For the reaction: 2 N2O5(g) 4 NO2(g) + O2(g) at the time when ...

[@Brianna17]

Question 1

For the reaction 2 HgCl₂ + C₂O₄^2-→ products, data are:

[HgCl₂]₀ (in M) 0.0836 0.0836 0.0418
[C₂O₄^2-]₀ (in M) 0.202 0.404 0.404
rate (M/hr) 0.26 1.04 0.53

The rate law is Rate = k[HgCl₂]^x[C₂O₄^2-]^y. Thus:
◦ x = 2, y = 1
◦ x = 2, y = 2
◦ x = 1, y = 2
◦ x = 1, y = 1
◦ x = 0, y = 2

Question 2

For the reaction: 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) at the time when N₂O₅ is being consumed at a rate of 1.2 × 10^-4 M/s, what is the rate at which O₂ is being formed?
◦ 1.2 × 10^-4 M/s
◦ 2.4 × 10^-4 M/s
◦ 6.0 × 10^-5 M/s
◦ 3.0 × 10^-5 M/s
◦ 4.8 × 10^-4 M/s

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[@Brianna17]

Thanks for the timely response, appreciate it

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