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breonaleonard6821
08.11.2019 •
Chemistry
For the reaction:
2n2o5(g) → 4no2(g) + o2(g) the rate law is: (δ[o2]/δt) = k[n2o5] at 300 k, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kj/mol. what is the half-life at 310 k? (hint: use rate law expression to determine the reaction order → solve for k1 at 300 k using the corresponding half-life expression → use two-point arrhenius equation to solve for k2 at 310 k → use the half-life expression again to solve for half-life at 310 k)
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Ответ:
Half-life at 310 K is 6.54 × 10³ s.
Explanation:
Let's consider the following reaction:
2 N₂O₅(g) → 4 NO₂(g) + O₂(g)
The rate law is:
(Δ[O₂]/Δt) = k . [N₂O₅]
Since [N₂O₅] is raised to the power of 1, the reaction order is 1.
For a first-order reaction:
where,
At 300 K,
We can use two-point Arrhenius equation to solve for k₂ at 310 K
At 310 K,
Ответ:
It's a big cycle, all leading to the demise of the ocean