Dinitrogen pentoxide. N_2O_5, decomposes in CCl_4 as shown below: The reaction i

Question

Dinitrogen pentoxide. N_2O_5, decomposes in CCl_4 as shown below: The reaction is a first order with a rate constant of 3.65 times 10^-4 /s at 40 degree C. W hat is the half-life for the reaction? If the initial concentration of N_2O_5 is 0.400 M. what will the concentration he after four half-lives? A possible mechanism for a reaction that takes place in solution is What is the for the overall reaction what is the predicted rate law which species is (are) intermediates, and which species is the catalyst? A sample of N_2O_4 (0.400 mol) was placed in an empty 1.00 L container at 500 K. After equilibrium was reached, the concentration of NO_2 was found to be 6.29 times 10^-4 M. Calculate the value of K_c at 500 K for the reaction:

Explanation / Answer

Answer :

Decomposition of N2O5 (g),

2 N2O5 (g) --------> 2 N2O4 (g) + O2 (g)

Given that this is a First order reaction with rate constant k = 3.65 x 10-4 s-1.

For First order reaction Half-life (t½) and rate constant (k) are related through equation,

t½ = 0.693/k

With k = 3.65 x 10-4 s-1 we have,

t½ = 0.693 / (3.65 x 10-4)

t½ = 1.899 x 103

t½ = 1899 s

Half-life (t½) of decomposition of N2O5 is 1899 s.

==============================================================

b) For First order reaction, Initial concentration [A]0, Final concentration [A] after n number of half lives is given as,

[A]= [A]0 /2n.

For N2O5 decomposition, [A]0 = 0.400 M. [A] = ?, number of half-lives n = 4.

Using above formula,

[A] = 0.400 / 24.

[A] = 0.400 / 16

[A] = 0.025 M

After 4 half-lives 0.025 M of N2O5 will left undecomposed.

====================XXXXXXXXXXXXXXXXXXXXXX==========================

Related Questions

Navigate

• Browse (All)
• Browse D
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.