Two glass bulbs of equal volume, connected by a narrow tube, are initially filled with a gas at 0^ C and a pressure of 76 cm of mercury. One bulb is subsequently immersed in melting ice, while the other is placed in a water bath maintained at 62^ C . Assuming the volume of the connecting tube is negligible, determine the new value of the pressure inside the bulbs.

Step-by-step solution

Let the volume of each bulb be V . Initial total number of moles of gas is given by the ideal gas equation: n = P₁ (2V) R T₁ where P₁ = 76 cm of Hg and T₁ = 273 K . When the bulbs are maintained at temperatures T₂ = 273 K (melting ice) and T₃ = 273 + 62 = 335 K (water bath), let the new pressure be P' . The total number of moles remains constant. n₁ + n₂ = n P' V R T₂ + P' V R T₃ = P₁ (2V) R T₁ Substituting the given values: P' V R 273 + P' V R 335 = 76 2V R 273 P' ( 1 273 + 1 335 ) = 152 273 P' ( 335 + 273 273 335