Chemistry - Ideal Gas Question with Solution | TestHub
Chemical explosions are characterised by the instantaneous release of large quantities of hot gases, which set up a shock wave of enormous pressure and velocity. Explosion of a compound X releases four gases A, B, C and D.
n X a A(g) + b B(g) + c C(g) + d D(g)
Assume that the explosion of 1 mol of X releases gases with a temperature of 2727°C and a volume of 3.0 l at 410 atm pressure. (R = 0.0821 l-atm/K-mol)
When gases B, C and D were passed through a tube of powdered Li₂O, gas B reacted to form Li₂CO₃. The remaining gases C and D were collected in another 821 ml flask at a pressure of 0.6 atm at 27°C. How many moles of B were present and what is its likely identity?
Options:
Answer:
Solution:
n(C+D) = 0.6 × 0.821/(0.0821 × 300) = 0.02 mol. n(B) = 0.06 - 0.02 = 0.04 mol; formation of Li₂CO₃ with Li₂O identifies B as CO₂. Hence (d).
