Question

whole resting an average 70 kg human male consumes 16.628 ltrs of oxygen per hour at 27°C and 100KPa number of molesof oxygen are are consumed by the 70 kg man while resting for 1hr is 6.7x10^-p where p=
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Answer 1

Given:

The volume of oxygen consumed by the person per hour, V = 16.628 L

The no of moles of oxygen consumed by the person per hour, n = 6.7 × 10^-p

Temperature, T = 27°C = 300 K

Pressure, P = 100 KPa = 10⁵ Pa = 0.987 atm

To Find:

The value of p.

Calculation:

- Applying the ideal gas equation, we have:

PV = nRT

⇒ n = PV/RT

⇒ n = 0.987 × 16.628/ 0.082 × 300

⇒ n = 0.67

⇒ n = 6.7 × 10⁻¹

- So, the value of p is 1.