Question

This question was in a previous exam paper and I really don’t know how to approach it. This was everything that was given in the question, so no temperature change was given. I’m not sure where to start.

1. Consider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g)
i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted.
ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted.
iii) Sketch a graph which shows how the pressure varies as a function of α.

Answer 1

It is solved on the basis of simple concept of reaction stoichiometry.

solution Gras phase readion at constant valuma (1) 2CH₂ N₂ (9) 2N2(g) + G H a Cg at initial po o l readed 3 Po po zlo then after untv Total Pressure Po -3% + 2 + 3p. z Po + 3 po Total 1 Po PUISSUU - (11) 2CH2N₂ (9) 2N2(g) + C2 Hq (g) at initial pe Seppose predion of po_jacked at equilibscium at equilibrium Po-apo apo apo Total Pressure P z Po-d%o tolo t apo P2 Po t apo In above equation total Peugswue p depends on a 012N2 (1) seacled'). fraction of

(iin PAIN from Paut cii) all got equatton - Page Portfo Pz Lidl+Po____ It is a type of y z mx tc where yap ,mz Pe , CzPo dzd. Hence we can draw graph as- k slope = pod d +