The mechanism below is proposed for the thermal decomposition of gaseous species G at 600 K.
Step 1 G ⇌ H (fast)
Step 2 H + G ⇌ I (fast)
Step 3 I ⇌ J (fast)
Step 4 J → 2 K (slow)
All steps are elementary; no other pathways exist.
(a) Using appropriate symbols for the stepwise equilibrium constants, express [H], [I], and [J] individually in terms of [G].
(b) Derive a rate law for the overall formation of K that contains only the measurable concentration [G] and the kinetic and equilibrium constants from the mechanism.
(c) Combine the stepwise equilibrium constants into a single constant Kc such that the rate law from part (b) is written in the form rate=kobs[G]n. State explicit algebraic expressions for Kc, kobs, and the reaction order n.
(d) The experimentally determined rate law at 600 K is rate=kexp[G]3/2. Compare this result with your expression from part (c) and discuss what information, if any, can be inferred about the relative magnitudes of the individual equilibrium constants.