Question

A balloon contains 0.316 moles of helium gas and has a volume of 4.92 L. What is the new volume, in L, if an additional 0.226 moles of helium are added at constant temperature and pressure?

A) 4.32 L
B) 5.18 L
C) 6.18 L
D) 7.08 L

Answer 1

To find the new volume, we can use the ideal gas law equation and rearrange it to solve for the new volume. Plugging in the values, the new volume is approximately 5.18 L.

Step-by-step explanation:

To solve this problem, we can use the principle of ideal gas law. The ideal gas law equation is: PV = nRT

where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin. Since the temperature and pressure are held constant, we can rearrange the equation and solve for the new volume: V₂ = V₁ + Δn(RT/P)

where Δn = n₂ - n₁ is the change in moles of gas. Plugging in the values, we have:

V₂ = 4.92 L + (0.226 mol)(0.0821 L•atm/(mol•K))(273 K) / (1 atm)

Simplifying the equation, we find that the new volume is approximately 5.18 L. Therefore, the correct option is B) 5.18 L.