Question

Suppose you inhaled 1.00 liter of air at −30.0 ◦C and held this air long enough to heat it to body temperature, 37.0◦C. What would be the new volume of the air in the lungs assuming the pressure remained constant? 1. 1.28 L 2. 0.81 L 3. 1.23 L 4. 1.02 L 5. 0.97 L

Answer 1

Answer: 1.28 L

Step-by-step explanation:

To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

`(V_1)/(T_1)=(V_2)/(T_2)`

where,

`V_1\text{ and }T_1` are the initial volume and temperature of the gas.

`V_2\text{ and }T_2` are the final volume and temperature of the gas.

We are given:

`V_1=1.00L\\T_1=-30^oC=(273-30)K=243K\\V_2=?\\T_2=37.0^0C=(273+37)K=310K`

Putting values in above equation, we get:

`(1.00)/(243K)=(V_2)/(310)\\\\V_2=1.28L`

Thus the new volume of the air in the lungs assuming the pressure remained constant is 1.28 L