Question

A balloon has a pressure of 56mmHg and is 1.5 L in volume. If the balloon is forced to fill a volume of 0.56L, what is the pressure of the ballon (in atm)? Assume constant temp. (Boyle's Law). 15 points pls help

Answer 1

P1V1 = P2V2
56 mmHg * 1.5 L = P2 * 0.56 L
P2 = 56 mmHg * 1.5 L / 0.56 L

To convert the pressure from mmHg to atmospheres (atm), we use the conversion factor:

1 atm = 760 mmHg

So,

P2 = 56 mmHg * 1.5 L / 0.56 L = 56 * 1.5 / 0.56 * 760 mmHg / atm
P2 = 976 mmHg
P2 = 976 mmHg / 760 mmHg/atm = 1.29 atm

Therefore, the pressure of the balloon after it is forced to fill a volume of 0.56 liters is 1.29 atmospheres.