Answer:
V = 1.6 L
Explanation:
assuming ideal gas:
∴ R = 0.082 atm.L/K.mol
∴ V1 = 1.50 L
∴ n1 = 3.00 mol
∴ T1 = 25°C ≅ 298 K
⇒ P1 = (RT1n1)/(V1) = ((0.082 atm.L/K.mol)(298 K)(3.00 mol))/(1.50 L)
⇒ P1 = 48.872 atm
with pressure and temperature held constant:
∴ T2 = T1 = 298 K
∴ P2 = P1 = 48.872 atm
∴ n2 = 0.20 mol + 3.00 mol = 3.20 mol
⇒ V2 = (RT2n2)/P2
⇒ V2 = ((0.082 atm.L/K.mol)(298 K)(3.20 mol))/(48.872 atm)
⇒ V2 = 1.6 L
A balloon initially filled to a volume of 1.50 L with 3.00 moles of gas at 25 °C, to which 0.20 moles of gas are added at constant pressure and temperature, will have a final volume of 1.60 L.
A balloon is filled to a volume of 1.50 L (V₁) with 3.00 moles of gas (n₁) at 25 °C. When 0.20 moles of gas are added, the final number of moles (n₂) will be:
[tex]n_2 = 3.00 mol + 0.20 mol = 3.20 mol[/tex]
With pressure and temperature held constant, we can calculate the final volume of the balloon (V₂) using Avogadro's law, which states that there is a direct relationship between the number of gaseous moles and the volume.
[tex]\frac{V_1}{n_1} = \frac{V_2}{n_2} \\V_2 = \frac{V_1 \times n_2 }{n_1} = \frac{1.50 L \times 3.20mol }{3.00mol} = 1.60 L[/tex]
A balloon initially filled to a volume of 1.50 L with 3.00 moles of gas at 25 °C, to which 0.20 moles of gas are added at constant pressure and temperature, will have a final volume of 1.60 L.
You can learn more about Avogadro's law here: https://brainly.com/question/4133756
