Question

A person inhales 640 gm of $O_2$ per day. If all the $O_2$ is used for converting sugar into $C{O}_2$ and $H_{2}O$, the sucrose $\left(C_{12}{H}_{22}{O}_{11}\right)$ consumed in gram in the body in one day and the heat evolved are
Given: $(\Delta H_{combustionofsucrose}=-5645kJmo{l}^{-1})$

• A. $250,8608.94kJ$
• B. $630,6552.52kJ$
• C. $850,9522.21kJ$
• D. $570,9408.34kJ$

Answer 1

Answer: (D)

$570,9408.34kJ$

$C_{12}{H}_{12}{O}_{11}+12O_2⟶12C{O}_2+11H_{2}O;\Delta H=-5645kJ$
Moles of $O_2$ used per day $=\frac{640}{32}=20$
$\therefore$ Moles of sucrose used per day or for 20 mole $O_2=\frac{20}{12}mol=\frac{20}{12}\times 342g=570g$.
Also, $\Delta H=\frac{5645\times 20}{12}=9408.34kJ$.