Question

Suppose that on a hot and sticky afternoon in the spring, a tornado passes over the high school. If the air pressure in the lab (volume of 180 m3) was 1.1 atm before the storm and 0.85 atm during the storm, to what volume would the laboratory try to expand in order to make up for the large pressure difference outside?
190 m3
230 m3
1,800 m3
7,100 m3

Answer 1

The answer is B) 230 m3

Answer 2

Answer: $230m^3$

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

$P\propto \frac{1}{V}$     (At constant temperature and number of moles)

$P_1V_1=P_2V_2$

where,

$P_1$ = initial pressure of gas  = 1.1 atm

$P_2$ = final pressure of gas  = 0.85 atm

$V_1$ = initial volume of gas  = $180m^3$

$V_2$ = final volume of gas  = ?

$1.1\times 180=0.85\times V_2$

$V_2=230m^3$

Therefore, the gas would expand to volume of $230m^3$