Question

If a balloon is filled with air at a pressure of 1.2 atm and has a volume of 5.2 L and that balloon is placed in a pressure chamber where the pressure is 9.5 atm, what will the new volume of the balloon be? Assume T is held constant at 285 K. How many moles of gas does the balloon hold in this pressure chamber situation?

A. 0.68 L, 0.52 moles
B. 0.32 L, 1.20 moles
C. 1.44 L, 2.50 moles
D. 2.18 L, 3.80 moles

Answer 1

To find the new volume of the balloon in the pressure chamber, use Boyle's Law. The new volume would be approximately 0.66 L. To determine the number of moles of gas the balloon holds in the pressure chamber, use the Ideal Gas Law. The balloon holds approximately 3.78 moles of gas.

Step-by-step explanation:

To find the new volume of the balloon when placed in a pressure chamber, we can use Boyle's Law, which states that the product of pressure and volume is constant as long as temperature is held constant. Using this relationship, we can set up the equation:

P1V1 = P2V2

Substituting the given values, we have:

(1.2 atm)(5.2 L) = (9.5 atm)(V2)

Solving for V2 gives us:

V2 = (1.2 atm)(5.2 L) / (9.5 atm) = 0.657 L

Therefore, the new volume of the balloon in the pressure chamber would be approximately 0.66 L.

To determine the number of moles of gas the balloon holds in the pressure chamber, we can use the ideal gas law equation:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the Ideal Gas Constant, and T is the temperature. Rearranging the equation to solve for n:

n = PV / RT

Substituting the given values, we have:

n = (9.5 atm)(0.657 L) / (0.0821 L·atm/mol·K)(285 K) = 3.78 moles

Therefore, the balloon holds approximately 3.78 moles of gas in the pressure chamber situation.