Chemistry - Ideal Gas Question with Solution | TestHub
The apparatus shown consists of three temperature jacketed 1.642 l bulbs connected by stopcocks. Bulb A contains a mixture of H2O(g), CO2(g) and N2(g) at 27°C and a total pressure of 570 mm Hg. Bulb B is empty and held at a temperature of -73°C. Bulb C is also empty and is held at a temperature of -193°C. The stopcocks are closed and the volume of the lines connecting the bulbs is zero. CO2 sublimes at -78°C and N2 boils at -196°C. Neglect the volume of any solid, if formed.
How many moles of CO2 are in the system?
Options:
Answer:
Solution:
At equilibrium only N2 is gaseous, at 22.5 mm Hg throughout the three bulbs: n(N2) = ((22.5/760) × 1.642)/0.0821(1/300 + 1/200 + 1/80) ≈ 0.0123 mol. The gas mixture totalled 0.035 mol, so n(CO2) = 0.035 - 0.0123 ≈ 0.0225 mol. Hence (c).
