Question

4) An average adult can hold up to 6 Liters of air in their lungs. The internal temperature of a

healthy person is around 32°C at a pressure of 1 atm. It has been found that people who had
Covid 19 may have a reduced lung capacity of 25% or a reduction to 4.5L. If the temperature
increases due to infection/fever to 44°C, what pressure is being exerted on the damaged lungs

Answer 1

if the temperature increases to 44°C, the pressure exerted on the damaged lungs would be approximately 1.334 atm.

Step-by-step explanation:

To determine the pressure being exerted on the damaged lungs, we can use the combined gas law, which states that the pressure of a gas is inversely proportional to its volume when temperature and amount of gas remain constant.

The combined gas law equation is: P₁V₁/T₁ = P₂V₂/T₂

Where:

P₁ = Initial pressure (1 atm)

V₁ = Initial volume (6 L)

T₁ = Initial temperature (32°C + 273.15 = 305.15 K)

P₂ = Final pressure (unknown)

V₂ = Final volume (4.5 L)

T₂ = Final temperature (44°C + 273.15 = 317.15 K)

Rearranging the equation to solve for P₂, we have:

P₂ = (P₁V₁T₂) / (V₂T₁)

Substituting the values:

P₂ = (1 atm * 6 L * 317.15 K) / (4.5 L * 305.15 K)

Calculating this expression gives us:

P₂ ≈ 1.334 atm