A ballon is inflated with 2.42L of helium at a temperature of 27.0°C. When put in the freezer, the volume changes to 2.37L and - 8.8°C, and the pressure is measured to be 754torr. What was the initial pressure?

838 torr

Step-by-step explanation:

To solve this problem, we can use the Combined Gas Laws:

p₁V₁/T₁ = p₂V₂/T₂ Multiply each side by T₁

p₁V₁ = p₂V₂ * T₁/T₂ Divide each side by V₁

p₁ = p₂ * V₂/V₁ * T₁/T₂

dа ta:

p₁ = ?; V₁ = 2.42 L; T₁ = 27.0 °C

p₂ = 754 torr; V₂ = 2.37 L; T₂ = - 8.8 °C

Calculations:

(a) Convert temperatures to kelvins

T₁ = (27.0 + 273.15) K = 300.15 K

T₂ = (-8.8 + 273.15) K = 264.35 K

(b) Calculate the pressure

p₁ = 754 torr * (2.37 L/2.42) * (300.15/264.35)

p₁ = 754 torr * 0.979 * 1.135

p₁ = 838 torr