reactants are glucose $\left[C_6{H}_{12}{O}_6\left(s\right)\right]$ and oxygen $\left[O_2\left(g\right)\right]$ . The products are CO₂(g) and H₂O(l).

1. Write a balanced equation for glucose oxidation, and determine the standard heat of reaction at 298 K.
2. During a day an average person consumes about 150 kJ of energy per kg of body mass. Assuming glucose the sole source of energy, estimate the mass (grams) of glucose required daily to sustain a person of 57 kg.
3. For a population of 275 million persons, what mass of CO₂ (a greenhouse gas) is produced daily by mere respiration. Data: For glucose, $△H_{f298}^{\circ }=-1274.4kJ\cdot mo{l}^{-1}$ . Ignore the effect of temperature on the heat of reaction.