The balanced reaction equation for this redox reaction is:
4NO(g) + O₂(g) → 2N₂O₃(g)
The rate of [NO] decreasing is 1.054 M/s.
This is a redox reaction, so to balance it, we need to identify which elements change their oxidation state. Obviously, nitrogen is oxidized from +2 (N²⁺O²⁻) to +3 (N⁺³₂O²⁻₃), and oxygen is reduced from 0 (O⁰₂) to -2.
N²⁺ → N⁺³ + e⁻
O⁰₂ + 4e⁻ → 2O²⁻
In order for the number of electrons released and taken to be the same, we need to multiply the number of nitrogens by 4:
4N²⁺ → 4N⁺³ + 4e⁻
O⁰₂ + 4e⁻ → 2O²⁻
We can now apply these numbers to the reaction equation:
4NO(g) + O₂(g) → 2N₂O₃(g)
With the balanced reaction equation, we can see that 4 moles of NO produce 2 moles of N₂O₃. So if 0.527 M were produced in a single second, the rate of NO decreasing would be 2 * 0.527 M = 1.054 M/s.
You can learn more about redox reactions here:
brainly.com/question/13293425
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