A laboratory study investigates the gas-phase reaction between nitrogen monoxide and nitrous oxide to form nitrogen and oxygen according to the elementary step
NO(g) + N2O(g) → N2(g) + NO2(g)
Molecular-level simulations capture two representative collision approaches:
• Approach X: The N atom of NO strikes the terminal N atom of the linear N2O molecule along the N–N bond axis.
• Approach Y: The O atom of NO strikes the central N atom of the linear N2O molecule at a right angle to the N–N bond axis.
Assume that all other factors (collision energy, pressure, temperature) are identical in the two simulations.
(a) Identify which approach (X or Y) is more likely to lead to product formation. Justify your answer in terms of bond-making and bond-breaking requirements for this elementary step.
(b) For the less effective approach identified in part (a), describe two specific geometric features that prevent the collision from resulting in products.
(c) The researchers replace linear N2O with bent N2O (an electronically excited isomer). Predict how the probability of a successful collision would change for approaches analogous to X and Y, and explain your reasoning.
(d) Propose one experimental modification (other than changing temperature) that could increase the fraction of successful collisions for the original linear N2O system. Explain how your suggestion addresses the orientation requirement.