Question

While resting, the average human male use 0.2 $d{m}^3$ of $O_2$ per hour at 1 atm & 273 K for each kg of body mass. Assume that all this $O_2$ is used to produce energy by oxidising glucose in the body. What is the mass of glucose required per hour by a resting male having mass 60 kg. What volume, at 1 atm and 273 K of $C{O}_2$ would be produced?

• A. 16.07 gm ; 12 dm${}^3$
• B. 26.07 gm ; 12 dm${}^3$
• C. 16.07 gm ; 22 dm${}^3$
• D. 26.07 gm ; 22 dm${}^3$

Answer 1

The correct option is A 16.07 gm ; 12 dm${}^3$

$C_6{H}_{12}{O}_6+6O_2\to 6C{O}_2+6H_{2}O$

$n_{O_2}=60\times \frac{0.2}{22.4}=0.5357$

$n_{glucose}=\frac{0.5357}{6}=0.08928$ moles

$W_{glucose}=180\times 0.08928=16.07$ gm

$n_{C{O}_2}=n_{O_2}=0.5357$ moles

$V_{C{O}_2}=22.4\times 0.5357=12d{m}^3$

Hence, the correct answer is option $\text{A}$.