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 C and D were passed through a hot tube of powdered copper, gas C reacted to form CuO. The remaining gas D was collected in a third 821 ml flask and found to have mass of 0.42 g and a pressure of 0.45 atm at 27°C. How many moles each of C and D were present and what are their likely identities?
Options:
Answer:
Solution:
n(D) = 0.45 × 0.821/(0.0821 × 300) = 0.015 mol; molar mass = 0.42/0.015 = 28 g/mol ⇒ N₂. n(C) = 0.02 - 0.015 = 0.005 mol; forming CuO with hot Cu identifies C as O₂. Hence (b).
