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AysviL [449]
3 years ago
13

Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 2 NO2(g) 2 NO(g) + O2(g). When 0.500 M

NO2 is allowed to react for 90.0 seconds, its concentration falls to 0.0196 M. What is the half-life of the reaction when [NO2]0 = 0.500 M?
Chemistry
1 answer:
OlgaM077 [116]3 years ago
3 0

Answer:

half-life is 3.67s

Explanation:

The general law of the second-order reaction is:

\frac{1}{[A]}=\frac{1}{[A]_0}+kt

As after 90.0s, the concentration of NO2 decreases from 0.500M to 0.0196M:

\frac{1}{[0.0196]}=\frac{1}{[0.500]}+k*90.0s

49.02M⁻¹ = K*90.0s

0.5447M⁻¹s⁻¹ = K

Now, half-life, t1/2 is:

t_{1/2}=\frac{1}{K[A]_0}

Half-life is:

t(1/2) = 1 / (0.5447M⁻¹s⁻¹*0.500M)

<h3>half-life is 3.67s</h3>
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4. By what quantity must the heat capacity be divided to obtain the specific heat of that material? (I poin
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Ek=(1/2)mv²
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